# High-Sensitivity Determination of K, Ca, Na, and Mg in Salt Mines Samples by Atomic Emission Spectrometry with a Miniaturized Liquid Cathode Glow Discharge

Authors: Jie Yu; Zhichao Zhang; Quanfang Lu; Duixiong Sun; Shuwen Zhu; Xiaomin Zhang; Xing Wang; Wu Yang
Journal: Journal of Analytical Methods in Chemistry
 (2017)

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## Abstract

An atomic emission spectrometer (AES) based on a novel atmospheric pressure liquid cathode glow discharge (LCGD) as one of the most promising miniaturized excitation sources has been developed, in which the glow discharge is produced between a needle-like Pt anode and the electrolyte (as cathode) overflowing from a quartz capillary. Lower energy consumption (<50 W) and higher excitation efficiency can be realized by point discharge of the needle-like Pt. The miniaturized LCGD seems particularly well suited to rapid and high-sensitivity determination of K, Ca, Na, and Mg in salt mines samples. The optimized analytical conditions of LCGD-AES were pH = 1 with HNO3 as electrolyte, 650 V discharge voltage, and 3 mL min−1 solution flow rate. The limits of detections (LODs) of K, Ca, Na, and Mg were 0.390, 0.054, 0.048, and 0.032 mg L−1, respectively. Measurement results of the LCGD-AES are in good agreement with the comparison value obtained by inductively coupled plasma (ICP) and ion chromatography (IC). All results suggested that the developed portable analytical instrument can be used for on-site and real-time monitoring of metal elements in field with further improvement.


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## Body

## 1. Introduction

Salt mines represent a natural mineral resource because they contain many useful components, such as K, Ca, Na, and Mg. Many salt mines are exploited for raw materials used in industry, agriculture, and medicine [1]. However, before the mining and processing, we often need to determine the metal contents. Only in this way will the salt mines enjoy more potential applications. Traditional analysis tools such as AAS, ICP-AES, and ICP-MS are widely used for the determination of metal contents in a variety of real samples. However, these tools are generally confined to the laboratory and required high temperatures, high vacuum, high power input, or even inert/special gases [2, 3]. In addition, it is difficult for ICP to introduce high-salinity solutions, because the salinity load may cause signal suppression, spectral interferences, plasma instability, and even nebulizers blocking [4]. These shortcomings limit their use only in laboratory and do not meet the requirements for the field deployment or real-time monitoring [4, 5]. Therefore, it is necessary to develop a simple, convenient, and portable analytical technique.Over the past two decades, electrolyte cathode atmospheric glow discharge (ELCAD) has received a rapid development [2, 3, 6, 7]. It is considered as one of the most promising alternative miniaturized excitation sources with potential advantages of commercial and analytical success of the plasma sources (i.e., ICP), because it is more compact and is a portable instrument with lower energy consumption (<75 W) and needs no special sample introduction system like a spray chamber and a nebulizer to transport the analytes to the analytical zone [2, 3, 7]. Also, for ELCAD, the analyte is directly introduced to the plasma without the use of nebulizer, which results in reduced memory effects and avoids the problem of deposits blocking the system [4]. Therefore, it is well suited to the field deployment and on-line analysis of multielements in salt mines samples.The first use of liquid microplasma for the incorporation of the solution as a cathode for the analysis of atomic spectra was performed in 1993 by Cserfalvi et al. [6] who named this source as electrolyte cathode atmospheric glow discharge (ELCAD) [6, 8]. The main device of ELCAD is a very simple atomization/excitation source; that is, the sample solution is used as a cathode, which overflows from the pipette to the reservoir filled with the electrolyte solution and the tip of the pipette is raised by 1–3 mm to make it electrically conductive, and a counter electrode (mostly W or Pt rod) above it (2–4 mm) is the anode [2, 3, 6, 8]. Following this pioneering study, significant variations of the ELCAD design have been developed, including solution cathode glow discharge (SCGD) [9, 10], direct current atmospheric pressure glow discharge (DC-APGD) [11, 12], liquid sampling-atmospheric pressure glow discharge (LS-APGD) [13, 14], liquid electrode plasma atomic emission spectroscopy (LEP-AES) [15, 16], alternating current electrolyte atmospheric liquid discharge (AC-EALD) [17, 18], drop spark discharge (DSD) [19, 20], and liquid electrode chip discharge [21, 22]. All these indicated that miniaturized and/or portable apparatus may be the most fruitful applications of ELCAD. Besides, the detectability, discharge stability, and emission efficiency are also improved [3, 7].In recent years, closed-type ELCAD has been applied for the analysis of several real samples including water samples [18, 23], human hair and stream sediment [24], honeys [25], tuna fish and aquatic plant [26], titanium dioxide [27], zircaloys [28, 29], colloidal silica [5], and soils and spruce needles [11]. Despite these progresses, to the best of our knowledge, ELCAD type is rarely applied for the determination of metal elements in salt mines samples, perhaps because of its complicated matrix.Recently, based on the principle of ELCAD, we also successfully developed a novel liquid cathode glow discharge-atomic emission spectrometry (LCGD-AES) for the simultaneous determination of multimetal elements in water samples [30] and ores samples [31], in which the glow discharge is sustained between a needle-like Pt anode and the electrolyte (as cathode) overflowing from a quartz capillary. Compared with conventional ELCAD, the LCGD has several advantages. For example, sealed Pt wire into a quartz tube can form a Pt point discharge, which can improve the excitation efficiency and reduce the energy consumption (<66 W). In addition, the insertion of the quartz capillary into the graphite tube excludes the reservoir of ELCAD. Moreover, several knots in peristaltic pump tubing can increase the stability of discharge plasma [30, 31].In this work, in order to further evaluate the feasibility of the method, simultaneous determination of K, Ca, Na, and Mg in salt mines samples was carried out by LCGD-AES. The stability of LCGD and effects of operation parameters, such as discharge voltage, solution flow rate, supporting electrolyte, solution pH, and interfering substance on emission intensity, were investigated in detail. Moreover, the measurement results of the LCGD-AES were compared with inductively coupled plasma (ICP) and ion chromatography (IC).


