![pH = pka + log\frac{[HCO^-_3]}{[H_2CO_3]} \\\\= 6.4 + log\frac{[HCO^-_3]}{[H_2CO_3]} -------(1)](/tpl/images/0558/9307/cd1e5.png)
![pH = pka + log\frac{[HPO_4^2^-]}{[H_2PO_4^-]} \\\\= 7.2 + log\frac{[HPO_4^2^-]}{[H_2PO_4^-]}-----(2)](/tpl/images/0558/9307/8d6aa.png)
Consider a solution consisting of the following two buffer systems:
H2CO3 HCO3– + H+ pKa...
Chemistry, 23.03.2020 17:05 lindseycagle00
Consider a solution consisting of the following two buffer systems:
H2CO3 HCO3– + H+ pKa = 6.4
H2PO4– HPO42– + H+ pKa = 7.2
At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?
***Please explain why the right answer is right and why the other ones are wrong.
a. [H2CO3] > [HCO3- ] and [H2PO4- ] > [HPO42- ]
b. [HCO3- ] > [H2CO3] and [HPO42- ] > [H2PO4- ]
c. [H2CO3 ] > [HCO3- ] and [HPO42- ] > [H2PO4- ]
d. [H2CO3] = [HCO3-] and [HPO42-] > [H2PO4- ]
e. [H2CO3] = [HCO3-] and [H2PO4- ] > [HPO42-]
Answers: 3
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