Calculate the pH of the solution that results when 15.0 mL of 0.1790 M formic acid ( Ka(HCOOH) = 1.80 × 10¬4) is %3D a. diluted to 45.0 mL with distilled water. pH = b. mixed with 30.0 mL of 0.0895 M NaOH solution. pH = c. mixed with 30.0 mL of 0.150 M NaOH solution. pH =

Calculate the pH of the solution that results when 15.0 mL of 0.1790 M formic acid ( Ka(HCOOH) = 1.80 × 10¬4) is %3D a. diluted to 45.0 mL with distilled water. pH = b. mixed with 30.0 mL of 0.0895 M NaOH solution. pH = c. mixed with 30.0 mL of 0.150 M NaOH solution. pH =

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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**Problem Statement:**

Calculate the pH of the solution that results when 15.0 mL of 0.1790 M formic acid $(K_a(\text{HCOOH}) = 1.80 \times 10^{-4})$ is:

a. diluted to 45.0 mL with distilled water.

- **pH =**

b. mixed with 30.0 mL of 0.0895 M NaOH solution.

- **pH =**

c. mixed with 30.0 mL of 0.150 M NaOH solution.

- **pH =**

d. mixed with 30.0 mL of 0.150 M sodium formate solution.

- **pH =**

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