NH3(aq)+H2O(l)⇄NH4+(aq)+OH−(aq) Kb=1.8×10−5 at 25°CThe reaction between NH3 and water is represented above. A solution that is initially 0.200M in NH3 has a pH of 11.28. Which of the following correctly predicts the pH of a solution for which [NH3]initial=0.100M, and why?AThe pH will be lower than 11.28 because decreasing the initial concentration of NH3 increases the equilibrium concentration of the conjugate acid NH4+.BThe pH will be lower than 11.28 because the equilibrium concentration of OH− ions decreases when the initial concentration of the base decreases.CThe pH will be higher than 11.28 because decreasing the initial concentration of NH3 decreases the equilibrium concentration of the conjugate acid NH4+.DThe pH will be higher than 11.28 because the equilibrium concentration of OH− ions increases when the initial concentration of the base decreases.

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