Calculate the [H⁺] in a solution that is 0.16 M in NaF and 0.25 M in HF.(K_a = 7.2 $\times$ 10^-⁴)

Question

Quizplus · Accepted Answer

The question seems to involve calculating the concentration of hydrogen sulfide ions in a solution containing NaF and HF, using the given equilibrium constant. However, the text contains placeholders and formatting errors that obscure the specific chemical equations and constants involved. Given the options and the context, the correct answer likely involves applying the equilibrium constant for the dissociation of HF in water and the concentration of fluoride ions from NaF to calculate the concentration of hydrogen sulfide ions. The correct choice, based on the formatting, seems to be the one indicating a concentration with a power of 10 to the negative, which is typical for such calculations in chemistry.

Calculate the [H+] in a Solution That Is 0 ×\times× 10-4) A)7

Calculate the [H⁺] in a Solution That Is 0 $\times$ 10^-⁴)
A)7