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Blood is a buffer of H(2)CO(3) and[HCO(3...

Blood is a buffer of `H_(2)CO_(3) and[HCO_(3)^(-)] ` with pH = 7.40. Given `K_(1) ` of `H_(2)CO_(3) = 4.5xx10^(-7)`. What will be the ratio of `[HCO_(3)^(-)]` to `[H_(2)CO_(3)]` in the blood ?

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To find the ratio of \([HCO_3^-]\) to \([H_2CO_3]\) in the blood, we can use the dissociation constant \(K_1\) of carbonic acid \((H_2CO_3)\) and the pH of the blood. ### Step-by-Step Solution: 1. **Understanding the Dissociation of Carbonic Acid:** The dissociation of carbonic acid can be represented as: \[ H_2CO_3 \rightleftharpoons H^+ + HCO_3^- ...
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