1.calculate the volume of 50% NaOH required to make 300 mL of a
0.1 M NaOH solutions 2.Calculate the standard potassium hydrogen
phthalate required to react with 25 mL of a 0.1 M NaOH solution 2.
Calculate the mass of the standard potassium hydrogen phthalate
required to react with 25 mL of a 0.1 M NaOH solution.
Calculate the volume of 0.20 mol/L KH2PO4
and the volume of 0.10 mol/L NaOH required to prepare 50.0 mL of
buffer with a formal (or total) concentration of
H2PO4 of 0.020 mol/L and a pH =
6.3. Repeat this calculation for buffers (of the same volume and
formal concentration) with pH = 6.5, 6.9, 7.5, 7.9, and 8.2.
Calculate the volume (in mL) of 0.170 M NaOH that must be added
to 259 mL of 0.0419 M 3-(N-Morpholino)propanesulfonic acid (MOPS)
to give the solution a pH of 7.55. The pKa of MOPS = 7.18.
a) Calculate the volume (in ML) of 0.170 M NaOH that must be
added to 365 mL of 0.0515 M 3-(N-Morpholino) propanesulfonic acid
(MOPS) to give the solution a pH of 7.55. The pKa of MOPS
=7.18.
b) A buffer with a pH of 4.24 contains 0.11 M of sodium benzoate
and 0.10 M of benzoic acid. What is the concentration of [H+] in
the solution after the addition of 0.056 mol of HCl to a final
volume of 1.6...
A 100.0 ml buffer solution is 0.20 M HC7H5O2 and 0.15 M
NaC7H5O2. Calculate the pH of the solution after the addition of
0.0025 moles of NaOH. Assume the volume of the buffer does not
change. (HC7H5O2 = Ka 6.5x10^-5)
. What volume of 0.1 M NaOH is required to completely react with
50.00 mL of 0.1 M CH3COOH? (In other words, what volume is required
to reach the equivalence point?). Show work/reasoning.
Calculate the pH during the titration of 50.0 mL of 0.116 M NaOH
with 0.0750 M HNO3 at:a) 0 mL titrant b) 3 mL before equivalence c)
at equivalence d) 3 mL past equivalence
Calculate the change in pH when 55.0 mL of a 0.620 M solution of
NaOH is added to 1.00 L of a solution that is 1.00 M in sodium
acetate and 1.00 M in acetic acid.
Calculate the change in pH when 49.0 mL of a 0.700 M solution of
NaOH is added to 1.00 L of a solution that is 1.00 M in sodium
acetate and 1.00 M in acetic acid.
Calculate the change in pH when 64.00 mL of a 0.575 M solution
of NaOH is added to 1.00 L of a solution that is 1.00 M in sodium
acetate and 1.00 M in acetic acid.