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If Kal for H2 CO3 is 4.20 x 10-, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.097 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3 0* instead of H*)

If Kal for H2 CO3 is 4.20 x 10-, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.097 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3 0* instead of H*)

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A buffer solution is made that is 0.331 M in H2CO3 and 0.331 M in KHCO3. If Kal for H2 CO3 is 4.20 x 10-, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.097 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3 O* instead of H)
Transcribed Image Text:A buffer solution is made that is 0.331 M in H2CO3 and 0.331 M in KHCO3. If Kal for H2 CO3 is 4.20 x 10-, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.097 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3 O* instead of H)
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