In: Chemistry
1.8 grams of ammonia, NH3 (M=18 g/mol), is dissolved in 10L of water. Which best approximates the pH of the solution? Please explain/show work.
The answer is 7-11.9, but I got 12 and was wondering why it's less than that.
mass of NH3= 1.8 grams
molar mass of NH3= 18 g/mole
number of moles NH3= mass/molar mass = 1.8/18=0.1 mole
Volume = 10.0L
Molarity = number of moles/volume = 0.1/10= 0.01 M
NH3 + H2O -------------------- NH4+ + OH-
0.01 0 0
-x +x +x
0.01-x +x +x
Kb of NH3 = 1.8x10^-5
kb = [NH4+][OH-]/[NH3]
1.8x10^-5 = x*x/(0.01-x)
for solving the quation
x= 0.000415
[OH-] = 0.000415M
-log(OH-)= -log(0.000415)
POH= 3.38
PH+POH=14
PH= 14-POH
PH= 14-3.38
PH= 14 - 3.38
PH= 10.62.