JK-TK/Newdata huggingface dataset:
From this definition, an acid donates H+ . H+ has no electrons and neutrons .It contains only a proton. Examples I. From the equation: HCl(aq) + H2O(l) === H3O+(aq) + Cl- (aq) (a)(i)For the forward reaction from left to right, H2O gains a proton to form H3O+ and thus H2O is a proton acceptor .It is a Bronsted-Lowry base (ii) For the backward reaction from right to left, H3O+ donates a proton to form H2O and thus H3O+ is an ‘opposite’ proton donor. It is a BronstedLowry conjugate acid (b)(i)For the forward reaction from left to right, HCl donates a proton to form Cl- and thus HCl is a proton donor . It is a Bronsted-Lowry acid (ii) For the backward reaction from right to left, Cl- gains a proton to form HCl and thus Cl- is an ‘opposite’ proton acceptor. It is a Bronsted-Lowry conjugate base. Every base /acid from Bronsted-Lowry definition thus must have a conjugate product/reactant. II. From the equation: HCl(aq) + NH3(aq) === NH4+(aq) + Cl- (aq) (a)(i)For the forward reaction from left to right, NH3 gains a proton to form NH4+ and thus NH3 is a proton acceptor . It is a Bronsted-Lowry base (ii) For the backward reaction from right to left, NH4+ donates a proton to form NH3 and thus NH4+ is an ‘opposite’ proton donor. It is a Bronsted-Lowry conjugate acid (b)(i)For the forward reaction from left to right, HCl donates a proton to form Cl- and thus HCl is a proton donor . It is a Bronsted-Lowry acid (ii) For the backward reaction from right to left, Cl- gains a proton to form HCl and thus Cl- is an ‘opposite’ proton acceptor. It is a Bronsted-Lowry conjugate base. 4. Acids and bases show acidic and alkaline properties/characteristics only in water but not in other solvents e.g.
It is a Bronsted-Lowry conjugate base. 4. Acids and bases show acidic and alkaline properties/characteristics only in water but not in other solvents e.g. (a)Hydrogen chloride gas dissolves in water to form hydrochloric acid Hydrochloric acid dissociates/ionizes in water to free H+(aq)/H3O+(aq) ions. The free H3O+(aq) / H+(aq) ions are responsible for: (i)turning blue litmus paper/solution red. (ii)show pH value 1/2/3/4/5/6 (iii)are good electrolytes/conductors of electricity/undergo electrolysis. (iv)react with metals to produce /evolve hydrogen gas and a salt. i.e. Ionically: -For a monovalent metal: 2M(s) + 2H+(aq) -> 2M+(aq) + H2(g) -For a divalent metal: M(s) + 2H+(aq) -> M2+(aq) + H2(g) -For a trivalent metal: 2M(s) + 6H+(aq) -> 2M3+(aq) + 3H2(g) Examples: -For a monovalent metal: 2Na(s) + 2H+(aq) -> 2Na+(aq) + H2(g) -For a divalent metal: Ca(s) + 2H+(aq) -> Ca2+(aq) + H2(g) -For a trivalent metal: 2Al(s) + 6H+(aq) -> 2Al3+(aq) + 3H2(g) (v)react with metal carbonates and hhydrogen carbonates to produce /evolve carbon(IV)oxide gas ,water and a salt. i.e.
i.e. Ionically: -For a monovalent metal: M2O(s) + 2H+(aq) -> 2M+(aq) + H2O (l) MOH(aq) + H+(aq) -> M+(aq) + H2O (l)
-For a divalent metal: MO(s) + 2H+(aq) -> M2+(aq) + H2O (l) M(OH) 2(s) + 2H+(aq) -> M2+(aq) + 2H2O(l) -For a trivalent metal: M2O3(s) + 6H+(aq) -> 2M3+(aq) + 3H2O (l) M(OH) 3(s) + 3H+(aq) -> M3+(aq) + 3H2O(l) Examples: -For a monovalent metal: K2O(s) + 2H+(aq) -> 2K+(aq) + H2O (l) NH4OH(aq) + H+(aq) -> NH4+(aq) + H2O (l) -For a divalent metal: ZnO (s) + 2H+(aq) -> Zn2+(aq) + H2O (l) Pb(OH) 2(s) + 2H+(aq) -> Pb2+(aq) + 2H2O(l) (b)Hydrogen chloride gas dissolves in methylbenzene /benzene but does not dissociate /ionize into free ions. It exists in molecular state showing none of the above properties. (c)Ammonia gas dissolves in water to form aqueous ammonia which dissociate/ionize to free NH4+ (aq) and OH-(aq) ions. This dissociation/ionization makes aqueous ammonia to: (i)turn litmus paper/solution blue. (ii)have pH 8/9/10/11 (iii)be a good electrical conductor (iv)react with acids to form ammonium salt and water only. NH4OH(aq) + HCl(aq) -> NH4Cl(aq) + H2O(l) (d)Ammonia gas dissolves in methylbenzene/benzene /kerosene but does not dissociate into free ions therefore existing as molecules 6.