## 2. Experimental

### 2.1. Apparatus

The schematic diagram of the experimental device for miniaturized LCGD-AES is similar to our previous work [30, 31] and is presented in Figure 1. It contains a DC high voltage power supply, sample introduction, glow discharge system, and spectral detection. The DC high voltage source was a DH 1722-6 power supply (Beijing Dahua Radio Factory, Beijing, China) providing the voltage of 0–1000 V and the current of 0–0.5 A.Figure 1
Schematic diagram of the experiment setup.The sample solution was pumped into the LCGD system through a quartz capillary (1.0 mm inner diameter and 1.2 mm outer diameter) with the aid of a peristaltic pump (YZ1515X, Beijing Dongnan Yicheng Laboratory Equipment Co., Ltd.). To reduce signal fluctuations of discharge induced by the peristaltic pump, several knots were tied in the peristaltic pump tubing.The excitation source system consists of two parts: a pointed Pt wire (diameter: 0.5 mm) called the anode was sealed into a conical quartz tube and positioned 1.0 mm above the top of quartz to form a needle-like Pt tip discharge that results in a higher excitation efficiency, while the sample solution was introduced through the quartz capillary and flowed over the top of the capillary into the grooves on the graphite tube, which in turn was served as the liquid cathode. The vertical distance between capillary and pointed Pt wire is 2 mm. The capillary was inserted into a graphite tube (1.2 mm inner diameter and 5.0 mm outer diameter) and protruded from the graphite tube about 2.5 mm. The graphite tube was fixed on the plug of waste reservoir. The solution overflowing from the top of the quartz capillary was flowed into the waste reservoir through many grooves on the graphite tube. The excitation source system was installed on a manual precision translation stage with three orthogonal micrometer screw gauges, which could be controlled precisely in thex, y, and z directions to adjust position of the glow plasma, obtain the maximum signal output, and focus the glow image into the entrance slit of monochromator (Omni-λ500, Zolix Instruments Co., Ltd.) with a 1800 grooves/mm holographic grating.The emission spectrometry of glow discharge was imaged with a quartz lens (diameter: 5 cm; focal length: 10 cm) into the vertical adjustable entrance slit of the monochromator. A PMTH-S1-CR131 photomultiplier (PMT) running at −1000 V was used as the detector. Monochromator control and data acquisition were performed with the ZolixScan Basic V4 based software integral to the Omni-λ500. Spectral resolution of the monochromator was 0.05 nm, and integration time was set as 100 ms for each measurement at 0.1 nm intervals.


### 2.2. Reagents and Samples

HNO3, HCl, and H2SO4 were of superior reagent grade and were supplied by Sinopharm Chemical Reagent Co., Ltd. (Ningbo, China). 1000 mg L−1 stock standards of K, Ca, Na, and Mg were obtained from the National Research Center for Certified Reference Materials (Beijing, China). Background electrolyte was adjusted to pH = 1 with HNO3. Working standard solutions were prepared by appropriate dilution from the corresponding stock solutions and then adjusted to pH = 1.0 with HNO3. The pH of the solutions was measured with a pH meter (PHS-3E, INESA, China). Deionized water (18.25 MΩ cm) purified using a water purification system (Sanshen Medical Devices Co., Ltd., Shanghai, China) was used for the preparation of all working solutions.Four preprocessed salt mines (denoted as A, B, C, and D) were supplied by Qinghai Salt Lake Potash Fertilizer Co., Ltd (Geermu, China). All samples treatment procedures were as follows: each real sample was weighed accurately 0.500 g and then dissolved, transferred into a 100 mL volumetric flask and adjusted to pH = 1.0 with HNO3, and then separated by high-speed centrifuge at 10000 r min−1 to obtain measured solution samples. After that, the contents of Ca, Na, and Mg in the solution samples were directly determined by LCGD-AES, ICP-AES, and IC. In addition, each solution sample (1 mL) was diluted 100 times with pH = 1.0 HNO3 solution to determine the content of K because the concentration of K in solution sample is much higher than that of Ca, Na, and Mg. All data points represent the average values from the 10 successive measurements.


## 2.1. Apparatus

The schematic diagram of the experimental device for miniaturized LCGD-AES is similar to our previous work [30, 31] and is presented in Figure 1. It contains a DC high voltage power supply, sample introduction, glow discharge system, and spectral detection. The DC high voltage source was a DH 1722-6 power supply (Beijing Dahua Radio Factory, Beijing, China) providing the voltage of 0–1000 V and the current of 0–0.5 A.Figure 1
Schematic diagram of the experiment setup.The sample solution was pumped into the LCGD system through a quartz capillary (1.0 mm inner diameter and 1.2 mm outer diameter) with the aid of a peristaltic pump (YZ1515X, Beijing Dongnan Yicheng Laboratory Equipment Co., Ltd.). To reduce signal fluctuations of discharge induced by the peristaltic pump, several knots were tied in the peristaltic pump tubing.The excitation source system consists of two parts: a pointed Pt wire (diameter: 0.5 mm) called the anode was sealed into a conical quartz tube and positioned 1.0 mm above the top of quartz to form a needle-like Pt tip discharge that results in a higher excitation efficiency, while the sample solution was introduced through the quartz capillary and flowed over the top of the capillary into the grooves on the graphite tube, which in turn was served as the liquid cathode. The vertical distance between capillary and pointed Pt wire is 2 mm. The capillary was inserted into a graphite tube (1.2 mm inner diameter and 5.0 mm outer diameter) and protruded from the graphite tube about 2.5 mm. The graphite tube was fixed on the plug of waste reservoir. The solution overflowing from the top of the quartz capillary was flowed into the waste reservoir through many grooves on the graphite tube. The excitation source system was installed on a manual precision translation stage with three orthogonal micrometer screw gauges, which could be controlled precisely in thex, y, and z directions to adjust position of the glow plasma, obtain the maximum signal output, and focus the glow image into the entrance slit of monochromator (Omni-λ500, Zolix Instruments Co., Ltd.) with a 1800 grooves/mm holographic grating.The emission spectrometry of glow discharge was imaged with a quartz lens (diameter: 5 cm; focal length: 10 cm) into the vertical adjustable entrance slit of the monochromator. A PMTH-S1-CR131 photomultiplier (PMT) running at −1000 V was used as the detector. Monochromator control and data acquisition were performed with the ZolixScan Basic V4 based software integral to the Omni-λ500. Spectral resolution of the monochromator was 0.05 nm, and integration time was set as 100 ms for each measurement at 0.1 nm intervals.


## 2.2. Reagents and Samples

HNO3, HCl, and H2SO4 were of superior reagent grade and were supplied by Sinopharm Chemical Reagent Co., Ltd. (Ningbo, China). 1000 mg L−1 stock standards of K, Ca, Na, and Mg were obtained from the National Research Center for Certified Reference Materials (Beijing, China). Background electrolyte was adjusted to pH = 1 with HNO3. Working standard solutions were prepared by appropriate dilution from the corresponding stock solutions and then adjusted to pH = 1.0 with HNO3. The pH of the solutions was measured with a pH meter (PHS-3E, INESA, China). Deionized water (18.25 MΩ cm) purified using a water purification system (Sanshen Medical Devices Co., Ltd., Shanghai, China) was used for the preparation of all working solutions.Four preprocessed salt mines (denoted as A, B, C, and D) were supplied by Qinghai Salt Lake Potash Fertilizer Co., Ltd (Geermu, China). All samples treatment procedures were as follows: each real sample was weighed accurately 0.500 g and then dissolved, transferred into a 100 mL volumetric flask and adjusted to pH = 1.0 with HNO3, and then separated by high-speed centrifuge at 10000 r min−1 to obtain measured solution samples. After that, the contents of Ca, Na, and Mg in the solution samples were directly determined by LCGD-AES, ICP-AES, and IC. In addition, each solution sample (1 mL) was diluted 100 times with pH = 1.0 HNO3 solution to determine the content of K because the concentration of K in solution sample is much higher than that of Ca, Na, and Mg. All data points represent the average values from the 10 successive measurements.


