In water, the following equilibrium exists: H⁺(aq) + OH^-(aq) H₂O(l)
In pure water at 25°C, the concentration of H+ ions is 1.00 × 10^-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

Question

In water, the following equilibrium exists: H⁺(aq) + OH^-(aq)

In water, the following equilibrium exists: H<sup>+</sup>(aq) + OH<sup>-</sup>(aq) H<sub>2</sub>O(l) In pure water at 25°C, the concentration of H+ ions is 1.00 × 10<sup>-7</sup> mol/L. Calculate the value of the equilibrium constant for the reaction as written above. A) 1.00 × 10<sup>14</sup> B) 1.00 × 10<sup>12</sup> C) 1.00 × 10<sup>-14</sup> D) 1.00 × 10<sup>-12</sup> E) 5.55 × 10<sup>15</sup>

H₂O(l)
In pure water at 25°C, the concentration of H+ ions is 1.00 × 10^-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

Quizplus · Accepted Answer

The Answer of In water, the following equilibrium exists: H⁺(aq) + OH^-(aq) H₂O(l) In pure water at 25°C, the concentration of H+ ions is 1.00 × 10^-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

In Water, the Following Equilibrium Exists: H+(aq) + OH-(aq)

In Water, the Following Equilibrium Exists: H⁺(aq) + OH^-(aq)