[Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution is made that is 0.361 M in H₂S and 0.361 M in NaHS. 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 0.085 mol HBr 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 + 9 more group attempts remaining

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Chapter1: Chemical Foundations
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[References]
Use the References to access important values if needed for this question.
A buffer solution is made that is 0.361 M in
H₂S and 0.361 M in
NaHS.
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 0.085 mol HBr is added to
1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of Ht)
+
Submit Answer
->>
Retry Entire Group
+
ce from Cengage Learning
9 more group attempts remaining
Transcribed Image Text:[Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution is made that is 0.361 M in H₂S and 0.361 M in NaHS. 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 0.085 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of Ht) + Submit Answer ->> Retry Entire Group + ce from Cengage Learning 9 more group attempts remaining
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