## 3. Results and Discussion

### 3.1. Emission Spectra of the LCGD-AES

In order to verify the feasibility of this method, the blank solution (pH = 1.0 HNO3) (a) and 50 mg L−1 mixed solution of K, Ca, Na, and Mg (adjusted to pH = 1.0 with HNO3) (b) were introduced into the LCGD-AES. Figure 2 shows the typical emission spectra between 200 and 800 nm. As shown in Figure 2(a), the bands in the wavelength from 262.0 to 309.0 nm are attributed to the emission of OH (A2Σ+→X2Π) [32, 33]. Molecular band spectra of N2 ranging from 315 to 406 nm and ascribed to the C3Πu→B3Πg systems are observed in emission spectra because the discharge is carried out in ambient air. In addition, a series of O II lines are distributed from 410.0 to 470.1 nm, which are produced from water vapor by electron impact. Moreover, the atomic lines of Hα and Hβ are at 656.3 and 486.1 nm, which come from the electrolyte around the cathode that is bombarded by the high energy electrons [30, 31]. Spectral lines of Na I also appear at 589.0 and 589.6 nm, which suggests that the blank sample still contains a small amount of impurities.Figure 2
Typical LCGD-AES spectrum of the pH = 1.0 HNO3 blank solution (a) and 50 mg L−1 K, Ca, Na, and Mg mixture solution adjusted to pH = 1 with HNO3 (b) (discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).
(a)
Blank solution
(b)
Mixed solution of K, Ca, Na, and MgHowever, when we added K, Ca, Na, and Mg to the blank solution (shown Figure2(b)), the new lines of K I, Ca I, Na I, and Mg I were observed at 766.5 or 770.1 nm, 422.7 nm, 589.0 nm or 589.6 nm, and 285.2 nm, respectively. As can be seen from Figure 2(b), K I 766.5 nm is stronger than 770.1 nm and Na I 589.0 nm is stronger than 589.6 nm. What is more, all lines are clearly isolated from the blank emission spectra. Therefore, the lines of 766.5, 422.7, 589.0, and 285.2 nm are selected as analytical lines of K I, Ca I, Na I, and Mg I, respectively. All these results indicated that it is viable to use LCGD-AES for simultaneous qualitative identification of K, Ca, Na, and Mg in salt mines.


### 3.2. Optimization of the Experimental Conditions

#### 3.2.1. Effect of Discharge Voltage on Emission Intensity

With the solution flow rate maintained at 3 mL min−1, the effect of discharge voltage on emission intensity was studied. The emission intensity increased significantly with increasing the discharge voltage from 610 to 680 V, as shown in Figure 3. When the discharge voltage is more than 680 V, the Pt cathode turns red and the samples start to boil, which impacts the detection accuracy [30]. A higher voltage also damages the quartz capillary and causes the discharge to become unstable [18]. Therefore, the 650 V is chosen as the optimal discharge voltage in this study.Figure 3
Effect of discharge voltage on emission intensity (concentration: 5 mg L−1 adjusted to pH = 1.0 with HNO3, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).Under the fixed wavelength at 766.5 nm, the emission intensity of K I was taken as a function of time to test the stability of discharge. Figure4 shows the temporal tracing of the emission intensity of 5 mg L−1 K solution in different voltages about 5 min after the plasma was stabilized for about 2 min. It is found that the emission intensity is increased with increasing the discharge voltage from 610 to 680 V. However, over 660 V, the increasing voltage will cause fluctuation of the emission intensities because of unstable discharge plasma [30, 31]. Because the emission intensity and stability of discharge are moderate at 650 V, the 650 V discharge voltage was adopted in subsequent studies.Figure 4
Stability of emission intensity as a function of time of LCGD (electrolytes: 5 mg L−1 K solution adjusted to pH = 1.0 with HNO3, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


#### 3.2.2. Effect of Solution Flow Rate on Emission Intensity

The effect of solution flow rate on emission intensity was also evaluated in the range of 2.5–5.5 mL min−1. As shown in Figure 5, the emission intensity of K is increased with flow rate from 2.5 to 5.5 mL min−1, but the emission intensities of Ca, Na, and Mg are increased from 2.5 to 3.0 mL min−1 and then declined after further increasing the flow rate from 3.0 to 5.5 mL min−1. The increase of the emission intensity with the increase of flow rate at lower range may be ascribed to the raised amounts of analytes which entered the discharge [17]. The reduction of emission intensity at higher flow rate may be a consequence of additional water vaporization which may reduce the energy or number of electrons available for exciting the atoms [18]. What is more, increasing the water at higher flow rates might also cool the plasma [34]. Based on these results, 3.0 mL min−1 was selected as the optimal solution flow rate.Figure 5
Effect of solution flow rate on emission intensity (electrolytes: 5 mg L−1 K, Ca, Na, and Mg solution adjusted to pH = 1.0 with HNO3, discharge voltage: 650 V, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


#### 3.2.3. Effect of the Supporting Electrolyte on Emission Intensity

Mezei et al. [35] found in the ELCAD system that using acids as the electrolyte results in stronger emission than using salts and that the acid anions also affect the emission intensity. Therefore, the effect of the different supporting electrolyte (adjusted to pH = 1.0 with HNO3, HCl, and H2SO4, resp.) on the emission intensity of 5 mg L−1 K, Ca, Na, and Mg solutions was investigated. As shown in Figure 6, the net intensities of K, Ca, Na, and Mg are all affected by the acid anions. It was found that the emission intensity follows the order NO3- > Cl- > SO42-. It suggested that HNO3 exhibits higher emission intensities for K, Ca, Na, and Mg. This result is consistent with what was reported by Mezei et al. [2, 35] and Webb et al. [36]. When the size of the anion is increased, the conductivity of the ions in electrolyte will be reduced, and then the current and power are to become lower [34]. As the size of NO3- is close to Cl-, the change of emission intensity is not obvious (ionic radii of NO3-, Cl-, and SO42- are 165, 181, and 244 pm, resp.). As the size of SO42- is larger than that of Cl- and NO3-, the lower emission intensity is observed. What is more, HCl and H2SO4 are easy to generate precipitation with several metal ions [30, 31]. In addition, HNO3 has good sensitivity and chemical compatibility [34]. Therefore, we chose HNO3 as supporting electrolyte mediums for subsequent experiments.Figure 6
Effect of the supporting electrolyte (electrolytes: 5 mg L−1 K, Ca, Na, and Mg solution adjusted to pH = 1.0 by support acid, discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


