Question

Які з даних солей гідролізують ? Напишіть молекулярні та йонні рівняння реакцій гідролізу солей для вказаного варіанту. Вкажіть рН середовища . Солі Na2S, ZnBr2, CH3COONH4, KNO3 Na2SO3, Fe2(SO4)3, (NH4)2CO3, CaCl2 CH3COOK, NHẠCI, Cu(NO3)2, NaC104 7K2CO3, CuCl2, (NH4)2SO3, NaCl

Answer 1

Salts that undergo hydrolysis

Certain salts undergo hydrolysis when dissolved in water. Hydrolysis is a chemical reaction in which water molecules react with the ions of the salt, resulting in the formation of new compounds. The extent of hydrolysis depends on the nature of the salt and the pH of the solution. Here are the salts you mentioned and their hydrolysis reactions:

1. Na2S (sodium sulfide): - Molecular equation: Na2S + 2H2O → 2NaOH + H2S - Ionic equation: 2Na+ + S2- + 2H2O → 2Na+ + 2OH- + H2S - pH of the solution: Basic (due to the formation of hydroxide ions)

2. ZnBr2 (zinc bromide): - Molecular equation: ZnBr2 + 2H2O → Zn(OH)2 + 2HBr - Ionic equation: Zn2+ + 2Br- + 2H2O → Zn(OH)2 + 2H+ + 2Br- - pH of the solution: Acidic (due to the formation of hydronium ions)

3. CH3COONH4 (ammonium acetate): - Molecular equation: CH3COONH4 + H2O → CH3COOH + NH4OH - Ionic equation: CH3COO- + NH4+ + H2O → CH3COOH + NH4OH - pH of the solution: Slightly acidic (due to the formation of acetic acid)

4. KNO3 (potassium nitrate): - Molecular equation: KNO3 + H2O → KOH + HNO3 - Ionic equation: K+ + NO3- + H2O → KOH + HNO3 - pH of the solution: Neutral (due to the formation of a strong acid and a strong base)

5. Na2SO3 (sodium sulfite): - Molecular equation: Na2SO3 + H2O → NaHSO3 + NaOH - Ionic equation: 2Na+ + SO3^2- + H2O → NaHSO3 + OH- - pH of the solution: Basic (due to the formation of hydroxide ions)

6. Fe2(SO4)3 (iron(III) sulfate): - Molecular equation: Fe2(SO4)3 + 6H2O → 2Fe(OH)3 + 3H2SO4 - Ionic equation: 2Fe^3+ + 3(SO4)^2- + 6H2O → 2Fe(OH)3 + 3H+ + 3(SO4)^2- - pH of the solution: Acidic (due to the formation of hydronium ions)

7. (NH4)2CO3 (ammonium carbonate): - Molecular equation: (NH4)2CO3 + H2O → 2NH4OH + CO2 - Ionic equation: 2NH4+ + CO3^2- + H2O → 2NH4OH + CO2 - pH of the solution: Basic (due to the formation of hydroxide ions)

8. CaCl2 (calcium chloride): - Molecular equation: CaCl2 + 2H2O → Ca(OH)2 + 2HCl - Ionic equation: Ca^2+ + 2Cl- + 2H2O → Ca(OH)2 + 2H+ + 2Cl- - pH of the solution: Acidic (due to the formation of hydronium ions)

9. CH3COOK (potassium acetate): - Molecular equation: CH3COOK + H2O → CH3COOH + KOH - Ionic equation: CH3COO- + K+ + H2O → CH3COOH + OH- - pH of the solution: Basic (due to the formation of hydroxide ions)

10. NH4Cl (ammonium chloride): - Molecular equation: NH4Cl + H2O → NH4OH + HCl - Ionic equation: NH4+ + Cl- + H2O → NH4OH + H+ + Cl- - pH of the solution: Acidic (due to the formation of hydronium ions)

11. Cu(NO3)2 (copper(II) nitrate): - Molecular equation: Cu(NO3)2 + 2H2O → Cu(OH)2 + 2HNO3 - Ionic equation: Cu^2+ + 2NO3- + 2H2O → Cu(OH)2 + 2H+ + 2NO3- - pH of the solution: Acidic (due to the formation of hydronium ions)

12. NaClO4 (sodium perchlorate): - Molecular equation: NaClO4 + H2O → NaOH + HClO4 - Ionic equation: Na+ + ClO4- + H2O → NaOH + HClO4 - pH of the solution: Basic (due to the formation of hydroxide ions)

13. 7K2CO3 (potassium carbonate): - Molecular equation: 7K2CO3 + 7H2O → 7KOH + 7CO2 - Ionic equation: 7K+ + 7CO3^2- + 7H2O → 7KOH + 7CO2 - pH of the solution: Basic (due to the formation of hydroxide ions)

14. CuCl2 (copper(II) chloride): - Molecular equation: CuCl2 + 2H2O → Cu(OH)2 + 2HCl - Ionic equation: Cu^2+ + 2Cl- + 2H2O → Cu(OH)2 + 2H+ + 2Cl- - pH of the solution: Acidic (due to the formation of hydronium ions)

15. (NH4)2SO3 (ammonium sulfite): - Molecular equation: (NH4)2SO3 + H2O → 2NH4OH + SO2 - Ionic equation: 2NH4+ + SO3^2- + H2O → 2NH4OH + SO2 - pH of the solution: Basic (due to the formation of hydroxide ions)

16. NaCl (sodium chloride): - Molecular equation: NaCl + H2O → NaOH + HCl - Ionic equation: Na+ + Cl- + H2O → NaOH + H+ + Cl- - pH of the solution: Neutral (due to the formation of a strong acid and a strong base)

Please note that the pH values mentioned are approximate and can vary depending on the concentration of the salt and other factors.