This dissociation/ionization makes aqueous ammonia to: (i)turn litmus paper/solution blue. (ii)have pH 8/9/10/11 (iii)be a good electrical conductor (iv)react with acids to form ammonium salt and water only. NH4OH(aq) + HCl(aq) -> NH4Cl(aq) + H2O(l) (d)Ammonia gas dissolves in methylbenzene/benzene /kerosene but does not dissociate into free ions therefore existing as molecules 6. Solvents are either polar or non-polar. A polar solvent is one which dissolves ionic compounds and other polar solvents. Water is polar solvent that dissolves ionic and polar substance by surrounding the free ions as below: H ð+ H ð+ O ð- H ð+ H ð+ H ð+ O ð- H ð+ H ð+ H ð+
O ð- H+ O ð- O ð- Cl - O ð- H ð+ Hð+ H ð+ O ð- H ð+ H+ H ð+ H ð+ H ð+ O ð- Beaker Cl- Cl- H+ water H+ Cl- H+ Free ions Note:Water is polar .It is made up of : Oxygen atom is partially negative and two hydrogen atoms which are partially positive. They surround the free H+ and Cl- ions. A non polar solvent is one which dissolved non-polar substances and covalent compounds. If a polar ionic compound is dissolved in non-polar solvent ,it does not ionize/dissociate into free ions as below: H-Cl H-Cl methyl benzene H-Cl H-Cl Covalent bond 7. Some acids and bases are strong while others are weak. (a)A strong acid/base is one which is fully/wholly/completely dissociated / ionized into many free H+ /OH- ions i.e. I. Strong acids exists more as free H+ ions than molecules. e.g.
I. Strong acids exists more as free H+ ions than molecules. e.g. HCl(aq) H+(aq) + Cl- (aq) (molecules) (cation) (anion) HNO3(aq) H+(aq) + NO3-(aq) (molecules) (cation) (anion) H2SO4(aq) 2H+(aq) + SO42-(aq) (molecules) (cation) (anion) II. Strong bases/alkalis exists more as free OH- ions than molecules. e.g. KOH(aq) K+(aq) + OH- (aq) (molecules) (cation) (anion) NaOH(aq) Na+(aq) + OH-(aq) (molecules) (cation) (anion) (b) A weak base/acid is one which is partially /partly dissociated /ionized in water into free OH- (aq) and H+(aq) ions. I. Weak acids exists more as molecules than as free H+ ions. e.g. CH3COOH(aq) H+(aq) + CH3COO- (aq) (molecules) (cation) (anion) H3PO4(aq) 3H+(aq) + PO43-(aq) (molecules) (cation) (anion) H2CO3(aq) 2H+(aq) + CO32-(aq) (molecules) (cation) (anion) II. Weak bases/alkalis exists more as molecules than free OH- ions. e.g. NH4OH(aq) NH4+(aq) + OH- (aq) (molecules) (cation) (anion) Ca(OH)2(aq) Ca2+(aq) + 2OH-(aq) (molecules) (cation) (anion) Mg(OH)2(aq) Mg2+(aq) + 2OH-(aq) (molecules) (cation) (anion)
8. The concentration of an acid/base/alkali is based on the number of moles of acid/bases dissolved in a decimeter(litre)of the solution. An acid/base/alkali with more acid/base/alkali in a decimeter(litre) of solution is said to be concentrated while that with less is said to be dilute. 9.
