An aqueous solution has [C6H5COOH] = 0.110 M and [Ca(C6H5COO)2] = 0.200 M. Ka = 6.3 × 10-5 for C6H5COOH. The solution volume is 5.00 L. What is the pH of the solution after 10.00 mL of 5.00 M NaOH is added? Group of answer choices 4.81 4.86 4.75 4.70 4.65

The answer is 4.8659

Explanation:

Given:

[C₆H₅COOH]=0.11M

[C₆H₅COO]=2*0.2=0.4M

Ka=6.3x10⁻⁵

First, calculate the pKa:

The pH is:

Like the volume is 5L, the volume of C₆H₅COO is x, then, the volume of C₆H₅COOH is 5-x

Solving for x:

x=2.49L=2490mL of C₆H₅COO

2510mL of C₆H₅COOH

The milimoles of C₆H₅COOH and C₆H₅COO is:

nC₆H₅COOH=(0.11*2510)-50=226.1mmol

nC₆H₅COO=(0.4*2490)+50=1046mmol

The pH is:

4.86

Explanation:

The pH of a solution is a measure of the molar concentration of hydrogen ions in the solution and as such is a measure of the acidity or basicity of the solution.

Please kindly check attachment for the step by step solution of the given problem.

the dissolution of polymer can be thermodynamically described in 2 steps.

your answer is c) plasma

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