#### 3.2.4. The Effect of the Solution pH on Emission Intensity

As we all know, the emission intensity was dependent on the solution pH in ELCAD [6] and AC-EALD [17, 18]. Thus, the effect of the solution pH was also optimized in the present study. It was found that when the pH was lower than 0.8, the glow is very violent and the emission intensity is prone to fluctuation due to the higher conductivity and higher energy. In addition, the Pt and quartz capillary would be destroyed when the pH was below 0.8. However, when the pH is above 1.6, the emission intensity could not be ascertained clearly because of the lower conductivity and weaker glow [30, 31]. Therefore, the effect of solution pH on element emission intensity was studied in the pH range of 0.8–1.6. As shown in Figure 7, the emission intensities were decreased from pH 0.8 to 1.6. By taking into account the emission efficiency, discharge stability, and detectability, we selected pH = 1.0 as the optimum solution pH.Figure 7
The effect of the solution pH on emission intensity (electrolytes: 5 mg L−1 K, Ca, Na, and Mg solution, discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


#### 3.2.5. Effect of Interfering Substance on Emission Intensity

To evaluate the sensitivity of LCGD to the matrix-induced interferences in the analysis of samples, the effects of organic additives (methanol, ethanol, formic acid, and acetic acid) and inorganic metals (K, Ca, Na, and Mg) on the emission intensity were studied, respectively. The potential interfering substances were added separately (3%, volume ratio), methanol, ethanol, formic acid and acetic acid, and 50-fold K, Ca, Na, and Mg, to the single-element working standard solutions at 5 mg L−1 with pH = 1.0 HNO3. Figure 8 shows the change of emission intensity with and without foreign substances. It was found that the emission intensities of K and Ca decreased significantly with the addition of foreign substances. However, in the case of the measurements of Na, no remarkable interferences from any foreign substances were observed. It could be observed that the inorganic salt (Ca) could enhance the emission intensity of Mg, but other interfering substances will reduce the emission intensity. Unfortunately, it is difficult to judge the cause of this type of interference. Certainly, this is related to a complex and unexplained mechanism for the release of the analytes from the surface of the flow solution [23].Figure 8
Mutual interference and the influence of organic matter (5 mg L−1 K, Ca, Na, and Mg solution adjusted to pH = 1.0 with HNO3, discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm, added to 3% (volume ratio) methanol, ethanol, formic acid, and acetic acid and 50-fold K, Ca, Na, and Mg).


### 3.3. Analytical Performance

The analytical performance of LCGD-AES was evaluated under optimal operating parameters (supporting electrolytes: adjusted to pH = 1.0 with HNO3, discharge voltage: 650 V, flow rate: 3 mL min−1, and interelectrode gap: 2 mm). Standard solutions of K, Ca, Na, and Mg ranging from 1 to 10 mg L−1 were prepared and established calibration curves. The results showed that all calibration curves have a good linear relationship. The linear equation, LODs, sensitivity, R2, and RSD are listed in Table 1. It is obvious that R2 and the RSD ranged from 0.9822 to 0.9981 and from 0.26% to 6.83%, respectively. The LODs of K, Ca, Na, and Mg are 0.390, 0.054, 0.048, and 0.032 mg L−1, respectively. The power consumption is 39–47 W. The results suggested that determination of K, Ca, Na, and Mg by using LCGD-AES has high sensitivity and precision and low LOD and power consumption. So it can be employed for quantitative determination of metal elements in salt mines.Table 1
Analytical performance of LCGD-AES for K, Ca, Na, and Mg solution.
Analyte
Analytical line (nm)
Power (W)
Calibration equation
R
2
Sensitivity
LOD (mg L−1)
R
S
D
∗  (%)
K
766.5
40.3–46.8
I = 21821 + 233931C
0.9981
233931
0.390
0.26
Ca
422.7
41.6–46.2
I = 4236 + 81256C
0.9973
81256
0.054
6.83
Na
589.0
39.3–44.2
I = 3182790 + 1473620C
0.9822
1473620
0.048
0.28
Mg
285.2
40.3–46.8
I = 589022 + 1846380C
0.9918
1846380
0.032
2.83
∗Standard concentration: 5 mg L−1, n= 10.A comparison of the LODs obtained by other ELCAD-type [8–14] is listed in Table 2. Obviously, the LODs for LCGD are found to be comparable to those of similar ELCAD systems.Table 2
Comparison of the LODs obtained by LCGD-AES system with other ELCAD-AES systems for the detection of K, Ca, Na, and Mg.
Methods
LOD (mg L−1)
Reference
K
Ca
Na
Mg
LCGD-AES
0.390
0.054
0.048
0.032
This work
ELCAD
0.200
0.400
0.060
0.800
[8]
Earlier
0.013
0.023
0.0008
0.019
[9]
SCGD
0.0006
0.45
0.0005
0.340
[10]
DC-APGD
0.004
0.36
0.002
0.1
[11]
DC-APGD
0.007
0.150
0.003
0.030
[12]
APGD
0.004
0.09
0.002
0.04
[13]
APGD
0.00085
0.25
0.00023
0.015
[14]