The concentration of an acid/base/alkali is based on the number of moles of acid/bases dissolved in a decimeter(litre)of the solution. An acid/base/alkali with more acid/base/alkali in a decimeter(litre) of solution is said to be concentrated while that with less is said to be dilute. 9. (a) (i)strong acids have pH 1/2/3 while weak acids have high pH 4/5/6. (ii)a neutral solution have pH 7 (iii)strong alkalis/bases have pH 12/13/14 while weak bases/alkalis have pH 11/10 /9 / 8. (b) pH is a measure of H+(aq) concentration in a solution. The higher the H+(aq)ions concentration ; -the higher the acidity -the lower the pH -the lower the concentration of OH-(aq) -the lower the alkalinity At pH 7 , a solution has equal concentration of H+(aq) and OH-(aq). Beyond pH 7,the concentration of the OH-(aq) increases as the H+(aq) ions decreases. 10.(a) When acids /bases dissolve in water, the ions present in the solution conduct electricity. The more the dissociation the higher the yield of ions and the greater the electrical conductivity of the solution. A compound that conducts electricity in an electrolyte and thus a compound showing high electrical conductivity is a strong electrolyte while a compound showing low electrical conductivity is a weak electrolyte. (b) Practically, a bright light on a bulb ,a high voltage reading from a voltmeter high ammeter reading from an ammeter, a big deflection on a galvanometer is an indicator of strong electrolyte(acid/base) and the opposite for weak electrolytes(acids/base) 11. Some compounds exhibit/show both properties of acids and bases/alkalis. A substance that reacts with both acids and bases is said to be amphotellic. The examples below show the amphotellic properties of: (a) Zinc (II)oxide(ZnO) and Zinc hydroxide(Zn(OH)2) (i)When ½ spatula full of Zinc(II)oxide is placed in a boiling tube containing 10cm3 of either 2M nitric(V)acid or 2M sodium hydroxide hydroxide solution, it dissolves on both the acid and the alkali/base to form a colourless solution.
Some compounds exhibit/show both properties of acids and bases/alkalis. A substance that reacts with both acids and bases is said to be amphotellic. The examples below show the amphotellic properties of: (a) Zinc (II)oxide(ZnO) and Zinc hydroxide(Zn(OH)2) (i)When ½ spatula full of Zinc(II)oxide is placed in a boiling tube containing 10cm3 of either 2M nitric(V)acid or 2M sodium hydroxide hydroxide solution, it dissolves on both the acid and the alkali/base to form a colourless solution. i.e. (i) when reacting with nitric(V)acid, the oxide shows basic properties by reacting with an acid to form a simple salt and water only. Basic oxide + Acid -> salt + water Examples: Chemical equation ZnO(s) + 2HNO3(aq) -> Zn(NO3) 2 (aq) + H2O(l) ZnO(s) + 2HCl(aq) -> ZnCl2 (aq) + H2O(l) ZnO(s) + H2SO4(aq) -> ZnSO4 (aq) + H2O(l) Ionic equation ZnO(s) + 2H+ (aq) -> Zn 2+ (aq) + H2O(l) (ii) when reacting with sodium hydroxide, the oxide shows acidic properties by reacting with a base to form a complex salt. Basic oxide + Base/alkali + Water -> Complex salt Examples: Chemical equation 1.When Zinc oxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxozincate(II) complex salt. ZnO(s) + 2NaOH(aq) + H2O(l) -> Na2Zn(OH) 4(aq) 2.When Zinc oxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxozincate(II) complex salt.
Basic oxide + Acid -> salt + water Examples: Chemical equation ZnO(s) + 2HNO3(aq) -> Zn(NO3) 2 (aq) + H2O(l) ZnO(s) + 2HCl(aq) -> ZnCl2 (aq) + H2O(l) ZnO(s) + H2SO4(aq) -> ZnSO4 (aq) + H2O(l) Ionic equation ZnO(s) + 2H+ (aq) -> Zn 2+ (aq) + H2O(l) (ii) when reacting with sodium hydroxide, the oxide shows acidic properties by reacting with a base to form a complex salt. Basic oxide + Base/alkali + Water -> Complex salt Examples: Chemical equation 1.When Zinc oxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxozincate(II) complex salt. ZnO(s) + 2NaOH(aq) + H2O(l) -> Na2Zn(OH) 4(aq) 2.When Zinc oxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxozincate(II) complex salt. ZnO(s) + 2KOH(aq) + H2O(l) -> K2Zn(OH) 4(aq) Ionic equation ZnO(s) + 2OH-(aq) + H2O(l) -> 2[Zn(OH) 4]2- (aq) (ii)When Zinc(II)hydroxide is placed in a boiling tube containing 10cm3 of either 2M nitric(V)acid or 2M sodium hydroxide hydroxide solution, it dissolves on both the acid and the alkali/base to form a colourless solution. i.e. (i) when reacting with nitric(V)acid, the hydroxide shows basic properties. It reacts with an acid to form a simple salt and water only.
