A buffer solution is made that is 0.389 M in HCN and 0.389 M in NaCN. If K, for HCN is 4.00 x 10-10 what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.079 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H30 instead of H*)
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![### Chemistry Buffer Solution Problem
A buffer solution is made that is 0.389 M in HCN and 0.389 M in NaCN.
If \( K_a \) for HCN is \( 4.00 \times 10^{-10} \), what is the pH of the buffer solution?
\[ \text{pH} = \]
Write the net ionic equation for the reaction that occurs when 0.079 mol HBr is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter. Use \( \text{H}_3\text{O}^+ \) instead of \( \text{H}^+ \).)
\[ \text{[ ]} + \text{[ ]} \rightarrow \text{[ ]} + \text{[ ]} \]
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