Question

# 1.) If a buffer solution is 0.110 M in a weak base (Kb = 5.7 ×...

1.) If a buffer solution is 0.110 M in a weak base (Kb = 5.7 × 10-5) and 0.590 M in its conjugate acid, what is the pH?

2.) You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.240 M sodium benzoate. How much of each solution should be mixed to prepare this buffer?

3.) Calculate the change in pH when 6.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). A list of ionization constants can be found here. Calculate the change in pH when 6.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.

The list is not present, please proivde the list for the 3 problem, remaining two answers are posted

Using the hessley henderbach equation

pOH = pKb + log[Conjugatea acid/Weak Base]

pOH = 5 - log(5.7) + log(5.3636)

pOH = 5 - log(1.0627) = 4.973

pH = 14 - 4.973 = 9.026

2)

pH = pKa + log(sodium benzoate/acid)

4 = 4.20 + log(sodium benzoate/acid)

sodium benzoate = 10^(-0.20) * [acid] = 0.6309 [acid]

V/1000 * 0.240 = 0.6309 * (100-V)/1000 * 0.100

4.804V = 100

V = 20.81 mL

Volume of base = 20.81 (sodium benzoate)

Volume of acid = 100 - 20.81 = 79.19 mL

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