i.e. (i) when reacting with nitric(V)acid, the hydroxide shows basic properties. It reacts with an acid to form a simple salt and water only. Basic hydroxide + Acid -> salt + water Examples: Chemical equation Zn(OH) 2 (s) + 2HNO3(aq) -> Zn(NO3) 2 (aq) + 2H2O(l)
Zn(OH) 2 (s) + 2HCl(aq) -> ZnCl2 (aq) + 2H2O(l) Zn(OH) 2 (s) + H2SO4(aq) -> ZnSO4 (aq) + 2H2O(l) Ionic equation Zn(OH) 2 (s) + 2H+ (aq) -> Zn 2+ (aq) + 2H2O(l) (ii) when reacting with sodium hydroxide, the hydroxide shows acidic properties by reacting with a base to form a complex salt. Basic hydroxide + Base/alkali -> Complex salt Examples: Chemical equation 1.When Zinc hydroxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxozincate(II) complex salt. Zn(OH) 2 (s) + 2NaOH(aq) -> Na2Zn(OH) 4(aq) 2.When Zinc hydroxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxozincate(II) complex salt. Zn(OH) 2 (s) + 2KOH(aq) -> K2Zn(OH) 4(aq) Ionic equation Zn(OH) 2 (s) + 2OH-(aq) -> 2[Zn(OH) 4]2- (aq) (b) Lead (II)oxide(PbO) and Lead(II) hydroxide (Pb(OH)2) (i)When ½ spatula full of Lead(II)oxide is placed in a boiling tube containing 10cm3 of either 2M nitric(V)acid or 2M sodium hydroxide hydroxide solution, it dissolves on both the acid and the alkali/base to form a colourless solution. i.e.
Zn(OH) 2 (s) + 2NaOH(aq) -> Na2Zn(OH) 4(aq) 2.When Zinc hydroxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxozincate(II) complex salt. Zn(OH) 2 (s) + 2KOH(aq) -> K2Zn(OH) 4(aq) Ionic equation Zn(OH) 2 (s) + 2OH-(aq) -> 2[Zn(OH) 4]2- (aq) (b) Lead (II)oxide(PbO) and Lead(II) hydroxide (Pb(OH)2) (i)When ½ spatula full of Lead(II)oxide is placed in a boiling tube containing 10cm3 of either 2M nitric(V)acid or 2M sodium hydroxide hydroxide solution, it dissolves on both the acid and the alkali/base to form a colourless solution. i.e. (i) when reacting with nitric(V)acid, the oxide shows basic properties by reacting with an acid to form a simple salt and water only. All other Lead salts are insoluble. Chemical equation PbO(s) + 2HNO3(aq) -> Pb(NO3) 2 (aq) + H2O(l) Ionic equation PbO(s) + 2H+ (aq) -> Pb 2+ (aq) + H2O(l) (ii) when reacting with sodium hydroxide, the oxide shows acidic properties by reacting with a base to form a complex salt. Chemical equation 1.When Lead(II) oxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxoplumbate(II) complex salt. PbO(s) + 2NaOH(aq) + H2O(l) -> Na2Pb(OH) 4(aq) 2.When Lead(II) oxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxoplumbate(II) complex salt.
