GC question

[Troyvdg]

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For some reason I keep getting the same answer, could someone walk me through this?

An unknown weak monoprotic acid, HY, is found to be 0.002% ionized in a 1.0 M aqueous solution. What is the Ka of HY?

a. 2 x 10^-3
b. 4 x 10^-6 what I keep getting
c. 4 x 10^-10 answer
d. 2 x 10^-5
e. 2 x 10^-10

Thanks for the help!

 

[HossIX949]

Percent Ionization is defined as: (molarity of H+ derived from HA/initial molarity of HA) X 100 = %.

.002 % = (molarity of H+ derived from HY/1.0 M (aq) of HY ) X 100

molarity of H+ derived from HY = 0.00002 M (2 x 10^-5)

HY --> H+ + Y-

Ksp = [H+][Y-]/[HY] NOTE: [H+] = [Y-] = 2 x 10^-5 M

Ksp = [2 x 10^-5 M]^2/ [1]

Ksp = 4.0 X 10-10

 

[Troyvdg]

Percent Ionization is defined as: (molarity of H+ derived from HA/initial molarity of HA) X 100 = %.

.002 % = (molarity of H+ derived from HY/1.0 M (aq) of HY ) X 100

molarity of H+ derived from HY = 0.00002 M (2 x 10^-5)

HY --> H+ + Y-

Ksp = [H+][Y-]/[HY] NOTE: [H+] = [Y-] = 2 x 10^-5 M

Ksp = [2 x 10^-5 M]^2/ [1]

Ksp = 4.0 X 10-10

thanks 👍 I just realized that I forgot that .002 was a percentage

 

[HossIX949]

No problem 🙂. Glad it helped.