A buffer solution is made that is 0.492 M in H2CO3 and 0.492 M in KHCO3. If Kal for H2CO3 is 4.20 X 10-7, what is the pH of the buffer solution? pH = _______ Write the net ionic equation for the reaction that occurs when 0.141 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+ )
A buffer solution is made that is 0.492 M in H2CO3 and 0.492 M in KHCO3. If Kal for H2CO3 is 4.20 X 10-7, what is the pH of the buffer solution? pH = _______ Write the net ionic equation for the reaction that occurs when 0.141 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+ )
Question
A buffer solution is made that is 0.492 M in H2CO3 and 0.492 M in KHCO3. If Kal for H2CO3 is 4.20 X 10-7, what is the pH of the buffer solution?
pH = _______
Write the net ionic equation for the reaction that occurs when 0.141 mol HNO3 is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit
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