22) Given the following hydroxides and their solubility product constants, which

Question

22) Given the following hydroxides and their solubility product constants, which would be the most soluble in 1.0 L of water?

A) Magnesium hydroxide; Ksp=1.2x10-11

B) Iron(II) hydroxide;Ksp=1.6x10-14

C) Zinc hydroxide;Ksp=1.8x10-14

D) Copper (II) hydroxide; Ksp=2.2x10-20

E) Calcium Hydroxide; Ksp=8.0x10-6

23) Consider the equilibrium of AgCl(s) in water: AgCl(s) ??Ag+ Cl- What is the effect of adding 6.5x10-3 M AgNO3?

a) The concentration will AgCl(s) will increase

b) The concentration will AgCl(s) will decrease

c) AgNO3 will precipitate

d) Silver dichloride precipitates

e) The AgNO3 has no effect on the solubility of AgCl

29) The Ksp of Mg(OH)2 is 3.6x10-4. At what pH will 0.2 M Mg+2 solution begin to show precipitation? 1.4, 2.8, 10.7, 11.2, 12.6

27) The solubility product for calcium phosphate is Ksp=1.36 x 10-26. What is the molar solubility of calcium phosphate? 1.3X10-26M, 1.5x10-7M, 2.6x10-6M, 4.6x10-6M, 6.6x10-6M  Show work, explain or no points

Explanation / Answer

22) Given the following hydroxides and their solubility product constants, which would be the most soluble in 1.0 L of water?

B) Iron(II) hydroxide;Ksp=1.6x10-14

23) Consider the equilibrium of AgCl(s) in water: AgCl(s) ??Ag+ Cl- What is the effect of adding 6.5x10-3 M AgNO3?

c) AgNO3 will precipitate

29) The Ksp of Mg(OH)2 is 3.6x10-4. At what pH will 0.2 M Mg+2 solution begin to show precipitation?

10.7,

27) The solubility product for calcium phosphate is Ksp=1.36 x 10-26. What is the molar solubility of calcium phosphate?

1.3X10-26M,

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