Chemical equation PbO(s) + 2HNO3(aq) -> Pb(NO3) 2 (aq) + H2O(l) Ionic equation PbO(s) + 2H+ (aq) -> Pb 2+ (aq) + H2O(l) (ii) when reacting with sodium hydroxide, the oxide shows acidic properties by reacting with a base to form a complex salt. Chemical equation 1.When Lead(II) oxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxoplumbate(II) complex salt. PbO(s) + 2NaOH(aq) + H2O(l) -> Na2Pb(OH) 4(aq) 2.When Lead(II) oxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxoplumbate(II) complex salt. PbO(s) + 2KOH(aq) + H2O(l) -> K2Pb(OH) 4(aq) Ionic equation PbO(s) + 2OH-(aq) + H2O(l) -> 2[Pb(OH) 4]2- (aq) (ii)When Lead(II)hydroxide is placed in a boiling tube containing 10cm3 of either 2M nitric(V)acid or 2M sodium hydroxide hydroxide solution, it dissolves on both the acid and the alkali/base to form a colourless solution. i.e. (i) when reacting with nitric(V)acid, the hydroxide shows basic properties. It reacts with the acid to form a simple salt and water only. Chemical equation Pb(OH) 2 (s) + 2HNO3(aq) -> Pb(NO3) 2 (aq) + 2H2O(l) Ionic equation Pb(OH) 2 (s) + 2H+ (aq) -> Pb 2+ (aq) + 2H2O(l) (ii) when reacting with sodium hydroxide, the hydroxide shows acidic properties. It reacts with a base to form a complex salt. Chemical equation 1.When Lead(II) hydroxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxoplumbate(II) complex salt.
Chemical equation Pb(OH) 2 (s) + 2HNO3(aq) -> Pb(NO3) 2 (aq) + 2H2O(l) Ionic equation Pb(OH) 2 (s) + 2H+ (aq) -> Pb 2+ (aq) + 2H2O(l) (ii) when reacting with sodium hydroxide, the hydroxide shows acidic properties. It reacts with a base to form a complex salt. Chemical equation 1.When Lead(II) hydroxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxoplumbate(II) complex salt. Pb(OH) 2 (s) + 2NaOH(aq) -> Na2Pb(OH) 4(aq) 2.When Lead(II) hydroxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxoplumbate(II) complex salt. Pb(OH) 2 (s) + 2KOH(aq) -> K2Pb(OH) 4(aq) Ionic equation Pb(OH) 2 (s) + 2OH-(aq) -> 2[Pb(OH) 4]2- (aq)
(c)Aluminium(III)oxide(Al2O3) and Aluminium(III)hydroxide(Al(OH)3) (i)When ½ spatula full of Aluminium(III)oxide is placed in a boiling tube containing 10cm3 of either 2M nitric(V)acid or 2M sodium hydroxide hydroxide solution, it dissolves on both the acid and the alkali/base to form a colourless solution. i.e. (i) when reacting with nitric(V)acid, the oxide shows basic properties by reacting with an acid to form a simple salt and water only.
Pb(OH) 2 (s) + 2KOH(aq) -> K2Pb(OH) 4(aq) Ionic equation Pb(OH) 2 (s) + 2OH-(aq) -> 2[Pb(OH) 4]2- (aq)
(c)Aluminium(III)oxide(Al2O3) and Aluminium(III)hydroxide(Al(OH)3) (i)When ½ spatula full of Aluminium(III)oxide is placed in a boiling tube containing 10cm3 of either 2M nitric(V)acid or 2M sodium hydroxide hydroxide solution, it dissolves on both the acid and the alkali/base to form a colourless solution. i.e. (i) when reacting with nitric(V)acid, the oxide shows basic properties by reacting with an acid to form a simple salt and water only. Chemical equation Al2O3 (s) + 6HNO3(aq) -> Al(NO3)3 (aq) + 3H2O(l) Al2O3 (s) + 6HCl(aq) -> AlCl3 (aq) + 3H2O(l) Al2O3 (s) + 3H2SO4(aq) -> Al2(SO4)3 (aq) + 3H2O(l) Ionic equation Al2O3 (s) + 3H+ (aq) -> Al 3+ (aq) + 3H2O(l) (ii) when reacting with sodium hydroxide, the oxide shows acidic properties by reacting with a base to form a complex salt. Chemical equation 1.When Aluminium(III) oxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxoaluminate(III) complex salt. Al2O3 (s) + 2NaOH(aq) + 3H2O(l) -> 2NaAl(OH) 4(aq) 2.When Aluminium(III) oxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxoaluminate(II) complex salt.
