A buffer solution is made that is 0.352 M in H2S and 0.352 M in NaHS.If Ka1 for H2S is 1.00 x 10 7, what is the pH of the buffer solution?pHWrite the net ionic equation for the reaction that occurs when 0.090 mol HNO3 is added to 1.00 L of the buffer solution.(Use the lowest possible coefficients. Omit states of matter. Use H30* instead of H*)++ A buffer solution is made that is 0.306 M in HCN and 0.306 M in KCN.If K, for HCN is 4.00 x 10 10, what is the pH of the buffer solution?pHWrite the net ionic equation for the reaction that occurs when 0.082 mol KOH is added to 1.00 L of the buffer solution.(Use the lowest possible coefficients. Omit states of matter.)

Name: A buffer solution is made that is 0.352 M in H2S and 0.352 M in NaHS.
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Description: A buffer solution is made that is 0.352 M in H2S and 0.352 M in NaHS.If Ka1 for H2S is 1.00 x 10 7, what is the pH of the buffer solution?pHWrite the net ionic equation for the reaction that occurs when 0.090 mol HNO3 is added to 1.00 L of the buffe

Given that: [H2S] = 0.352 M [NaHS] = 0.352 MKa = 1.00×10-7 Here H2S is a weak acid and NaHS is a…

Answered: quation for the reaction that occurs…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 10ALQ

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A buffer solution is made that is 0.352 M in H2S and 0.352 M in NaHS.
If Ka1 for H2S is 1.00 x 10 7, what is the pH of the buffer solution?
pH
Write the net ionic equation for the reaction that occurs when 0.090 mol HNO3 is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter. Use H30* instead of H*)
+
+

A buffer solution is made that is 0.306 M in HCN and 0.306 M in KCN.
If K, for HCN is 4.00 x 10 10, what is the pH of the buffer solution?
pH
Write the net ionic equation for the reaction that occurs when 0.082 mol KOH is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter.)

Expert Solution

Step 1

Given that:

[H₂S] = 0.352 M
[NaHS] = 0.352 M
K_a = 1.00×10^-7

Here H₂S is a weak acid and NaHS is a salt of weak acid.

Step 2

pH of the buffer solution can be calculated by the Henderson-Hasselbalch equation.

$\begin{array}{l} pH = - \log K_{a} + \log \frac{[Salt]}{[Acid]} \\ pH = - \log (1.00 \times 10^{- 7}) + \log \frac{0.352}{0.352} \\ pH = - (- 7) + 0 \\ pH = 7 \end{array}$

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