Given the following acid dissociation constants: K_a (H₃PO₄) = 7.5 × 10^-3
K_a (NH₄⁺) = 5.6 × 10^-10
Determine the equilibrium constant for the reaction below at 25 °C.
H₃PO₄(aq) + NH₃(aq) NH₄⁺(aq) + H₂PO₄−(aq)

Question

Given the following acid dissociation constants: K_a (H₃PO₄) = 7.5 × 10^-3
K_a (NH₄⁺) = 5.6 × 10^-10
Determine the equilibrium constant for the reaction below at 25 °C.
H₃PO₄(aq) + NH₃(aq)

Given the following acid dissociation constants: K<sub>a</sub> (H<sub>3</sub>PO<sub>4</sub>) = 7.5 × 10<sup>-3</sup> K<sub>a</sub> (NH<sub>4</sub><sup>+</sup>) = 5.6 × 10<sup>-10</sup> Determine the equilibrium constant for the reaction below at 25 °C. H<sub>3</sub>PO<sub>4</sub>(aq) + NH<sub>3</sub>(aq) NH<sub>4</sub><sup>+</sup>(aq) + H<sub>2</sub>PO<sub>4</sub>−(aq) A) 4.2 × 10<sup>-12</sup> B) 7.5 × 10<sup>-8</sup> C) 4.2 × 10<sup>2</sup> D) 1.3 × 10<sup>7</sup> E) 2.4 × 10<sup>11</sup>

NH₄⁺(aq) + H₂PO₄−(aq)

Quizplus · Accepted Answer

The Answer of Given the following acid dissociation constants: K_a (H₃PO₄)= 7.5 × 10^-3 K_a (NH₄⁺)= 5.6 × 10^-10 Determine the equilibrium constant for the reaction below at 25 °C. H₃PO₄(aq)+ NH₃(aq) NH₄⁺(aq)+ H₂PO₄−(aq) A) 4.2 × 10^-12 B) 7.5 × 10^-8 C) 4.2 × 10² D) 1.3 × 10⁷ E) 2.4 × 10¹¹

Given the Following Acid Dissociation Constants: Ka (H3PO4)= 7

Given the Following Acid Dissociation Constants: K_a (H₃PO₄)= 7