CHEM 2 CH 15 Q&A

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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


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