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.

Homework Answers

Answer #1

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

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
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 Benzoic Acid and Sodium Benzoate should be added in mL?
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.120 M sodium benzoate. How much of each solution should be mixed to prepare this buffer? ___ ml benzoic acid ___ ml sodium benzoate
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.180 M sodium benzoate. How much of each solutionshould be mixed to prepare this buffer? ____ mL of benzoic acid ____ mL sodium benzoate
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.140 M sodium benzoate.
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.180 M sodium benzoate. How much of each solution should be mixed to prepare this buffer?
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.200 M sodium benzoate. How much of each solution should be mixed to prepare this buffer?
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.220 M sodium benzoate. How much of each solution should be mixed to prepare tis solution?
Calculate the change in pH when 6.00 mL of 0.100 M HCl(aq) is added to 100.0...
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. change in pH = Calculate the change in pH when 6.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0...
Calculate the change in pH when 3.00 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. pH= ? Calculate the change in pH when 3.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution. pH=?
Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0...
Calculate the change in pH when 3.00 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. https://sites.google.com/site/chempendix/ionization Calculate the change in pH when 3.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.