Question

a.A saturated solution has:

a. so much solute that it may spontaneously crystallize out

b.enough solute so that some precipitate remains undissolved

c.the ability to absorb easily much more solute

d.the maximum solute that can dissolve in it

b. In which solution will 0.010 M F- remain soluble?

a. 0.020 M Ba2+ (Ksp of BaF2=1.7x10-6)

b. 4.0x10-7 M Ca2+ (Ksp of CaF2=3.9x10-11)

c. 3.0x10-13 M La3+ (Ksp of LaF3=2x10-19)

d. 0.00030 M Pb2+ (Ksp of PbF2=3.6x10-8)

c. Which can be an Arrhenius, Brønsted-Lowry, and Lewis acid?

a. NH3(aq)

b. CO2(g)

c. CH3NH2(aq)

d. H3O+(aq)

d. The Lewis acid-base concept explains better than other concepts the acid-base nature of

a. proton acceptors

b. carboxylic acids

c. alkali metals

d. transition metal ions

Answer 1

a)

Correct option: d. the maximum solute that can dissolve in it

A saturated solution has the maximum amount of solute that can dissolve in it. Any additional solute will remain undissolved.

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b)

Correct option: d. 0.00030 M Pb²⁺ (K_sp of PbF₂=3.6x10^-8)

Ionic product, Q_sp of BaF₂ = [Ba²⁺][F^-]² = (0.020)(0.010)² = 2.0 x 10^-6

Ionic product, Q_sp of CaF₂ = [Ca²⁺][F^-]² = (4.0x10^-7)(0.010)² = 4.0 x 10^-11

Ionic product, Q_sp of LaF₃ = [La³⁺][F^-]³ = (3.0x10^-11)(0.010)³ = 3.0 x 10^-17

Ionic product, Q_sp of PbF₂ = [Pb²⁺][F^-]² = (0.00030)(0.010)² = 3.0 x 10^-8

For 0.00030 M Pb²⁺solution Q_sp < K_sp. Hence, in 0.00030 M Pb²⁺, 0.010 M F^- will remain soluble