A 5.50 −g sample of a weak acid with Ka=1.3×10−4 was
combined with 4.90 mL of...
A 5.50 −g sample of a weak acid with Ka=1.3×10−4 was
combined with 4.90 mL of 6.20 M NaOH and the resulting solution was
diluted to 750 mL. The measured pH of the
solution was 4.35.
A 5.65 −g sample of a weak acid with Ka=1.3×10−4 was combined
with 4.80 mL of 6.10 M NaOH and the resulting solution was diluted
to 750 mL. The measured pH of the solution was 4.15. What is the
molar mass of the weak acid?
A 5.65 −g sample of a weak acid with Ka=1.3×10−4 was combined
with 4.80 mL of 5.90 M NaOH and the resulting solution was diluted
to 750 mL. The measured pH of the solution was 4.25.
A 5.65 −g sample of a weak acid with Ka=1.3×10−4 was
combined with 5.20 mL of 5.90 M NaOH and the resulting solution was
diluted to 750 mL. The measured pH of the
solution was 4.30. What is the molar mass of the weak acid?
**please show work
A 5.65 −g sample of a weak acid with Ka=1.3×10−4 was
combined with 5.20 mLof 6.10 M NaOH and the resulting solution was
diluted to 750 mL. The measured pH of the
solution was 4.20.
What is the molar mass of the weak acid?
A 25.0 mL sample of a 0.150 M weak acid, Ka = 4.6 x 10−5 , is
titrated with 0.200 M NaOH. Calculate the pH when 10.0 mL of the
base has been titrated into the acid.
A certain weak acid, HA, has a Ka value of 1.3×10−7.
A) Calculate the percent ionization of HA in a 0.10 M solution.
Express your answer as a percent using two significant
figures.
B)Calculate the percent ionization of HA in a 0.010 M solution.
Express your answer as a percent using two significant figures.
A 25.00 mL sample containing a certain monoprotic weak acid, HA
(Ka 4.5 x 10-5) requires 16.25 mL of 0.102 M
NaOH to reach the endpoint of titration.
a) Determine the concentration of the acid in the sample.
b) Determine the pH of the original solution before any titrant
was added.
c) Determine the concentration of the conjugate base
A- at the endpoint of titration.
d) Determine the pH of the solution at the endpoint of the
titration.
25.00 mL of 0.185 M HCN (Ka = 4.90 x 10^-10) was titrated with
18.50 mL of Ca(OH)2. What is the pH of the original HCN solutuon?
What is the pH after 9.25 mL of base have been added?
Lactic acid (HC3H5O3), a weak
monoprotic acid with a Ka = 1.4 x 10-4, is
titrated with KOH. If you have 50.0 mL of a 0.500 M
HC3H5O3solution,
calculate the pH after 150.0 mL of 0.250 M KOH have been added: