Question

what is the ph of a 80.0 ml solution which is 0.23 m in io− and 0.47 m in hio ? the a for hio is 2.3×10−11 .

Answer 1

To find the pH of the solution, we use the equation for the ionization of hio and the equilibrium expression. By substituting the given values, we can solve for the concentration of hio, which is 4.7 x 10^-10 M.

Step-by-step explanation:

To find the pH of the solution, we need to consider the ionization of hio. The equation for the ionization is:
hio → h+ + io-
The concentration of h+ ions is 0.47 M, and the concentration of io- ions is 0.23 M. The equilibrium expression for the ionization reaction is given by:
Ka = [h+][io-]/[hio]
Substituting the given values:
2.3 x 10-11 = (0.47)(0.23)/x
Solving for x, we find x = [hio] = 0.47 x 0.23 / 2.3 x 10-11 = 4.7 x 10-10 M

Answer 2

To find the pH of the solution, calculate the concentration of the hydronium ion using the given information. Then use the formula pH = -log[H3O+].

Step-by-step explanation:

To determine the pH of the solution, we need to calculate the concentration of the hydronium ion (H3O+). The formula to calculate pH is pH = -log[H3O+].

Given that the solution is 0.23 M in IO- and 0.47 M in HIO, we can find the concentrations of the hydronium ion and the hydroxide ion using the equation [H3O+] [OH-] = 10-14.

Using this information, we can calculate the pH of the solution.