etermine the ammonia concentration of an aqueous solution that has a pH of 11 he
ID: 587160 • Letter: E
Question
etermine the ammonia concentration of an aqueous solution that has a pH of 11 he dissociation of NH3 (Kb = 1.8 × 10-5) is NH3(a) H20()NH4 (aa)+ OH-(aq) (0.056 M) Calculate the pH of a 0.020 M carbonic acid solution, H2CO3(a), that has the s stants Kal-4.3x 10-7 and Ka2 = 5.6 × 10-11 . 36. What is the pH of a 0.20 M solution of NHC1 [KbNHs)-1.8 x 10 ] 37. Which one of these salts will form a basic solution upon dissolving in wate (pH 4.03) A) NaCl B) NaNO2 C) NH4NO3 D) KBr E) AlCl3 Write the reaction of these compounds with water. Which one of the following tion in water? Why? A) NH4ClExplanation / Answer
What is the pH of a 0.020 M solution of NH4Cl? [Kb(NH3)= 1.8 * 10^-5]
NH4Cl(aq) ---------------------------> NH4^+ (aq) + Cl^- (aq)
0.02M 0.02M
cationic hydrolic is takes place
NH4^+ (aq) + H2O ---------------------> NH3(aq) + H3O^+
I 0.02 0 0
C -x +x +x
E 0.02-x +x +x
Kb = 1.8*10^-5
Ka = Kw/Kb
= 1*10^-14/1.8*10^-5 = 5.6*10^-10
Ka = [NH3][H3O^+]/[NH4^+]
5.6*10^-10 = x*x/0.02-x
5.6*10^-10 *(0.02-x) = x^2
x = 3.35*10^-6
[H3O^+] = x = 3.35*10^-6M
PH = -log[H3O^+]
= -log3.35*10^-6
= 5.4749 >>>>>answer
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.