25.0 ml of 0.500M cyanic acid, HCNO, is titrated with 0.500M
sodium hydroxide, NaOH. Calculate the...
25.0 ml of 0.500M cyanic acid, HCNO, is titrated with 0.500M
sodium hydroxide, NaOH. Calculate the pH of the solution after the
addition of 10.0 ml of NaOH solution.
A 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a
0.150 M NaOH solution. What is the pH at the equivalence point? The
Ka of hydrofluoric acid is 6.8 × 10-4.
A 25.0 mL sample of 0.100 M acetic acid is titrated with a 0.125
M NaOH solution. Calculate the pH of the mixture after 10, 20, and
30 ml of NaOH have been added (Ka=1.76*10^-5)
For the titration of 25.0 mL of 0.20 M hydrofluoric acid with
0.20 M sodium hydroxide , determine the volume of based added when
pH is a) 2.85 b) 3.15 c)11.89
A 25.0 mL sample of 0.150 M potassium hydroxide is titrated with
0.125 M hydrobromic acid solution. Calculate the pH after the
following volumes of acid have been added: a) 20.0 mL b) 25.0 mL c)
30.0 mL d) 35.0 mL e) 40.0 mL
A 25.0-mL sample of 0.150 M hydrocyanic acid, HCN, is titrated
with a 0.150 M NaOH solution. What is the pH after 16.3 mL of base
is added? The K a of hydrocyanic acid is 4.9 × 10 -10.
A 25.0 mL sample of 0.150 M hydrocyanic acid, HCN, is titrated
with a 0.150 M NaOH solution. What is the pH at the equivalence
point? The K a of hydrocyanic acid is 4.9 × 10 -10.
What is the pH...
A 25.0 mL of a weak acid is titrated with a strong base (0.1 M).
Calculate the pH of the solution during the titration if the weak
acid concentration is 0.10 M and its Ka = 1.8 x 10-5 and 10.0 mL of
base has been added. (Hint: use Henderson-Hasselbach equation).
a) pH = 4.56
b) pH= 5.28
c) pH= 4.74
40.00 mL of a 0.1000 M carbonic acid
(H2CO3) was titrated with 0.2000 M
sodium hydroxide.
carbonic acid pka1:6.35 pka2:10.33
1.Calculate the volume of sodium hydroxide required to reach the
first equivalence point.
2.Calculate the volume of sodium hydroxide required to reach the
second equivalence point.
3.Write the balanced acid-base reaction and calculate the pH
before the addition of sodium hydroxide.
4.Write the balanced acid-base reaction and calculate the pH
after the addition of 12.00 mL of sodium hydroxide
5.Write...
Suppose that you first titrated 25.00mL of 0.500M HCl with 0.500M
NaOH and then 25.00mL of 0.500M of your weak acid HA with 0.500M
NaOH. How would the titration curves compare at 15.00mL of NaOH
beyond the equivalence points?