Chemical equation Al2O3 (s) + 6HNO3(aq) -> Al(NO3)3 (aq) + 3H2O(l) Al2O3 (s) + 6HCl(aq) -> AlCl3 (aq) + 3H2O(l) Al2O3 (s) + 3H2SO4(aq) -> Al2(SO4)3 (aq) + 3H2O(l) Ionic equation Al2O3 (s) + 3H+ (aq) -> Al 3+ (aq) + 3H2O(l) (ii) when reacting with sodium hydroxide, the oxide shows acidic properties by reacting with a base to form a complex salt. Chemical equation 1.When Aluminium(III) oxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxoaluminate(III) complex salt. Al2O3 (s) + 2NaOH(aq) + 3H2O(l) -> 2NaAl(OH) 4(aq) 2.When Aluminium(III) oxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxoaluminate(II) complex salt. Al2O3 (s) + 2KOH(aq) + 3H2O(l) -> 2NaAl(OH) 4(aq) Ionic equation Al2O3 (s) + 2OH-(aq) + 3H2O(l) -> 2[Al(OH) 4]- (aq) (ii)When Aluminium(III)hydroxide is placed in a boiling tube containing 10cm3 of either 2M nitric(V)acid or 2M sodium hydroxide hydroxide solution, it dissolves on both the acid and the alkali/base to form a colourless solution. i.e. (i) when reacting with nitric(V)acid, the hydroxide shows basic properties. It reacts with the acid to form a simple salt and water only.
i.e. (i) when reacting with nitric(V)acid, the hydroxide shows basic properties. It reacts with the acid to form a simple salt and water only. Chemical equation Al(OH) 3 (s) + 3HNO3(aq) -> Al(NO3)3 (aq) + 3H2O(l)
Al(OH)3 (s) + 3HCl(aq) -> AlCl3 (aq) + 3H2O(l) 2Al(OH)3 (s) + 3H2SO4(aq) -> Al2(SO4)3 (aq) + 3H2O(l) Ionic equation Al(OH)3 (s) + 3H+ (aq) -> Al 3+ (aq) + 3H2O(l) (ii) when reacting with sodium hydroxide, the hydroxide shows acidic properties. It reacts with a base to form a complex salt. Chemical equation 1.When aluminium(III) hydroxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxoaluminate(III) complex salt. Al(OH) 3 (s) + NaOH(aq) -> NaAl(OH) 4(aq) 2.When aluminium(III) hydroxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxoaluminate(III) complex salt.
It reacts with a base to form a complex salt. Chemical equation 1.When aluminium(III) hydroxide is reacted with sodium hydroxide the complex salt is sodium tetrahydroxoaluminate(III) complex salt. Al(OH) 3 (s) + NaOH(aq) -> NaAl(OH) 4(aq) 2.When aluminium(III) hydroxide is reacted with potassium hydroxide the complex salt is potassium tetrahydroxoaluminate(III) complex salt. Al(OH) 3 (s) + KOH(aq) -> KAl(OH) 4(aq) Ionic equation Al(OH) 3 (s) + OH-(aq) -> [Al(OH) 4]- (aq) Summary of amphotellic oxides/hydroxides Oxide Hydroxide Formula of simple salt from nitric (V)acid Formula of complex salt from sodium hydroxide ZnO Zn(OH)2 Zn(NO3)2 Na2Zn(OH)4 [Zn(OH)4]2-(aq) Sodium tetrahydroxozincate(II) PbO Pb(OH)2 Pb(NO3)2 Na2Pb(OH)4 [Pb(OH)4]2-(aq) Sodium tetrahydroxoplumbate(II) Al2O3 Al(OH) 3 Al(NO3)3 NaAl(OH)4 [Al(OH)4]-(aq) Sodium tetrahydroxoaluminate(II) 12.(a) A salt is an ionic compound formed when the cation from a base combine with the anion derived from an acid. A salt is therefore formed when the hydrogen ions in an acid are replaced wholly/fully or partially/partly ,directly or indirectly by a metal or ammonium radical. (b) The number of ionizable/replaceable hydrogen in an acid is called basicity of an acid. Some acids are therefore: (i)monobasic acids generally denoted HX e.g. HCl, HNO3,HCOOH,CH3COOH. (ii)dibasic acids ; generally denoted H2X e.g. H2SO4, H2SO3, H2CO3,HOOCOOH. (iii)tribasic acids ; generally denoted H3X e.g. H3PO4.
