What is the ionic product for water (Kw) at 25°C?

What is the ionic product for water (Kw) at 25°C?

• A. 1 x 10-7
• B. 1 x 10-14
• C. 1 x 10-10
• D. 1 x 10-6

Answer: (B)

The ionic product for water (Kw) at 25°C is defined as the equilibrium constant for the self-ionization of water. This process can be expressed by the following equilibrium equation: \[ H_2O(l) \rightleftharpoons H^+(aq) + OH^-(aq) \] At equilibrium, the concentration of hydrogen ions \([H^+]\) and hydroxide ions \([OH^-]\) in pure water at 25°C is both 1 x 10^-7 mol/L. The ionic product (Kw) can be calculated using the equation: \[ K_w = [H^+][OH^-] \] Substituting the concentrations at 25°C: \[ K_w = (1 \times 10^{-7})(1 \times 10^{-7}) = 1 \times 10^{-14} \] This means that the actual value for Kw at this temperature is 1 x 10^-14. This value is critical in understanding the acid-base balance in aqueous solutions and is a reference point in many calculations involving pH and pOH. Understanding that at 25°C the ionic product is a constant aids in predicting the behavior of acids and bases in water,

The ionic product for water (Kw) at 25°C is defined as the equilibrium constant for the self-ionization of water. This process can be expressed by the following equilibrium equation:

[ H_2O(l) \rightleftharpoons H^+(aq) + OH^-(aq) ]

At equilibrium, the concentration of hydrogen ions ([H^+]) and hydroxide ions ([OH^-]) in pure water at 25°C is both 1 x 10^-7 mol/L. The ionic product (Kw) can be calculated using the equation:

[ K_w = [H^+][OH^-] ]

Substituting the concentrations at 25°C:

[ K_w = (1 \times 10^{-7})(1 \times 10^{-7}) = 1 \times 10^{-14} ]

This means that the actual value for Kw at this temperature is 1 x 10^-14. This value is critical in understanding the acid-base balance in aqueous solutions and is a reference point in many calculations involving pH and pOH.

Understanding that at 25°C the ionic product is a constant aids in predicting the behavior of acids and bases in water,