Lab Section: 3. Determine the K, and pK, (to two decimal places) for an aqueous
ID: 544795 • Letter: L
Question
Lab Section: 3. Determine the K, and pK, (to two decimal places) for an aqueous solution containing 0.19 M of a weak, monoprotic acid, HA, with a pH of 5.10. HA(aq) + H20 (r) t H30+ (aq) + A- A: 3.32x 10-10,9.48 4. The K, for the acetie acid (CHiCo,H) is i8x 10-9. What is the K, (to two decimal places) for its conjugate base (at 25°C)? A: 556×10-10 5. What is the percent ionization (to two decimal places) of a 0.50 M HNO2 aqueous solution? HNO2 (aq) + H20 () HO+ (aq) + No5 Ka (HNO) 460 x 10-4 , A:3.03%Explanation / Answer
3)
use:
pH = -log [H3O+]
5.1 = -log [H3O+]
[H3O+] = 7.943*10^-6 M
HA dissociates as:
HA -----> H+ + A-
0.19 0 0
0.19-x x x
Ka = [H+][A-]/[HA]
Ka = x*x/(c-x)
Ka = 7.943*10^-6*7.943*10^-6/(0.19-7.943*10^-6)
Ka = 3.32*10^-10
use:
pKa = -log Ka
= -log (3.32*10^-10)
= 9.48
Answer:
Ka = 3.32*10^-10
pKa = 9.48
4)
use:
Kb = (1.0*10^-14)/Ka
Kb = (1.0*10^-14)/1.8*10^-5
Kb = 5.56*10^-10
Answer: Kb = 5.56*10^-10
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