Hydrolysis and Neutralization

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Hydrolysis and Neutralization

Presentation transcript:

Hydrolysis and Neutralization

Predict whether an aqueous solution of a given ionic compound will be acidic, basic or neutral given the formula.

Ionic compound produced by reacting an acid with a base. Neutralization reaction: acid + base salt + water Ionic compound produced by reacting an acid with a base. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) Salt produced in a neutralization can react with the water to produce acidic or basic solutions. We call this process salt hydrolysis.

HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) 3 possible neutralization reactions: SA + SB - results in neutral solution, pH = 7 HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) Anions of strong acids won’t affect pH: Cl-, ClO4-, I-, Br-, NO3- WA + SB - produces a solution with pH > 7 SA + WB – produces a solution with pH < 7

NH4+(aq) + H2O (aq) H3O+(aq) + NH3 (aq) Salt anions may accept hydrogen ions from the water producing a basic solution. OR Salt cations may donate hydrogen ions to the water producing an acidic solution. HNO3(aq) + NH3 (aq) NH4NO3 (aq) + H2O(l) NH4+(aq) + NO3¯(aq) NH4+(aq) + H2O (aq) H3O+(aq) + NH3 (aq)

Basic salts result from the reaction of a strong base with a weak acid. CH3COOH(aq) + NaOH (aq) CH3COONa (aq) + H2O(l) Na+(aq) + CH3COO¯(aq) CH3COO-(aq) + H2O(l) OH-(aq) + CH3COOH (aq)

Is K2CO3, acidic, basic or neutral? Step 1. Identify the ions present. Potassium carbonate will dissociate in water K2CO3(s) → 2 K+(aq) + CO32–(aq) Step 2. Determine if each ion will affect the pH. Carbonate ion is a strong CB of weak acid HCO3– . CO32– (aq) + H2O (l)  HCO3– (aq) + OH– (aq) Solution is basic.

FeCl3 is acidic in water: Other Salts: Metal salts containing 3+ or 2+ transition metal ions, will be acidic in water. FeCl3 is acidic in water: Fe(H2O)63+ + H2O  H3O+ + Fe(H2O)5(OH)2+ Oxides are basic in water because oxide ion, O2–, is a strong base. – (Na2O) O2–(aq) + H2O(l) → OH–(aq) + OH–(aq)