Amount of NaNO2 added = 2.31 g
Amount of water = 253.00 mL = 0.253 L
Molarity of NaNO2 solution = (2.31/69)/0.253 = 13.23 M
Kb = 2.2 x 10-11
NO2- + H2O ----> HNO2 + OH−
Iintial 13.23 0 0 0
Equil. 13.23-x 0 x x
Kb = (x) (x)/ (13.23-x)
2.2 x 10-11 = x2/13.23
x2 = 2.91 x 10-10
x = 1.705 x 10-5 = [OH-]
[H+] = Kw/[OH-] = 1.0 x 10-14/1.705 x 10-5 = 0.586 x 10-9 = 5.86 x 10-8
pH = -log [H+] = - log 5.86 x 10-8 = 8- log 5.86 = 8 - 0.767 = 7.23 ≈ 7.27
A 0.685 M solution of a weak acid HA has a pH of 4.50. What is the percent ionization of HA in the solution? Submit Answer Tries 0/98 For the solution described above, what is the K,? Submit Answer Tries 0/98 This discussion is closed. Ote E o Type here to search 6