### 3.4. Analysis of the Real Sample

To validate the proposed method, salt mines samples (A, B, C, and D) were applied for the determination of K, Ca, Na, and Mg. The recovery of samples was carried out to verify the accuracy using the standard addition method. In addition, the measurement results of samples obtained by LCGD-AES were also compared with ICP-AES and IC. The measurement results of LCGD, ICP, and IC are listed in Table3. As shown in Table 3, the measurement results of real samples by using LCGD-AES are in agreement with the comparative values obtained by ICP-AES and IC. Moreover, the recoveries of K, Ca, Na, and Mg by LCGD-AES ranged from 84.05% to 115.94%. All these indicated that the measurement results of LCGD-AES are reliable and accurate.Table 3
Measurement results of K, Ca, Na, and Mg in real salt mines by LCGD-AES, ICP, and IC.
Sample
Element
This work (mg g−1)
ICP (mg g−1)
IC (mg g−1)
R
e
c
o
v
e
r
y
a (%)
A
K
599.08 ± 16.55
—
479.20 ± 8.23
107.86
Ca
0.28 ± 0.04
0.23 ± 0.05
0.31 ± 0.01
84.05
Na
5.34 ± 1.04
—
3.25 ± 0.03
90.63
Mg
2.34 ± 0.30
2.66 ± 0.03
2.13 ± 0.05
106.92
B
K
577.93 ± 10.56
—
466.08 ± 5.14
115.94
Ca
0.33 ± 0.03
0.84 ± 0.05
0.37 ± 0.01
87.16
Na
4.55 ± 1.10
—
3.60 ± 0.05
98.76
Mg
2.97 ± 0.13
3.14 ± 0.05
2.84 ± 0.03
103.04
C
K
641.35 ± 21.78
—
488.18 ± 8.56
112.69
Ca
0.32 ± 0.01
0.31 ± 0.01
0.37 ± 0.01
88.37
Na
5.06 ± 1.12
—
4.79 ± 0.05
91.83
Mg
2.71 ± 0.20
3.62 ± 0.07
3.53 ± 0.05
104.02
D
K
641.52 ± 10.42
—
485.82 ± 6.42
109.19
Ca
0.25 ± 0.04
0.30 ± 0.03
0.28 ± 0.01
94.03
Na
5.22 ± 1.13
—
4.24 ± 0.05
94.63
Mg
3.33 ± 0.28
4.50 ± 0.05
4.03 ± 0.03
106.32
A
d
d
e
d
a standard concentration: 5 mg L−1, n = 10.The statisticalt-test is widely used for estimating the concordance of an analytical method [37, 38]. Thet-test method calculates p value to find the statistical significance of the test within a specified confidence interval by initially assuming that the means of both groups are identical. Values of p<0.05 (with a confidence interval of 95%) indicate that the groups’ means are different. Otherwise p attains a value > 0.05, indicating that both groups have identical means [38, 39]. The statistical results between LCGD-AES and IC were listed in Table 4. As can be seen from Table 4, all values of t do not go over t95% = 2.78 (t-test for a confidence level of 95%) except for K measurement in all samples, Ca measurement in sample B, and Mg measurement in samples C and D. In addition, most ofp values (significant level) are higher than 0.05 (Table 4). This is because K ions concentrations in the samples are very high and dilution can lead to the larger errors. That is to say, some results are in good agreement with thet-test for a confidence level of 95%. All results indicated that there is no significant difference between the two methods and suggested that the measurement results using LCGD-AES are roughly reliable and both the techniques are in agreement with each other. Therefore, the developed LCGD-AES has the potential to be applied for the determination of metal in complex salt mines samples.Table 4
t-test and p values between the analytical results obtained by LCGD-AES and IC.
Elements
Sample
A
B
C
D
t (p) values
K
40.90 (9.7×10-10)a
443.57 (1.9×10-7)a
15.73 (1.3×10-5)a
832.08 (6.4×10-7)a
Ca
1.71 (0.09)
3.22 (0.02)a
1.77 (0.62)
1.52 (0.10)
Na
2.28 (0.23)
1.01 (0.15)
0.29 (0.11)
1.03 (0.25)
Mg
1.61 (0.05)
2.22 (0.11)
9.26 (0.01)a
5.55 (0.01)a
T
h
e
a values of t95%> 2.78 (with a confidence interval of 95%) and p<0.05 indicated that there was a significant difference between IC and LCGD-AES.


## 3.1. Emission Spectra of the LCGD-AES

In order to verify the feasibility of this method, the blank solution (pH = 1.0 HNO3) (a) and 50 mg L−1 mixed solution of K, Ca, Na, and Mg (adjusted to pH = 1.0 with HNO3) (b) were introduced into the LCGD-AES. Figure 2 shows the typical emission spectra between 200 and 800 nm. As shown in Figure 2(a), the bands in the wavelength from 262.0 to 309.0 nm are attributed to the emission of OH (A2Σ+→X2Π) [32, 33]. Molecular band spectra of N2 ranging from 315 to 406 nm and ascribed to the C3Πu→B3Πg systems are observed in emission spectra because the discharge is carried out in ambient air. In addition, a series of O II lines are distributed from 410.0 to 470.1 nm, which are produced from water vapor by electron impact. Moreover, the atomic lines of Hα and Hβ are at 656.3 and 486.1 nm, which come from the electrolyte around the cathode that is bombarded by the high energy electrons [30, 31]. Spectral lines of Na I also appear at 589.0 and 589.6 nm, which suggests that the blank sample still contains a small amount of impurities.Figure 2
Typical LCGD-AES spectrum of the pH = 1.0 HNO3 blank solution (a) and 50 mg L−1 K, Ca, Na, and Mg mixture solution adjusted to pH = 1 with HNO3 (b) (discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).
(a)
Blank solution
(b)
Mixed solution of K, Ca, Na, and MgHowever, when we added K, Ca, Na, and Mg to the blank solution (shown Figure2(b)), the new lines of K I, Ca I, Na I, and Mg I were observed at 766.5 or 770.1 nm, 422.7 nm, 589.0 nm or 589.6 nm, and 285.2 nm, respectively. As can be seen from Figure 2(b), K I 766.5 nm is stronger than 770.1 nm and Na I 589.0 nm is stronger than 589.6 nm. What is more, all lines are clearly isolated from the blank emission spectra. Therefore, the lines of 766.5, 422.7, 589.0, and 285.2 nm are selected as analytical lines of K I, Ca I, Na I, and Mg I, respectively. All these results indicated that it is viable to use LCGD-AES for simultaneous qualitative identification of K, Ca, Na, and Mg in salt mines.


## 3.2. Optimization of the Experimental Conditions

### 3.2.1. Effect of Discharge Voltage on Emission Intensity

With the solution flow rate maintained at 3 mL min−1, the effect of discharge voltage on emission intensity was studied. The emission intensity increased significantly with increasing the discharge voltage from 610 to 680 V, as shown in Figure 3. When the discharge voltage is more than 680 V, the Pt cathode turns red and the samples start to boil, which impacts the detection accuracy [30]. A higher voltage also damages the quartz capillary and causes the discharge to become unstable [18]. Therefore, the 650 V is chosen as the optimal discharge voltage in this study.Figure 3
Effect of discharge voltage on emission intensity (concentration: 5 mg L−1 adjusted to pH = 1.0 with HNO3, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).Under the fixed wavelength at 766.5 nm, the emission intensity of K I was taken as a function of time to test the stability of discharge. Figure4 shows the temporal tracing of the emission intensity of 5 mg L−1 K solution in different voltages about 5 min after the plasma was stabilized for about 2 min. It is found that the emission intensity is increased with increasing the discharge voltage from 610 to 680 V. However, over 660 V, the increasing voltage will cause fluctuation of the emission intensities because of unstable discharge plasma [30, 31]. Because the emission intensity and stability of discharge are moderate at 650 V, the 650 V discharge voltage was adopted in subsequent studies.Figure 4
Stability of emission intensity as a function of time of LCGD (electrolytes: 5 mg L−1 K solution adjusted to pH = 1.0 with HNO3, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


