Question
In: Chemistry
2) A 25.0 mL sample of 0.160 M KOH is titrated with 0.250 M HCl. Determine...
2)
A 25.0 mL sample of 0.160 M KOH is titrated with 0.250 M HCl.
Determine the following quantities:
a)
The initial pH of the KOH solution before any acid is added.
b)
The pH of the solution after 3.00 mL of HCl is added.
c)
The quantity of HCl solution required to reach the equivalence
point.
d)
The pH of the solution at the equivalence point.
e)
The pH of the solution after20.0 mL of HCl is added.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A 30.00 mL sample of 0.200 M HBr was titrated with 0.160 M KOH. a. What...
A 30.00 mL sample of 0.200 M HBr was titrated with 0.160 M
KOH.
a. What is the initial pH of the sample?
b. What is the equivalence volume?
c. What is the pH after 19.16 mL of KOH is added?
A 25.0 mL sample of 0.30 M HCOOH is titrated with 0.20 M KOH. What is...
A 25.0 mL sample of 0.30 M HCOOH is titrated with 0.20 M KOH.
What is the pH of the solution after 25.0 mL of KOH has been added
to the acid? Ka = 1.8x10^-4
A 25.0 mL sample of 0.35 M lactic acid, HC3H5O3, is titrated with 0.070 M KOH....
A 25.0 mL sample of 0.35 M lactic acid, HC3H5O3, is titrated
with 0.070 M KOH. Determine the pH of the solution at the
equivalence point and at half-way to equivalence point. The Ka of
lactic acid is 1.38x10^-4.
A 100.0 mL sample of 0.20 M HF is titrated with 0.20 M KOH. Determine the...
A 100.0 mL sample of 0.20 M HF is titrated with 0.20 M KOH.
Determine the pH of the solution after the addition of 50.0 mL of
KOH. The Ka of HF is 3.5 × 10-4.
A. 2.08
B. 3.15
C. 4.33
D. 3.46
E. 4.15
A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the...
A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.
Determine the pH of the solution after the addition of 200.0 mL of
KOH. The Ka of HF is 3.5 × 10-4.
Answer: 8.14 but how do I get this?? I'm so lost!
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution....
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M
KOH solution. Calculate the pH after the following additions of the
KOH solution: (a) 0.0 mL, (b) 5.0 mL, (c) 10.0 mL, (d) 12.5 mL, (e)
15.0 mL. (25 points)
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution....
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M
KOH solution. Calculate the pH after the following additions of the
KOH solution: (a) 0.0 mL, (b) 5.0 mL, (c) 10.0 mL, (d) 12.5 mL, (e)
15.0 mL. (25 points)
25.0 mL of a 0.100 M HCN solution is titrated with 0.100 M KOH. Ka of...
25.0 mL of a 0.100 M HCN solution is titrated with
0.100 M KOH. Ka of HCN=6.2 x 10^-10.
a)What is the pH when 25mL of KOH is added (this is the equivalent
point).
b) what is the pH when 35 mL of KOH is added.
A 50.0 mL solution of 0.167 M KOH is titrated with 0.334 M HCl . Calculate...
A 50.0 mL solution of 0.167 M KOH is titrated with 0.334 M HCl .
Calculate the pH of the solution after the addition of each of the
given amounts of HCl .
0.00 mL pH = 7.00 mL pH = 12.5 mL pH = 19.0 mL pH = 24.0 mL pH = 25.0 mL pH = 26.0 mL pH = 31.0 mL pH =
A 50.0 mL solution of 0.199 M KOH is titrated with 0.398 M HCl. Calculate the...
A 50.0 mL solution of 0.199 M KOH is titrated with 0.398 M HCl.
Calculate the pH of the solution after the addition of the
following amounts of HCl.
a) 0.00 mL HCl
b) 7.00 mL HCl
c) 12.5 mL HCl
d) 20.0 mL HCl
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