Answer to Question #349490 in General Chemistry for hailey

Question

An aqueous solution of HF is added to an aqueous solution of K(OH) and a reaction occurs. The

concentration of H + ions is 2.68x10 -1 M. Calculate the concentration of the (OH) - ions. Is the solution

more acidic or basic?

Answer 1

Solution:

[H⁺] = 2.68×10^−1 M

We can convert between [H⁺] and pH using the following equations:

pH = −log[H⁺]

pH = −log(2.68×10^−1) = 0.57

pH = 0.57

Any solution that has a pH of less than 7 is considered acidic

For any aqueous solution at 25^∘C:

[H⁺] × [OH^−] = K_w = 1.0×10^−14

Therefore,

[OH^−] = K_w / [H⁺]

[OH^−] = (1.0×10^−14) / (2.68×10^−1) = 3.73×10^−14

[OH^−] = 3.73×10^−14 M

Answer:

The concentration of hydroxide ions (OH^−) is 3.73×10^−14 M

The solution is acidic