H2SO4, H2SO3, H2CO3,HOOCOOH. (iii)tribasic acids ; generally denoted H3X e.g. H3PO4. (c) Some salts are normal salts while other are acid salts. (i)A normal salt is formed when all the ionizable /replaceable hydrogen in an acid is replaced by a metal or metallic /ammonium radical. (ii)An acid salt is formed when part/portion the ionizable /replaceable hydrogen in an acid is replaced by a metal or metallic /ammonium radical. Table showing normal and acid salts derived from common acids Acid name Chemical formula Basicity Normal salt Acid salt Hydrochloric acid HCl Monobasic Chloride(Cl-) None Nitric(V)acid HNO3 Monobasic Nitrate(V)(NO3-) None Nitric(III)acid HNO2 Monobasic Nitrate(III)(NO2-) None Sulphuric(VI)acid H2SO4 Dibasic Sulphate(VI) (SO42-) Hydrogen sulphate(VI) (HSO4-) Sulphuric(IV)acid H2SO3 Dibasic Sulphate(IV) (SO32-) Hydrogen sulphate(IV) (HSO3-) Carbonic(IV)acid H2CO3 Dibasic Carbonate(IV)(CO32-) Hydrogen carbonate(IV) (HCO3-) Phosphoric(V) H3PO4 Tribasic Phosphate(V)(PO43-) Dihydrogen
acid phosphate(V) (H2PO42-) Hydrogen diphosphate(V) (HP2O42-) The table below show shows some examples of salts.
(i)A normal salt is formed when all the ionizable /replaceable hydrogen in an acid is replaced by a metal or metallic /ammonium radical. (ii)An acid salt is formed when part/portion the ionizable /replaceable hydrogen in an acid is replaced by a metal or metallic /ammonium radical. Table showing normal and acid salts derived from common acids Acid name Chemical formula Basicity Normal salt Acid salt Hydrochloric acid HCl Monobasic Chloride(Cl-) None Nitric(V)acid HNO3 Monobasic Nitrate(V)(NO3-) None Nitric(III)acid HNO2 Monobasic Nitrate(III)(NO2-) None Sulphuric(VI)acid H2SO4 Dibasic Sulphate(VI) (SO42-) Hydrogen sulphate(VI) (HSO4-) Sulphuric(IV)acid H2SO3 Dibasic Sulphate(IV) (SO32-) Hydrogen sulphate(IV) (HSO3-) Carbonic(IV)acid H2CO3 Dibasic Carbonate(IV)(CO32-) Hydrogen carbonate(IV) (HCO3-) Phosphoric(V) H3PO4 Tribasic Phosphate(V)(PO43-) Dihydrogen
acid phosphate(V) (H2PO42-) Hydrogen diphosphate(V) (HP2O42-) The table below show shows some examples of salts. Base/alkali Cation Acid Anion Salt Chemical name of salts NaOH Na+ HCl Cl NaCl Sodium(I)chloride Mg(OH)2 Mg2+ H2SO4 SO42 MgSO4 Mg(HSO4)2 Magnesium sulphate(VI) Magnesium hydrogen sulphate(VI) Pb(OH)2 Pb2+ HNO3 NO3 Pb(NO3)2 Lead(II)nitrate(V) Ba(OH)2 Ba2+ HNO3 NO3 Ba(NO3)2 Barium(II)nitrate(V) Ca(OH)2 Ba2+ H2SO4 SO42 MgSO4 Calcium sulphate(VI) NH4OH NH4+ H3PO4 PO43 (NH4 )3PO4 (NH4 )2HPO4 NH4 H2PO4 Ammonium phosphate(V) Diammonium phosphate(V) Ammonium diphosphate(V) KOH K+ H3PO4 PO43 K3PO4 Potassium phosphate(V) Al(OH)3 Al3+ H2SO4 SO42 Al2(SO4)2 Aluminium(III)sulphate(VI) Fe(OH)2 Fe2+ H2SO4 SO42 FeSO4 Iron(II)sulphate(VI) Fe(OH)3 Fe3+ H2SO4 SO42 Fe2(SO4)2 Iron(III)sulphate(VI) (d) Some salts undergo hygroscopy, deliquescence and efflorescence.