Use the References to access important values if needed for this question. A buffer solution is made that is 0.346 M in H₂S and 0.346 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 0.098 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H*)

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Use the References to access important values if needed for this question.
A buffer solution is made that is 0.346 M in H₂S and 0.346 M in NaHS.
If Kal for H₂S is 1.00 x 107, what is the pH of the buffer solution?
pH =
Write the net ionic equation for the reaction that occurs when 0.098 mol HNO3 is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H*)
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Transcribed Image Text:Use the References to access important values if needed for this question. A buffer solution is made that is 0.346 M in H₂S and 0.346 M in NaHS. If Kal for H₂S is 1.00 x 107, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.098 mol HNO3 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 8 more group attempts remaining
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