### 3.2.2. Effect of Solution Flow Rate on Emission Intensity

The effect of solution flow rate on emission intensity was also evaluated in the range of 2.5–5.5 mL min−1. As shown in Figure 5, the emission intensity of K is increased with flow rate from 2.5 to 5.5 mL min−1, but the emission intensities of Ca, Na, and Mg are increased from 2.5 to 3.0 mL min−1 and then declined after further increasing the flow rate from 3.0 to 5.5 mL min−1. The increase of the emission intensity with the increase of flow rate at lower range may be ascribed to the raised amounts of analytes which entered the discharge [17]. The reduction of emission intensity at higher flow rate may be a consequence of additional water vaporization which may reduce the energy or number of electrons available for exciting the atoms [18]. What is more, increasing the water at higher flow rates might also cool the plasma [34]. Based on these results, 3.0 mL min−1 was selected as the optimal solution flow rate.Figure 5
Effect of solution flow rate on emission intensity (electrolytes: 5 mg L−1 K, Ca, Na, and Mg solution adjusted to pH = 1.0 with HNO3, discharge voltage: 650 V, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


### 3.2.3. Effect of the Supporting Electrolyte on Emission Intensity

Mezei et al. [35] found in the ELCAD system that using acids as the electrolyte results in stronger emission than using salts and that the acid anions also affect the emission intensity. Therefore, the effect of the different supporting electrolyte (adjusted to pH = 1.0 with HNO3, HCl, and H2SO4, resp.) on the emission intensity of 5 mg L−1 K, Ca, Na, and Mg solutions was investigated. As shown in Figure 6, the net intensities of K, Ca, Na, and Mg are all affected by the acid anions. It was found that the emission intensity follows the order NO3- > Cl- > SO42-. It suggested that HNO3 exhibits higher emission intensities for K, Ca, Na, and Mg. This result is consistent with what was reported by Mezei et al. [2, 35] and Webb et al. [36]. When the size of the anion is increased, the conductivity of the ions in electrolyte will be reduced, and then the current and power are to become lower [34]. As the size of NO3- is close to Cl-, the change of emission intensity is not obvious (ionic radii of NO3-, Cl-, and SO42- are 165, 181, and 244 pm, resp.). As the size of SO42- is larger than that of Cl- and NO3-, the lower emission intensity is observed. What is more, HCl and H2SO4 are easy to generate precipitation with several metal ions [30, 31]. In addition, HNO3 has good sensitivity and chemical compatibility [34]. Therefore, we chose HNO3 as supporting electrolyte mediums for subsequent experiments.Figure 6
Effect of the supporting electrolyte (electrolytes: 5 mg L−1 K, Ca, Na, and Mg solution adjusted to pH = 1.0 by support acid, discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


### 3.2.4. The Effect of the Solution pH on Emission Intensity

As we all know, the emission intensity was dependent on the solution pH in ELCAD [6] and AC-EALD [17, 18]. Thus, the effect of the solution pH was also optimized in the present study. It was found that when the pH was lower than 0.8, the glow is very violent and the emission intensity is prone to fluctuation due to the higher conductivity and higher energy. In addition, the Pt and quartz capillary would be destroyed when the pH was below 0.8. However, when the pH is above 1.6, the emission intensity could not be ascertained clearly because of the lower conductivity and weaker glow [30, 31]. Therefore, the effect of solution pH on element emission intensity was studied in the pH range of 0.8–1.6. As shown in Figure 7, the emission intensities were decreased from pH 0.8 to 1.6. By taking into account the emission efficiency, discharge stability, and detectability, we selected pH = 1.0 as the optimum solution pH.Figure 7
The effect of the solution pH on emission intensity (electrolytes: 5 mg L−1 K, Ca, Na, and Mg solution, discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


### 3.2.5. Effect of Interfering Substance on Emission Intensity

To evaluate the sensitivity of LCGD to the matrix-induced interferences in the analysis of samples, the effects of organic additives (methanol, ethanol, formic acid, and acetic acid) and inorganic metals (K, Ca, Na, and Mg) on the emission intensity were studied, respectively. The potential interfering substances were added separately (3%, volume ratio), methanol, ethanol, formic acid and acetic acid, and 50-fold K, Ca, Na, and Mg, to the single-element working standard solutions at 5 mg L−1 with pH = 1.0 HNO3. Figure 8 shows the change of emission intensity with and without foreign substances. It was found that the emission intensities of K and Ca decreased significantly with the addition of foreign substances. However, in the case of the measurements of Na, no remarkable interferences from any foreign substances were observed. It could be observed that the inorganic salt (Ca) could enhance the emission intensity of Mg, but other interfering substances will reduce the emission intensity. Unfortunately, it is difficult to judge the cause of this type of interference. Certainly, this is related to a complex and unexplained mechanism for the release of the analytes from the surface of the flow solution [23].Figure 8
Mutual interference and the influence of organic matter (5 mg L−1 K, Ca, Na, and Mg solution adjusted to pH = 1.0 with HNO3, discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm, added to 3% (volume ratio) methanol, ethanol, formic acid, and acetic acid and 50-fold K, Ca, Na, and Mg).


## 3.2.1. Effect of Discharge Voltage on Emission Intensity

With the solution flow rate maintained at 3 mL min−1, the effect of discharge voltage on emission intensity was studied. The emission intensity increased significantly with increasing the discharge voltage from 610 to 680 V, as shown in Figure 3. When the discharge voltage is more than 680 V, the Pt cathode turns red and the samples start to boil, which impacts the detection accuracy [30]. A higher voltage also damages the quartz capillary and causes the discharge to become unstable [18]. Therefore, the 650 V is chosen as the optimal discharge voltage in this study.Figure 3
Effect of discharge voltage on emission intensity (concentration: 5 mg L−1 adjusted to pH = 1.0 with HNO3, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).Under the fixed wavelength at 766.5 nm, the emission intensity of K I was taken as a function of time to test the stability of discharge. Figure4 shows the temporal tracing of the emission intensity of 5 mg L−1 K solution in different voltages about 5 min after the plasma was stabilized for about 2 min. It is found that the emission intensity is increased with increasing the discharge voltage from 610 to 680 V. However, over 660 V, the increasing voltage will cause fluctuation of the emission intensities because of unstable discharge plasma [30, 31]. Because the emission intensity and stability of discharge are moderate at 650 V, the 650 V discharge voltage was adopted in subsequent studies.Figure 4
Stability of emission intensity as a function of time of LCGD (electrolytes: 5 mg L−1 K solution adjusted to pH = 1.0 with HNO3, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


