6. Calculate the pH of the0.20 M NH3/0.20 M NH4Cl buffer.What is the pH of the buffer after the addition of 10.0 mL of 0.10M HCl to 65.0 mL of the buffer?
7. A 0.2688 g sample of amonoprotic acid neutralized 16.4 mL of 0.08133 M KOH solution.Calculate the molar mass of the acid.
8. In a titrationexperiment, 12.5 mL of 0.500 M H2SO4neutralize 50.0 mL of NaOH. What is the concentration of the NaOHsolution?
9. A 0.1276 g sample of anunknown monoprotic acid was dissolved in 25.0 mL of water andtitrated with 0.0633 M NaOH solution. The volume of baserequired to bring the solution to the equivalence point was 18.4mL. (a) Calculate the molar mass of the acid. (b) After 10.0 mL ofbase had been added during the titration, the pH was determined tobe 5.87. What is the Ka of the unknown acid?
10. Calculate the pH at the equivalence pointfor the following titration: 0.20 M HCl versus 0.20 Mmethylamine (CH3NH3; Kb =4.4
6. Calculate the pH of the0.20 M NH3/0.20 M NH4Cl buffer.What is the pH of the buffer after the addition of 10.0 mL of 0.10M HCl to 65.0 mL of the buffer?
7. A 0.2688 g sample of amonoprotic acid neutralized 16.4 mL of 0.08133 M KOH solution.Calculate the molar mass of the acid.
8. In a titrationexperiment, 12.5 mL of 0.500 M H2SO4neutralize 50.0 mL of NaOH. What is the concentration of the NaOHsolution?
9. A 0.1276 g sample of anunknown monoprotic acid was dissolved in 25.0 mL of water andtitrated with 0.0633 M NaOH solution. The volume of baserequired to bring the solution to the equivalence point was 18.4mL. (a) Calculate the molar mass of the acid. (b) After 10.0 mL ofbase had been added during the titration, the pH was determined tobe 5.87. What is the Ka of the unknown acid?
10. Calculate the pH at the equivalence pointfor the following titration: 0.20 M HCl versus 0.20 Mmethylamine (CH3NH3; Kb =4.4
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