For each acid–base equilibrium, label the stronger acid, the stronger base, the weaker acid, and the weaker base. Then predict whether the position of equilibrium lies toward the right or toward the left. [latex](a) H_{2}CO_{3} + OH^{-} \rightleftarrows HCO_{3} ^{-} + H_{2}O[/latex] [latex](b) HPO4^{2-} + NH3 \rightleftarrows PO4^{3-} + NH4 ^+[/latex] Strategy Use Table 8.2 to identify the stronger acid from the weaker acid and the stronger base from the weaker base. Once you have done that, determine in which direction the equilibrium lies. It always lies in the direction of the stronger components moving towards the weaker components.

Arrows connect the conjugate acid–base pairs, with the red arrows showing the stronger acid. The position of equilibrium in (a) lies toward the right. In (b) it lies toward the left.

Question 8.2: For each acid–base equilibrium, label the stronger acid, the...

Introduction to General, Organic and Biochemistry

For each acid–base equilibrium, label the stronger acid, the stronger base, the weaker acid, and the weaker base. Then predict whether the position of equilibrium lies toward the right or toward the left.

(a) H_{2}CO_{3} + OH^{-} \rightleftarrows HCO_{3}  ^{-} + H_{2}O

(b) HPO4^{2-}  + NH3 \rightleftarrows PO4^{3-}  + NH4 ^+

Strategy
Use Table 8.2 to identify the stronger acid from the weaker acid and the stronger base from the weaker base. Once you have done that, determine in which direction the equilibrium lies. It always lies in the direction of the stronger components moving towards the weaker components.

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