A buffer solution is made that is 0.317 M in H2S and 0.317 M in KHS....

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A buffer solution is made that is 0.317 M in H2S and 0.317 M in KHS. If Kal for H2S is 1.00 x 10, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.078 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) A buffer solution is made that is 0.317 M in H2S and 0.317 M in KHS. If Kal for H2S is 1.00 x 10, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.078 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)