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Hydrolysis and Neutralization

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10 diapositives · 651 Views · Sep 26, 2014

Hydrolysis and Neutralization. Predict whether an aqueous solution of a given ionic compound will be acidic, basic or neutral given the formula . Write balanced neutralization reactions involving strong acids and bases. Additional KEY Terms salt hydrolysis.

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Hydrolysis and Neutralization
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  1. Hydrolysis and Neutralization

  2. Predict whether an aqueous solution of a given ionic compound will be acidic, basic or neutral given the formula. • Write balanced neutralization reactions involving strong acids and bases. Additional KEY Terms salt hydrolysis

  3. Neutralization reaction (double replacement): acid + base salt + water Ionic compound produced by reacting an acid with a base. • When saltdissociates in water it canreact and produce an acidic or basic solutions • We call this process salt hydrolysis

  4. acid + base salt + water • 3 possible neutralization outcomes: • SA + SB - results in neutral solution, pH = 7 • 2. WA + SB – results in basicsolution pH > 7 • 3. SA + WB – results in acidic solution pH < 7

  5. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) • SA + SB - results in neutral solution, pH = 7 • strongacid/base leaves behind weak conjugates • so weak to be unreactive leaving neutral solution Na+ + Cl- weak CB • anions of strongest acids won’t affect pH: • Cl-, ClO4-, I-, Br-, NO3-(weakest CBs)

  6. CH3COO-(aq) + H2O(l) OH-(aq) + CH3COOH (aq) CH3COOH(aq) + NaOH (aq) CH3COONa (aq) + H2O(l) weak acid 2. WA + SB – results in basicsolution pH > 7 • weakacids leaves behind strong conjugate base • strong anion reacts to form basic solution Na+ + CH3COO¯ strong CB

  7. NH4+(aq) + H2O (aq) H3O+(aq) + NH3 (aq) HNO3(aq) + NH3 (aq) NH4NO3 (aq) + H2O(l) • 3. SA + WB – results in acidic solution pH < 7 • weakbases leaves behind strong conjugate acid • strong cation reacts to form acidic solution weak base NH4+ + NO3¯ strong CA

  8. 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) strong CB 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

  9. 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)

  10. CAN YOU / HAVE YOU? • Predictwhether an aqueous solution of a given ionic compound will be acidic, basic or neutral given the formula. • Write balanced neutralization reactions involving strong acids and bases. Additional KEY Terms salt hydrolysis