Question

**A)Calculate the pH of 0.100 L of a buffer solution that
is 0.27 M in HF (Ka = 3.5 x 10-4 ) and 0.51 M in
NaF?B)**What is the pH after adding 0.004 mol of HNO3 to the
buffer described in Part A?

C)What is the pH after adding 0.004 mol of KOH to the buffer described in Part A?

Answer #1

A)

volume = 0.1 L

molatity of HF = 0.27 M

molarity of NaF = 0.51 M

pKa of HF = 3.46

pH = pKa + log [salt / acid]

= 3.46 + log (0.51 / 0.27)

= 3.74

**pH = 3.74**

B)

HNO3 moles (C) = 0.004

pH = pKa + log [salt - C] / [acid + C]

= 3.46 + log [0.51 x 0.1 - 0.004 / 0.27 x 0.1 + 0.004]

= 3.64

**pH = 3.64**

C)

moles of KOH (C) = 0.004

pH = pKa + log [salt + C / acid - C]

= 3.46 + log [0.51 x 0.1 + 0.004 / 0.27 x 0.1 - 0.004]

= 3.84

**pH = 3.84**

Part A
Calculate the pH of 0.100 L of a buffer solution that is 0.23 M
in HF (Ka = 3.5 x 10-4 ) and 0.45 M in NaF.
Express your answer using three significant figures.
pH =
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Part B
What is the pH after adding 0.001 mol of HNO3 to the buffer
described in Part A?
Express your answer using three significant figures.
pH =
SubmitMy AnswersGive
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Part C
What is the pH after adding...

Part A
Calculate the pH of 0.100 L of a buffer solution that is 0.23 M
in HF and 0.55 M in NaF.
Part B
Calculate pH of the solution on addition of the following. 0.004
mol of HNO3
Part C
Calculate pH of the solution on addition of the following. 0.002
mol of KOH

A 1.00 L buffer solution is composed of 0.250 M HF and 0.250 M
NaF. Calculate the 13)______ pH of the solution after the addition
of 0.150 moles of solid NaOH. Assume no volume change upon the
addition of base. The Ka for HF is 3.5 × 10-4.

A buffer is created with 0.100 moles of HF and 0.100 moles of
NaF in a 1.00 L aqueous solution. This buffer has a pH of 3.15. How
many moles of NaOH would you need to add to this buffer in order to
obtain a solution with a pH of 3.80. (Ka of HF = 7.1 x 10–4)

A 1.0 L solution contains 0.25 M HF and 0.32 M NaF (Ka for HF is
7.2x10^-4.
a) What is the pH of the above solution
b) If one adds 0.3 L of 0.020 M KOH to the solution, what will
be the pH of the solution?

The Ka value for HF is 3.5×10?4.
Calculate the change in pH when 2.0×10?2mol of NaOH is added to
0.50 L of a buffer solution that is 0.15 M in HF and 0.20
M in NaF.

Calculate the pH of a solution that is 0.200 M in NaF (aq) and
0.300 M HF (aq). Ka for HF is 3.5*10-4
Calculate the pH after 0.050 moles of NaOH is added to 1 L of
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Please help thank you in advnce

50 mL of 0.100 M HF is titrated with 55 mL of 0.100 M KOH. What
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A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.
Calculate the pH of the solution after the addition of 0.150 moles
of solid LiOH. Assume no volume change upon the addition of base.
The Ka for HF is 3.5x10^-4.
Please show how to work out this problem.

Calculate the pH of a buffer, consisting of 0.42 M HF and 0.42 M
F -, before and after addition of 0.44 g of NaOH to 1.0 L of the
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(a) before
(b) after

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