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A buffer solution is made that is 0.418 M in HCN and 0.418 M in NaCN. K₂ for HCN is 4.00 x 10-¹0, what is the pH of the buffer solution? If pH = Write the net ionic equation for the reaction that occurs when 0.120 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) + +

A buffer solution is made that is 0.418 M in HCN and 0.418 M in NaCN. K₂ for HCN is 4.00 x 10-¹0, what is the pH of the buffer solution? If pH = Write the net ionic equation for the reaction that occurs when 0.120 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) + +

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
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Buffer Solution and pH Calculation** A buffer solution is made that is 0.418 M in HCN and 0.418 M in NaCN. If \( K_a \) for HCN is \( 4.00 \times 10^{-10} \), what is the pH of the buffer solution? pH = [________] **Net Ionic Equation for Reaction with KOH** Write the net ionic equation for the reaction that occurs when 0.120 mol KOH is added to 1.00 L of the buffer solution. *(Use the lowest possible coefficients. Omit states of matter.)* [________] + [________] ⟶ [________] + [________]
Transcribed Image Text:**Buffer Solution and pH Calculation** A buffer solution is made that is 0.418 M in HCN and 0.418 M in NaCN. If \( K_a \) for HCN is \( 4.00 \times 10^{-10} \), what is the pH of the buffer solution? pH = [________] **Net Ionic Equation for Reaction with KOH** Write the net ionic equation for the reaction that occurs when 0.120 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: Determine the pH of the buffer solution and the net ionic equation with base:

Given,

Molarity of HCN = 0.418 M

Molarity of NaCN = 0.418 M

Ka of HCN = 4.00 x 10-10 

moles of KOH = 0.120 mol

volume of buffer solution = 1.00 L

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