In: Chemistry
What mass of sodium nitrite must be added to 350 mL of water to give a solution with a pH = 8.40? (Ka (HNO2) = 5.6 x 10-4)
PH = 8.4
POH = 14-PH
= 14-8.4
= 5.6
-log[OH^-] = 5.6
[OH^-] = 10^-5.6 = 2.5*10^-6 M
Kb = Kw/Ka
= 1*10^-14/5.6*10^-4 = 1.78*10^-11
NaNO2(aq) --------------> Na^+ (aq) + NO2^- (aq)
NO2^- (aq) + H2O ----------------> HNO2(aq) + OH^- (aq)
I x 0 0
C -2.5*10^-6 2.5*10^-6 2.5*10^-6
E x-2.5*10^-6 2.5*10^-6 2.5*10^-6
Kb = [HNO2][OH^-]/[NO2^-]
1.78*10^-11 = 2.5*10^-6*2.5*10^-6/(x-2.5*10^-6)
1.78*10^-11 *(x-2.5*10^-6) = 2.5*10^-6*2.5*10^-6
x = 0.35
molarity = 0.35M
no of moles of NaNO2 = molarity *volume in L
= 0.35*0.35 = 0.1225 moles
mass of NaNO2 = no of moles * gram molar mass
= 0.1225*69 = 8.4525g >>>>>>>>answer