## 3.2.2. Effect of Solution Flow Rate on Emission Intensity

The effect of solution flow rate on emission intensity was also evaluated in the range of 2.5–5.5 mL min−1. As shown in Figure 5, the emission intensity of K is increased with flow rate from 2.5 to 5.5 mL min−1, but the emission intensities of Ca, Na, and Mg are increased from 2.5 to 3.0 mL min−1 and then declined after further increasing the flow rate from 3.0 to 5.5 mL min−1. The increase of the emission intensity with the increase of flow rate at lower range may be ascribed to the raised amounts of analytes which entered the discharge [17]. The reduction of emission intensity at higher flow rate may be a consequence of additional water vaporization which may reduce the energy or number of electrons available for exciting the atoms [18]. What is more, increasing the water at higher flow rates might also cool the plasma [34]. Based on these results, 3.0 mL min−1 was selected as the optimal solution flow rate.Figure 5
Effect of solution flow rate on emission intensity (electrolytes: 5 mg L−1 K, Ca, Na, and Mg solution adjusted to pH = 1.0 with HNO3, discharge voltage: 650 V, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


## 3.2.3. Effect of the Supporting Electrolyte on Emission Intensity

Mezei et al. [35] found in the ELCAD system that using acids as the electrolyte results in stronger emission than using salts and that the acid anions also affect the emission intensity. Therefore, the effect of the different supporting electrolyte (adjusted to pH = 1.0 with HNO3, HCl, and H2SO4, resp.) on the emission intensity of 5 mg L−1 K, Ca, Na, and Mg solutions was investigated. As shown in Figure 6, the net intensities of K, Ca, Na, and Mg are all affected by the acid anions. It was found that the emission intensity follows the order NO3- > Cl- > SO42-. It suggested that HNO3 exhibits higher emission intensities for K, Ca, Na, and Mg. This result is consistent with what was reported by Mezei et al. [2, 35] and Webb et al. [36]. When the size of the anion is increased, the conductivity of the ions in electrolyte will be reduced, and then the current and power are to become lower [34]. As the size of NO3- is close to Cl-, the change of emission intensity is not obvious (ionic radii of NO3-, Cl-, and SO42- are 165, 181, and 244 pm, resp.). As the size of SO42- is larger than that of Cl- and NO3-, the lower emission intensity is observed. What is more, HCl and H2SO4 are easy to generate precipitation with several metal ions [30, 31]. In addition, HNO3 has good sensitivity and chemical compatibility [34]. Therefore, we chose HNO3 as supporting electrolyte mediums for subsequent experiments.Figure 6
Effect of the supporting electrolyte (electrolytes: 5 mg L−1 K, Ca, Na, and Mg solution adjusted to pH = 1.0 by support acid, discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


## 3.2.4. The Effect of the Solution pH on Emission Intensity

As we all know, the emission intensity was dependent on the solution pH in ELCAD [6] and AC-EALD [17, 18]. Thus, the effect of the solution pH was also optimized in the present study. It was found that when the pH was lower than 0.8, the glow is very violent and the emission intensity is prone to fluctuation due to the higher conductivity and higher energy. In addition, the Pt and quartz capillary would be destroyed when the pH was below 0.8. However, when the pH is above 1.6, the emission intensity could not be ascertained clearly because of the lower conductivity and weaker glow [30, 31]. Therefore, the effect of solution pH on element emission intensity was studied in the pH range of 0.8–1.6. As shown in Figure 7, the emission intensities were decreased from pH 0.8 to 1.6. By taking into account the emission efficiency, discharge stability, and detectability, we selected pH = 1.0 as the optimum solution pH.Figure 7
The effect of the solution pH on emission intensity (electrolytes: 5 mg L−1 K, Ca, Na, and Mg solution, discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm).


## 3.2.5. Effect of Interfering Substance on Emission Intensity

To evaluate the sensitivity of LCGD to the matrix-induced interferences in the analysis of samples, the effects of organic additives (methanol, ethanol, formic acid, and acetic acid) and inorganic metals (K, Ca, Na, and Mg) on the emission intensity were studied, respectively. The potential interfering substances were added separately (3%, volume ratio), methanol, ethanol, formic acid and acetic acid, and 50-fold K, Ca, Na, and Mg, to the single-element working standard solutions at 5 mg L−1 with pH = 1.0 HNO3. Figure 8 shows the change of emission intensity with and without foreign substances. It was found that the emission intensities of K and Ca decreased significantly with the addition of foreign substances. However, in the case of the measurements of Na, no remarkable interferences from any foreign substances were observed. It could be observed that the inorganic salt (Ca) could enhance the emission intensity of Mg, but other interfering substances will reduce the emission intensity. Unfortunately, it is difficult to judge the cause of this type of interference. Certainly, this is related to a complex and unexplained mechanism for the release of the analytes from the surface of the flow solution [23].Figure 8
Mutual interference and the influence of organic matter (5 mg L−1 K, Ca, Na, and Mg solution adjusted to pH = 1.0 with HNO3, discharge voltage: 650 V, flow rate: 3 mL min−1, interelectrode gap: 2 mm, and capillary diameter: 1 mm, added to 3% (volume ratio) methanol, ethanol, formic acid, and acetic acid and 50-fold K, Ca, Na, and Mg).


## 3.3. Analytical Performance

The analytical performance of LCGD-AES was evaluated under optimal operating parameters (supporting electrolytes: adjusted to pH = 1.0 with HNO3, discharge voltage: 650 V, flow rate: 3 mL min−1, and interelectrode gap: 2 mm). Standard solutions of K, Ca, Na, and Mg ranging from 1 to 10 mg L−1 were prepared and established calibration curves. The results showed that all calibration curves have a good linear relationship. The linear equation, LODs, sensitivity, R2, and RSD are listed in Table 1. It is obvious that R2 and the RSD ranged from 0.9822 to 0.9981 and from 0.26% to 6.83%, respectively. The LODs of K, Ca, Na, and Mg are 0.390, 0.054, 0.048, and 0.032 mg L−1, respectively. The power consumption is 39–47 W. The results suggested that determination of K, Ca, Na, and Mg by using LCGD-AES has high sensitivity and precision and low LOD and power consumption. So it can be employed for quantitative determination of metal elements in salt mines.Table 1
Analytical performance of LCGD-AES for K, Ca, Na, and Mg solution.
Analyte
Analytical line (nm)
Power (W)
Calibration equation
R
2
Sensitivity
LOD (mg L−1)
R
S
D
∗  (%)
K
766.5
40.3–46.8
I = 21821 + 233931C
0.9981
233931
0.390
0.26
Ca
422.7
41.6–46.2
I = 4236 + 81256C
0.9973
81256
0.054
6.83
Na
589.0
39.3–44.2
I = 3182790 + 1473620C
0.9822
1473620
0.048
0.28
Mg
285.2
40.3–46.8
I = 589022 + 1846380C
0.9918
1846380
0.032
2.83
∗Standard concentration: 5 mg L−1, n= 10.A comparison of the LODs obtained by other ELCAD-type [8–14] is listed in Table 2. Obviously, the LODs for LCGD are found to be comparable to those of similar ELCAD systems.Table 2
Comparison of the LODs obtained by LCGD-AES system with other ELCAD-AES systems for the detection of K, Ca, Na, and Mg.
Methods
LOD (mg L−1)
Reference
K
Ca
Na
Mg
LCGD-AES
0.390
0.054
0.048
0.032
This work
ELCAD
0.200
0.400
0.060
0.800
[8]
Earlier
0.013
0.023
0.0008
0.019
[9]
SCGD
0.0006
0.45
0.0005
0.340
[10]
DC-APGD
0.004
0.36
0.002
0.1
[11]
DC-APGD
0.007
0.150
0.003
0.030
[12]
APGD
0.004
0.09
0.002
0.04
[13]
APGD
0.00085
0.25
0.00023
0.015
[14]


