1 / 10

Hydrolysis and Neutralization

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.

crete
Download Presentation

Hydrolysis and Neutralization

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related