Calculate the maximum concentration (in M) of silver ions in a solution that con
ID: 968284 • Letter: C
Question
Calculate the maximum concentration (in M) of silver ions in a solution that contains 0.025 M of CO3 ^ 2-. The Ksp of Ag2CO3 is 8.1 x 10^ -12.
Would it be:
a) 8.1 x 10 ^ -12
b)1.4 x 10^ -6
c) 3.2 x 10 ^ -10
d) 2.8 x 10 ^ -6
e) 1.8 x 10 ^ -5
Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.300 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 x 10 ^ -5.
Would it be:
a) 4.300
b) 5.204
c) 9.700
d) 8.796
e) 8.781
A solution contains 2.3 x 10 ^ -4 M Ag+ and 1.7 x 10 ^ -3 M Pb^2+.
Part 1: If NaI is added, will AgI; Ksp 8.3 x 10 ^-17 or PbI2; 7.9 x 10 ^ -9 precipitate first?
a) AgI will precipitate first
b) PbI will precipitate first
Part 2: Specify he concentration of I needed to begin precipitation.
The Kb of ammonia is 1.76 x 10^-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 25.0 mL of 1.00 M ammonium nitrate is ________.
Would it be:
a)9.372
b) 4.742
c) 9.547
d) 4.632
e) None of the above
The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 55.0 mL of 0.145 M HCl is ______.
a)0.00824
b)11.423
c)2.577
d)12.923
e)1.314
What is the pH of a buffer solution that is 0.185 M in lactic acid and 0.132 M in sodium lactate? The Ka of lactic acid is 1.4 x 10 ^ -4.
Would it be:
a)10.30
b)4.00
c)3.70
d)14.15
e)5.47
Explanation / Answer
Calculate the maximum concentration (in M) of silver ions in a solution that contains 0.025 M of CO3 ^ 2-. The Ksp of Ag2CO3 is 8.1 x 10^ -12.
Ksp = [Ag+2]^2[CO3-2]
(8.1*10^-12) = (Ag+)^2(0.025)
[Ag+] = sqrt((8.1*10^-12)/(0.025)) = 0.000018 M = 1.8*10^-5 M
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