## 3.4. Analysis of the Real Sample

To validate the proposed method, salt mines samples (A, B, C, and D) were applied for the determination of K, Ca, Na, and Mg. The recovery of samples was carried out to verify the accuracy using the standard addition method. In addition, the measurement results of samples obtained by LCGD-AES were also compared with ICP-AES and IC. The measurement results of LCGD, ICP, and IC are listed in Table3. As shown in Table 3, the measurement results of real samples by using LCGD-AES are in agreement with the comparative values obtained by ICP-AES and IC. Moreover, the recoveries of K, Ca, Na, and Mg by LCGD-AES ranged from 84.05% to 115.94%. All these indicated that the measurement results of LCGD-AES are reliable and accurate.Table 3
Measurement results of K, Ca, Na, and Mg in real salt mines by LCGD-AES, ICP, and IC.
Sample
Element
This work (mg g−1)
ICP (mg g−1)
IC (mg g−1)
R
e
c
o
v
e
r
y
a (%)
A
K
599.08 ± 16.55
—
479.20 ± 8.23
107.86
Ca
0.28 ± 0.04
0.23 ± 0.05
0.31 ± 0.01
84.05
Na
5.34 ± 1.04
—
3.25 ± 0.03
90.63
Mg
2.34 ± 0.30
2.66 ± 0.03
2.13 ± 0.05
106.92
B
K
577.93 ± 10.56
—
466.08 ± 5.14
115.94
Ca
0.33 ± 0.03
0.84 ± 0.05
0.37 ± 0.01
87.16
Na
4.55 ± 1.10
—
3.60 ± 0.05
98.76
Mg
2.97 ± 0.13
3.14 ± 0.05
2.84 ± 0.03
103.04
C
K
641.35 ± 21.78
—
488.18 ± 8.56
112.69
Ca
0.32 ± 0.01
0.31 ± 0.01
0.37 ± 0.01
88.37
Na
5.06 ± 1.12
—
4.79 ± 0.05
91.83
Mg
2.71 ± 0.20
3.62 ± 0.07
3.53 ± 0.05
104.02
D
K
641.52 ± 10.42
—
485.82 ± 6.42
109.19
Ca
0.25 ± 0.04
0.30 ± 0.03
0.28 ± 0.01
94.03
Na
5.22 ± 1.13
—
4.24 ± 0.05
94.63
Mg
3.33 ± 0.28
4.50 ± 0.05
4.03 ± 0.03
106.32
A
d
d
e
d
a standard concentration: 5 mg L−1, n = 10.The statisticalt-test is widely used for estimating the concordance of an analytical method [37, 38]. Thet-test method calculates p value to find the statistical significance of the test within a specified confidence interval by initially assuming that the means of both groups are identical. Values of p<0.05 (with a confidence interval of 95%) indicate that the groups’ means are different. Otherwise p attains a value > 0.05, indicating that both groups have identical means [38, 39]. The statistical results between LCGD-AES and IC were listed in Table 4. As can be seen from Table 4, all values of t do not go over t95% = 2.78 (t-test for a confidence level of 95%) except for K measurement in all samples, Ca measurement in sample B, and Mg measurement in samples C and D. In addition, most ofp values (significant level) are higher than 0.05 (Table 4). This is because K ions concentrations in the samples are very high and dilution can lead to the larger errors. That is to say, some results are in good agreement with thet-test for a confidence level of 95%. All results indicated that there is no significant difference between the two methods and suggested that the measurement results using LCGD-AES are roughly reliable and both the techniques are in agreement with each other. Therefore, the developed LCGD-AES has the potential to be applied for the determination of metal in complex salt mines samples.Table 4
t-test and p values between the analytical results obtained by LCGD-AES and IC.
Elements
Sample
A
B
C
D
t (p) values
K
40.90 (9.7×10-10)a
443.57 (1.9×10-7)a
15.73 (1.3×10-5)a
832.08 (6.4×10-7)a
Ca
1.71 (0.09)
3.22 (0.02)a
1.77 (0.62)
1.52 (0.10)
Na
2.28 (0.23)
1.01 (0.15)
0.29 (0.11)
1.03 (0.25)
Mg
1.61 (0.05)
2.22 (0.11)
9.26 (0.01)a
5.55 (0.01)a
T
h
e
a values of t95%> 2.78 (with a confidence interval of 95%) and p<0.05 indicated that there was a significant difference between IC and LCGD-AES.


## 4. Conclusions

The liquid cathode glow discharge-atomic emission spectrometry (LCGD-AES) was successfully applied for measurement of K, Ca, Na, and Mg in salt mines samples. The optimization analytical conditions of LCGD-AES were pH = 1 with HNO3 as electrolyte, 650 V voltage, and 3 mL min−1 flow rate. The power consumption is below 50 W. R2 and the RSD ranged from 0.9822 to 0.9981 and from 0.26% to 6.83%, respectively. The LODs of K, Ca, Na, and Mg were 0.390, 0.054, 0.048, 0.032 mg L−1, respectively. The recoveries of K, Ca, Na, and Mg by LCGD-AES ranged from 84.05% to 115.95%. The measurement results of LCGD-AES are very consistent with the comparative values of ICP-AES and IC. Compared with ICP-AES, LCGD-AES has some advantages, such as low power consumption, no gas requirement, low cost in setup, and easy operation and design. Moreover, it is easy in achieving real-time and on-line monitoring for samples. All the results suggested that the LCGD-AES is a very promising portable analytical instrument for highly efficient determination of metal elements in salt mines samples.



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*Source: 7105831-2017-11-07.xml*