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Calculate the pH of each of the following solutions. Ka(НС2 Н3О2) %3D 1.8 х 10 5 Ка(НCN) — 6.2 х 10 -10 Къ (NH3) — 1.8х 10-5 а. О.2 М КС2Н;О2 pH = b. 0.51 M NaCN pH = с. 0.4 М NH4CI pH =

Calculate the pH of each of the following solutions. Ka(НС2 Н3О2) %3D 1.8 х 10 5 Ка(НCN) — 6.2 х 10 -10 Къ (NH3) — 1.8х 10-5 а. О.2 М КС2Н;О2 pH = b. 0.51 M NaCN pH = с. 0.4 М NH4CI pH =

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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### Calculate the pH of Each of the Following Solutions Given equilibrium constants: - \( K_a(\text{HC}_2\text{H}_3\text{O}_2) = 1.8 \times 10^{-5} \) - \( K_a(\text{HCN}) = 6.2 \times 10^{-10} \) - \( K_b(\text{NH}_3) = 1.8 \times 10^{-5} \) #### a. \( 0.2 \, M \, \text{KC}_2\text{H}_3\text{O}_2 \) - **pH =** [Input Box] #### b. \( 0.51 \, M \, \text{NaCN} \) - **pH =** [Input Box] #### c. \( 0.4 \, M \, \text{NH}_4\text{Cl} \) - **pH =** [Input Box]
Transcribed Image Text:### Calculate the pH of Each of the Following Solutions Given equilibrium constants: - \( K_a(\text{HC}_2\text{H}_3\text{O}_2) = 1.8 \times 10^{-5} \) - \( K_a(\text{HCN}) = 6.2 \times 10^{-10} \) - \( K_b(\text{NH}_3) = 1.8 \times 10^{-5} \) #### a. \( 0.2 \, M \, \text{KC}_2\text{H}_3\text{O}_2 \) - **pH =** [Input Box] #### b. \( 0.51 \, M \, \text{NaCN} \) - **pH =** [Input Box] #### c. \( 0.4 \, M \, \text{NH}_4\text{Cl} \) - **pH =** [Input Box]
Expert Solution
Step 1

#(a):

KC2H3O2(aq) is a conjugate base of HC2H3O2(aq).

Hence it will undergo hydrolysis to form HC2H3O2(aq) and OH-(aq).

Chemical equation:

KC2H3O2(aq) + H2O(l)  <-----> HC2H3O2(aq) + OH-(aq) ;

Kb = KwKa = 1*10-141.8*10-5 = 5.56*10-10

Initial concentration of KC2H3O2(aq) = 0.2 M

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