Part A)
A buffer solution is made that is 0.304 M in H2CO3 and 0.304 M in NaHCO3.
If Ka1 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 0.088 mol KOH is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter.)
PART B)
A buffer solution is made that is 0.311 M in H2CO3 and 0.311 M in KHCO3.
If ka1 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 0.089 mol HI is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter. Use H3O instead of H )
Answer:-
The answer is given in the image,
Part A) A buffer solution is made that is 0.304 M in H2CO3 and 0.304 M...
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