Achieve Week 2&3 #2

[andrea guzman 1F]

The Ka of a monoprotic week acid is 0.00577. What is the percent ionization of a 0.198 M solution of the acid?

I keep getting variations of 17% how do I go about solving this question do I need to use the quadratic equation?

[106046096]

Hi! You would first make an ice table for the equation HA -> H+ + A- with your 0.198 M being the initial for HA and your change being -x for HA and +x for H+ and A-. You can now make your equilibrium constant equation, which will be [H+][A-]/[HA], and plug in your values and solve for x. To get percent ionization, divide [H+] at equilibrium by [HA] at initial and multiply the value by 100.

[306060519]

You need to use the formula entitled [H+][A-]/[HA].