Final answer:
To find the ionization constant of water (Kw) at 50 degrees Celsius with a pH of 6.630, we first calculate the concentration of hydronium ions from the pH, then square this value, as Kw equals the squared concentration of hydronium ions in pure water at equilibrium.
Step-by-step explanation:
The student is asking for the ionization constant, Kw, of pure water at 50 degrees Celsius given a pH of 6.630. In chemistry, the ionization constant is used to describe the equilibrium constant for the ionization of water, which varies with temperature.
To calculate Kw at 50°C, we first need to find the concentration of hydronium ions [H3O+], which can be obtained from the pH value:
[H3O+] = 10-pH = 10-6.630≈ 2.34 × 10-7M
Since the product of the concentrations of hydronium ions and hydroxide ions equals the ionization constant (Kw):
Kw = [H3O+][OH-]
For pure water, [H3O+] is equal to [OH-], thus:
Kw = (2.34 × 10-7M)2 = 5.48 × 10-14