A) What is the pH of a solution made by mixing 30.0 mL of 0.10 M acetic acid, CH

Question

A) What is the pH of a solution made by mixing 30.0 mL of 0.10 M acetic acid, CH3COOH, with 30.0 mL of 0.10 M KOH? (See Appendix C for necessary information.) B) Write the balanced net ionic equation for the following reaction in basic solution. Be sure to show phase labels in your final answer. Mn2+ (aq) + H2O2 (aq) MnO2 (s) + H2O (l) c) Indicate whether ammonium nitrate will produce an acidic, basic, or neutral solution. Then, write the balanced equation that explains why that pH is seen. D) What is the pH of the resulting solution when 25.0 mL of 0.432 M methylamine, CH3NH2, is added to 15.0 mL of 0.234 M HCl? Ka = 2.70 x 10-11 for CH3NH3+

Explanation / Answer

a)pH=7+0.5pKa+logC

where C is the concentration of the salt.

so pH=8.963

b)Mn2(aq) + H2O2(aq) + 2OH(aq) --------------> 2MnO2(s) + 2H2O(l)

c)acidic since it is a salt of strong acid and weak base

D)pH=pKa+log(salt/acid)

=10.568+log((15*0.234)/(25*0.432-15*0.234))

=10.2506

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