Problem: The pH of 0.50 M HClO is 3.91. Calculate the change in pH when 1.68 g of NaClO (FW = 74.44 g/mol) is added to 47 mL of 0.50 M HClO (FW = 52.46 g/mol). Ignore any changes in volume. The Ka value for HClO is 3.0 x 10-8.a. 6.17b. 3.59c. 4.50d. 7.54e. 2.26

FREE Expert Solution

We’re being asked to calculate the change in pH when 1.68 g of NaClO (FW = 74.44 g/mol) is added to 47 mL of 0.50 M HClO (FW = 52.46 g/mol).

A solution that contains a weak acid and its conjugate base is a buffer solution. The pH of a buffer solution can be determined using the Henderson-Hasselbalch equation.

pH=pKa+log (conjugate baseweak acid)


Given solution:

The solution is composed of 1.68 g of NaClO (FW = 74.44 g/mol) is added to 47 mL of 0.50 M HClO (FW = 52.46 g/mol).

 HClO is a weak acid
 the anion in NaClO is the conjugate base

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Problem Details

The pH of 0.50 M HClO is 3.91. Calculate the change in pH when 1.68 g of NaClO (FW = 74.44 g/mol) is added to 47 mL of 0.50 M HClO (FW = 52.46 g/mol). Ignore any changes in volume. The Ka value for HClO is 3.0 x 10-8.

a. 6.17
b. 3.59
c. 4.50
d. 7.54
e. 2.26

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