Please fill in the following table. Thanks for all the help!

Give the pKa and pKb of weak acids and bases. For each solution, calculate the pH of a 0.1000 M solution, and calculate the volume of 0.1000 M NaOH or HCl that would be required to titrate a 10.00 mL sample to the equivalence point. To fill-in the table below, answer the subsequent questions.

pKb(NH₃) =

pKa(CH₃COOH) =

pKa(NH₄Cl) =

pKb(CH₃COONa) =

pH(0.1000 M HCl) =

pH(0.1000 M KOH) =

pH(0.1000 M NH₃) =

pH(0.1000 M CH₃COOH) =

ptspH(0.1000 M NH₄Cl) =

pH(0.1000 M CH₃COONa) =

Volume of 0.1000 M NaOH required to titrate 10.00 mL of 0.1000 M HCl =

Volume of 0.1000 M HCl required to titrate 10.00 mL of 0.1000 M KOH =

Volume of 0.1000 M HCl required to titrate 10.00 mL of 0.1000 M NH₃ =

Volume of 0.1000 M NaOH required to titrate 10.00 mL of 0.1000 M CH₃COOH =

Volume of 0.1000 M NaOH required to titrate 10.00 mL of 0.1000 M NH₄Cl =

Volume of 0.1000 M HCl required to titrate 10.00 mL of 0.1000 M CH₃COONa =

Transcribed Image Text:

acid or base type strong acid strong base weak base weak acid weak acid CH3COONa weak base compound HCI KOH NH3 CH3COOH NH4Cl pka pkb initial pH (calculated) volume titrant (mL) acid or base type strong acid strong base weak base weak acid weak acid CH3COONa weak base compound HCI KOH NH3 CH3COOH NH4Cl pka pkb initial pH (calculated) volume titrant (mL)

Answer rating: 100% (QA)

1 pKb NH3475 2 pKaCH3COOH476at 25 degree Centigrade 3 pKa NH4Cl Does not exist as NH4Cl is a salt fo... View the full answer