Question

a) The pKa of HF is 3.17. Calculate the pH of a 1.00 L solution that is 1.00 M HF and 1.50 M NaF.

b) What is the pH of this solution after addition of 50.0 mL of 10.0 M HCl?

Answer #1

a)

use:

pH = pKa + log {[conjugate base]/[acid]}

= 3.17+ log {1.5/1}

= 3.346

Answer: 3.35

b)

mol of HCl added = 10.0M *0.05 L = 0.5 mol

F- will react with H+ to form HF

Before Reaction:

mol of F- = 1.5 M *1.0 L

mol of F- = 1.5 mol

mol of HF = 1.0 M *1.0 L

mol of HF = 1 mol

after reaction,

mol of F- = mol present initially - mol added

mol of F- = (1.5 - 0.5) mol

mol of F- = 1 mol

mol of HF = mol present initially + mol added

mol of HF = (1 + 0.5) mol

mol of HF = 1.5 mol

since volume is both in numerator and denominator, we can use mol instead of concentration

use:

pH = pKa + log {[conjugate base]/[acid]}

= 3.17+ log {1/1.5}

= 2.994

Answer: 2.99

The pKa of HF is 3.17.
a. Calculate the pH of a 1.00 L solution that is 1.00M HF and
1.50M NaF.
b. What is the pH of this solution after addition of 50.0ml of
10.0M HCl.

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.

How many grams of sodium fluoride (NaF) would need to be added
to 1.00 L of 0.19 M HF to yield a solution with pH = 4.93? (pKa of
HF = 3.17)

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.

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?

A 1.00 L buffer solution is 0.150 M in HC7H5O2 and 0.25 M in
LiC7H5O2. Calculate the pH of the solution after the addition of
100.0 mL of 1.00 M HCl. The Ka for HC7H5O2 is 6.5x10^-5

The pKa of hypochlorous acid is 7.530. A 50.0 mL solution of
0.142 M sodium hypochlorite (NaOCl) is titrated with 0.338 M HCl.
Calculate the pH of the solution:
a) after the addition of 7.12 mL of 0.338 M HCl.
b) after the addition of 21.8 mL of 0.338 M HCl.
c) at the equivalence point with 0.338 M HCl.

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

Calculate the pH of 1.00 L of a buffer that is 0.120 M HNO2 and
0.150 M NaNO2.
then, Calculate the pH of the buffer described above after the
addition of 1.00 mL of 12.0 M HCl.

0.75 moles of HF and 1.00 mole of NaF were added to 1.00 L of
water. To this solution was added 0.300 mols of HCl. What was the
final pH of the solution? Give your answer to two decimal
places

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