Question #a8da2
1 Answer
The pH of the solution is
Explanation:
To solve this problem, you need the value of the base dissociation constant of ammonia,
Since ammonia is a weak base, it will increase the concentration of
Use the ICE table (more here) to solve for the concentration of
#" " " ""NH"_ (3(aq)) + "H"_ 2"O"_ ((l)) rightleftharpoons "NH" _ (4(aq))^(+) + "OH" _((aq))^(-)#
#"I"color(white)(aaaaacolor(black)(0.15)aaaaaaaaaaaaaaaa color(black)(0) aaaaaaa color(black)(0)#
#"C"color(white)(aaaaacolor(black)(-x)aaaaaaaaaaaaaaa color(black)(+x) aaaaa color(black)(+x)#
#"E"color(white)(aaacolor(black)(0.15-x)aaaaaaaaaaaaaa color(black)(x) aaaaaaa color(black)(x)#
Use the definition of the base dissociation constant
#K_b = (["OH"^(-)] * ["NH"_4^(+)])/(["NH"_3])#
#1.8 * 10^(-5) = ( x * x)/(0.15 - x) = x^2/(0.15-x)#
Because
#0.15 - x ~~ 0.15#
You will have
#1.8 * 10^(-5) = x^2/0.15#
#x = sqrt(0.15 * 1.8 * 10^(-5))#
#x = 0.001643#
This means that you have
#["OH"^(-)] = "0.001643 M"#
The solution's
#"pOH" = - log(["OH"^(-)])#
#"pOH" = -log(0.001643) = 2.78#
Therefore, the
#"pH" = 14 - "pOH"#
#"pH" = 14 - 2.78 = color(green)(11.22)#