a.
The ka of acetic acid is 1.8*10^-5.
What is the pka of the acetic acid?
b.What should be the ph of a solution of 1.0 mL of 0.1 M acetic
acid and 1.0 mL of 0.1 M sodium acetate and 48.0 mL H2O?
c.What should be the ph of a solution of 5.0 ml of 0.1 M acetic
acid and 5.0ml of 0.1M sodium acetate and 40.0ml h20?
is the answer 4.74 for all parts ?? thanks
1.) Acetic acid is a weak monoprotic acid with Ka=1.8*10^-5. In
an acid base titration, 100 mL of 0.100M acetic acid is titrated
with 0.100M NaOH. What is the pH of the solution:
a.)Before any NaOH is added
b.)Before addition of 15.0mL of 0.100M NaOH
c.)At the half-equivalence point
d.)After addition of total of 65.0mL of 0.100M NaOH
e.)At equivalence point
f.)After addition of a total of 125.0mL of 0.100M NaOH
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka =
1.8 10-5) by 0.100 M KOH. Calculate the pH of the resulting
solution after 0.0mL of KOH has been added.
1) 25.00 mL of acetic acid (Ka = 1.8 x 10-5) is titrated with a 0.09991M NaOH. It takes 49.50 mL of base to fully neutralize the acid and reach equivalence.
What is the concentration of the acid sample?
What is the initial pH?
What is the pH after 20.00 mL of base has been added?
What is the pH at equivalence ?
What is the pH after 60.00 mL of base has been added?
What indicator should be...
Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic
acid, CH3CO2H, is 1.8 × 10-5. If someone could list the steps and
calculations that would be helpful. Thank you!
Assuming that Ka = 1.85×10-5 for acetic
acid, calculate the pH at the equivalence point for a titration of
50 mL of 0.100 M acetic acid with 0.100 M NaOH.
3. a) Calculate the pH of a sodium acetate-acetic acid
buffer solution (Ka= 1.78 x 10-5) in
which the concentration of both components is 1.0 M. What would be
the pH of the
solution if 1.5 mL of 0.50 M NaOH was added to 35.0 mL of the
buffer? How much
does the pH change?
b) If the same amount and concentration of NaOH was
added to 35.0 mL of pure water
(initial pH = 7), what would be the...
The Ka of benzoic acid is 6.5 x 10 ^(-5)
a) Calculate the pH of a 40.00 mL, 0.1 M benzoic acid buffer
solution after the addition of 20.00 mL of a 0.1M NaOH
b) Calculate the pH of a 40.00 mL, 0.1 M benzoic acid buffer
solution after the addition of 50.00 mL of a 0.1M NaOH
REDOX TITRATION
2) Express the reactions for potassium permanganate titration
with sodium oxalate: Hint: include the 2 half-reactions.
3) What is the...