For the insoluble salt cadmium (II) iodate, the solubility product, Ksp, is 2.3 x 10-8.
a) Write the solubility product expression for cadmium (II) iodate.
b) Determine the molar solubility (M) of cadmium (II) iodate in pure water.
c) Calculate the solubility (M) of cadmium (II) iodate in a solution of 0.20 M Cd(NO3)2. Comment on whether the solubility has increased or decreased from part (b).
d) Predict whether the solubility of cadmium (II) iodate will increase or decrease if you add 0.10 M Na2S to the solution (knowing that S2- (aq) forms a precipitate of CdS (s) with Cd2+ (aq)).
For the insoluble salt cadmium (II) iodate, the solubility product, Ksp, is 2.3 x 10-8. a)...
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10×10−11 CdCO3 1.80×10−14 Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.20×10−2 M Fe2+ and 1.60×10−2 M Cd2+. What will the concentration of Cd2+ at the moment before Fe2+ begins to precipitate?
Silver phosphate, Ag3PO4, is an insoluble salt that has a Ksp = 1.3 x 10-20. a. Calculate the molar solubility of Ag3PO4 in pure water. b. Will the molar solubility of Ag3PO4 increase or decrease in a solution containing 0.020 M Na3PO4? c. Will a precipitate form if a solution is made by combining 3.0 x 10-5 M AgNO3 and 2.3 x 10-4 M Na3PO4? (hint: calculate Q)
At 25.0 degrees Celsius, the value of Ksp for cadmium (II) arsenate, Cd3(AsO4)2, is Ksp is 2.2X10^-33. a) Calculate the molar solubility (in mol/L) of cadmium (II) arsenate in water at 25.0 degrees celcius. b) Calculate the molar solubility in (mol/L) of cadmium (II) arsenate in a 0.200M solution of Cd(NO3)2 (aq) at 25.0 degrees Celsius.
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10×10−11 CdCO3 1.80× 10−14 Part C What will the concentration of Cd2+ at the moment before Fe2+ begins to precipitate? Express your answer with the appropriate units.
Calcium fluoride, CaF2, is an insoluble salt (Ksp = 1.46 x 10-10) that can be formed by precipitation by mixing solutions of calcium nitrate and sodium fluoride. Suppose 200.0 mL of a 0.600 M Ca(NO3)2(aq) solution are mixed with 400.0 mL of a 0.0600 M NaF(aq) solution. Will a precipitate form? How much calcium fluoride could form?
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10×10−11 CdCO3 1.80× 10−14 A solution of Na2CO3 is added dropwise to a solution that contains 1.00×10−2 M Fe2+ and 1.49×10−2 M Cd2+. What concentration of CO32− is need to initiate precipitation? Neglect any volume changes during the addition.
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10×10−11 CdCO3 1.80×10−14 A solution of Na2CO3 is added dropwise to a solution that contains 1.21×10−2MFe2+ and 1.45×10−2M Cd2+. What concentration of CO32− is need to initiate precipitation? Neglect any volume changes during the addition. Express the molar concentration numerically.
Suppose the solubility product constant of calcium iodate is 6.47 x 10-6. If the concentration of calcium iodate is 0.45 M. What would be the concentrations of Ca2+ and IO3- at equilibrium? Would this solution form a precipitate? Is the solution unsaturated, saturated, or supersaturated? Note* Ksp = [Ca2+][IO3-]2
At 25 0C the solubility product constant, Ksp, for strontium sulfate, SrSO4, is 7.6 x 10-7. The solubility product constant for strontium fluoride, SrF2, is 7.9 x 10-10. (a) What is the molar solubility of SrSO4 in pure water at 25 0C? (b) What is the molar solubility of SrF2 in pure water at 25 0C? (c) An aqueous solution of Sr(NO3)2 is added slowly to 1.0 litre of a well-stirred solution containing 0.020 mole F- and 0.10 mole SO42-...
Find Ksp The generic metal A forms an insoluble salt AB(s) and a complex ACs(aq). The equilibrium concentrations in a solution of ACs were found to be (A) = 0.100 M, [C] = 0.0140 M, and [ACs) = 0.100 M. Determine the formation constant, K, of AC5. Number K,= 1.86 x 10 The solubility of AB(s) in a 1.000-M solution of C(aq) is found to be 0.175 M. What is the Ksp of AB? Number