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6. A titration is carried out where 3.0 mL of 0.70 M NaOH is added to 15.0 mL of 0.150 M HCl. What is the final pH (to two decimal places) of this solution? A: 2.08

6. A titration is carried out where 3.0 mL of 0.70 M NaOH is added to 15.0 mL of 0.150 M HCl. What is the final pH (to two decimal places) of this solution? A: 2.08

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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**Worksheet 14** 6. A titration is carried out where 3.0 mL of 0.70 M NaOH is added to 15.0 mL of 0.150 M HCl. What is the final pH (to two decimal places) of this solution? *A: 2.08*
Transcribed Image Text:**Worksheet 14** 6. A titration is carried out where 3.0 mL of 0.70 M NaOH is added to 15.0 mL of 0.150 M HCl. What is the final pH (to two decimal places) of this solution? *A: 2.08*
Expert Solution
Step 1

Given,

For NaOH solution

Concentration of NaOH solution = 0.70 M = 0.70 mol/L

Volume of NaOH solution = 3.0 mL = 0.003 L

For HCl solution

Concentration of HCl solution = 0.150 M = 0.150 mol/L

Volume of HCl solution = 15.0 mL = 0.015 L

pH of the solution = ?

 

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