Othe [Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution is made that is 0.464 M in H₂S and 0.464 M in KHS. If Kal 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 0.114 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + + - Submit Answer Retry Entire Group 1 more group attempt remaining

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Use the References to access important values if needed for this question.
A buffer solution is made that is 0.464 M in H₂S and 0.464 M in KHS.
If Kal 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 0.114 mol HCl is added to 1.00 L of the buffer
solution.
(Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+)
+
+
Submit Answer
Retry Entire Group
1 more group attempt remaining
Transcribed Image Text:Other [Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution is made that is 0.464 M in H₂S and 0.464 M in KHS. If Kal 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 0.114 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + + Submit Answer Retry Entire Group 1 more group attempt remaining
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