r chromate is sparingly solübl 2. Silve in aqucous solutions. The Ksp of Ag2CrO4
ID: 541795 • Letter: R
Question
r chromate is sparingly solübl 2. Silve in aqucous solutions. The Ksp of Ag2CrO4 is 1.12x 10-12. What is the solubility (in mol/L) of silver chromate a) in 1.50 M potassium chromate aqueous solution? b) in 1.50 M silver nitrate aqueous solution? 3.Suppose a solution contains 0.23 M Pb2 and 0.41 M A13. Calculate the pH range minimum and maximum) that would allow Al(OH)3 to precipitate but not Pb(OH)2. The Ksp values for Al(OH)3 and Pb(OH)2 can be found here 4. Calculate the solubility of Mg(OH)2(s) in g/L in an aqueous solution buffered at pH 8.10. The Ksp of Mg(OH)2 is 5.61 x 10-12. 5. Suppose you have a solution that contains 0.0450 M Ca2 and 0.0910 M Ag If solid Na3PO4 is added to this mixture, which of the following phosphate species would precipitate out of solution first? When the second cation just starts to precipitate, what percentage of the first cation remains in solution? 6. Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and 0.0310 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag2SO4(s) begins to precipitate? Solubility- product constants, Ksp, can be found here. 7. The complex ion Cu(NH3)42 is formed in a solution made of 0.0500 M Cu(NO3)2 and 0.400 M NH3. What are the concentrations of Cu2NH3, and Cu(NH3)42 at equilibrium? The formation constant",Kf, of Cui NH342 is 1.70 × 1013 8. A 0.170-mole quantity of NiC12 is added to a liter of 1.20 M NH3 solution. What is the concentration of Ni2 ions at equilibrium? Assume the formation constant* of Ni(NH3)62 is 5.5 × 108 9. Calculate the value of the equilibrium constant for the following reaction: Pbl2(s)+21 (a)- Pbl4 2-(aq) Kc? The solubility product constant, Ksp, for PbI2 is 9.8x 10-9 and the overall formation constant, Kf(84), for Pbl42- is 3.0x 104 10.Copper(I) ions in aqueous solution react with NH3(aq) according to: Cu(a)+2NH3(a)> Cu(NH3)2n+ (aq) Kf-6.3x10^10 Calculate the solubility (in g L-1) of CuBr(s) (Ksp 6.3x 10-9) in 0.21 M NH3(aq).Explanation / Answer
Q2.
Ag2CrO4
Ksp = 1.1210^-12
a)
in 1.5 M of K2CRO4
[CrO4-2] = 1.5 M
Ksp = [Ag+]^2 * [CrO4-2]
1.1210^-12 = (2S)^2 * (1.5)
S = ((1.1210^-12)/(1.5)/4) ^0.5
S = 0.2057 M of Ag+
then,
[Ag2CrO4] = 1/2*[Ag+] = 1/2*0.2057 = 0.10285 M
b)
[AgNO3] = [Ag+] = 1.5
from
Ksp = [Ag+]^2 * [CrO4-2]
1.1210^-12 = (1.5)^2 * (S)
S= (1.1210^-12) / (1.5^2) = 0.112862
[Ag2CrO4] =0.112862M
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