CHEM 2 CH 15 Q&A
If the equilibrium concentration of Ag+ is x, what would be the equilibrium concentration of SO4 ^2-? Given: Ag2SO4 (s) === 2Ag + (aq) + SO4 -2 (aq)
+x/2
Calculate the molar solubility of AgCl in water. Ksp = 1.6x10 -10
0.000013 M
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of PbI2 in water. Ksp = 1.4x10 -8
0.00152 M
The Ksp of calcium hydroxide, Ca(OH)2, is 1.3 × 10-6. Calculate the molar solubility of calcium hydroxide.
0.0069 M
The Ksp value for lead(II) iodide is 2.4 × 10-4. What is the molar solubility of lead(II) iodide?
0.039 M
Calculate the concentration of chloride ions in a saturated lead(II) chloride (Ksp = 2.4 × 10-4) solution.
0.078 mol/L
The solubility product for calcium sulfite is 1.1 × 10-10. Calculate the molar solubility of calcium sulfite.
1.1 × 10-5 M
The solubility of lead(II) iodide is 0.064 g/100 mL at 20ºC. What is the solubility product for lead(II) iodide?
1.1 × 10-8
A saturated sodium carbonate solution contains 7.1 g of dissolved sodium carbonate per 100. mL of solution. What is the Ksp for sodium carbonate?
1.2
The solubility product for a compound MCl3 is Ksp = 6.6 × 10-11. What is the molar solubility of MCl3?
1.2 × 10-3 M
The Ksp for copper(I) phosphate is 1.8 × 10-18. Calculate the molar solubility of copper(I) phosphate.
1.6 × 10-5 mol/L
What is the molar solubility of CaF2(s) in 0.00133 M KF? Ksp = 4.0x10 -11
2.3x10^-5 M
Calculate the copper ion concentration in a saturated solution of copper(I) carbonate if Ksp = 8.1 × 10-12.
2.5 × 10-4 mol/L
The molar solubility of lead(II) bromate in water is 4.0 × 10-5 mol/L. Calculate Ksp for lead(II) bromate.
2.6 × 10-13
The solubility product for calcium phosphate is Ksp = 1.3 × 10-26. Calculate the molar solubility of calcium phosphate.
2.6 × 10-6 M
If the equilibrium concentration of Mg 2+ is x, what will be the equilibrium concentration of PO4 3-? Given: Mg3(PO4)2 (s) === 3Mg +2 (aq) +2 PO4 -3 (aq)
2/3 x
The molar solubility of barium carbonate is 1.8 × 10-4 mol/L. What is Ksp for this compound?
3.2 × 10-8
When solid lead(II) phosphate is in equilibrium with its ions, the ratio of lead(II) ions to phosphate ions is.................
3:2
Calculate the molar solubility of Mg(OH)2 in a solution with pH = 12.20. Ksp (Mg(OH)2 = 1.2 x 10-11
4.8 x 10-8 M
What is the molar solubility of Zn(OH)2(s) in a solution at a pH of 11.45? Ksp = 4.5x10 -17
5.7x10^-12 M
Calculate the molar solubility of MgF2 in a 0.25 M solution of LiF(aq). Ksp (MgF2) = 4.0 x 10-11
6.4 x 10-10 M
Calculate the molar solubility of AgCl in 0.025 M NaCl. Ksp = 1.6x10 -10
6.4x10^-9 M
Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. MgF2 , Ksp = 6.9 × 10-9
6.9 × 10-7 M
Calculate the molar solubility of MgCO3 in a 0.10 M solution of Na2CO3(aq). Ksp (MgCO3) = 8.1 x 10-9
8.1 x 10-8 M
Which one can be considered as Lewis acid?
Ag+
Choose the correct Ksp expression for the dissolution of Ag2SO4.
Ksp = [Ag+ ]2 [SO4-2]
Choose the correct Ksp expression for the dissolution of LaF3.
Ksp = [La3+ ] [F-]3
Choose the correct Ksp expression for the dissolution of Pb(OH)2.
Ksp = [Pb+2 ] [OH-]2
At given temperature which of the following would decrease the Ksp for PbBr2?
Ksp does not change.
When Mg(OH)2 dissolves in water, what ions are formed?
Mg^2+ and OH^-
Which one can be considered as Lewis base?
NH3
Will a precipitate of magnesium fluoride form when 300. mL of 1.1 × 10-3 M MgCl2 are added to 500. mL of 1.2 × 10-3 M NaF? Ksp (MgF2) = 6.9 × 10-9
No, Q < Ksp
How do the concentrations of Ag+ and CrO4 2- in a saturated solution above 1.0 g of solid Ag2CrO4 change when 100 g of solid Ag2CrO4 is added to the system?
There is no change.
Will a precipitate of magnesium fluoride form when 200. mL of 1.9 × 10-3 M MgCl2 are added to 300. mL of 1.4 × 10-2 M NaF? Ksp (MgF2) = 6.9 × 10-9
Yes, Q >Ksp
In a saturated solution of silver phosphate, the concentration of Ag+ is 45.x10 -6 M. What is the Ksp of silver phosphate?
none of the above
If the equilibrium concentration of Ag+ is x, what would be the equilibrium concentration of Cl-? AgCl (s) === Ag + (aq) + Cl - (aq)
x
