Chapter 17 Quizizz Part 2

The K_sp value for PbF₂ is 4 x 10^-8. Calculate the molar solubility of solid PbF₂ in a 0.5M NaF solution.

• 8.0 x 10^-9

• 5.2 x 10^-7

• 8 x 10^-8

• 1.6 x 10^-7

if K_sp < Q_sp then

• no precipitate will form

• precipitate will form

• the reaction will not occur

• the reaction will remain saturated

Does a precipitate form when 0.050 L of 2.0x10^-2M Pb(NO₃)₂ is mixed with 0.010 L of 1.0x10^-2M Na₂SO₄? (PbSO₄ has a Ksp = 3 x 10^-28)

• Yes Q_sp = 2.84x10^-5

• No Q_sp = 2.84x10^-35

• Yes Q_sp = 3.14x10^-5

• No Q_sp = 3.14x10^-35

Ksp for CaF₂ is 3.9x10^-11 mol/L. If 50 mL of 0.025 M CaBr₂ is mixed with 40 mL of 0.030 M NaF, will a precipitate occur?

• Yes, Q = 2.4x10^-6

• Yes, Q = 9.8x10^-5

• Yes Q = 1.85x10^-3

• No, Q = 4.6x10^-12

How do you expect the solubility to be affected when NaClO₂ is dissolved in HCl vs pure water?

• It will be more soluble in HCl, because ClO₂^- is removed from the equilibrium

• It will be less soluble in HCl becuase ClO₂^- is removed from the equilibrium

• It will be less soluble in HCl because H⁺ is added to the equilibrium

• It will not affect the solubility of NaClO₂

How will the solubility of BaSO₄ be affected by the addition of H₂SO₄ to the solution?

• Solubility will increase

• Solubility will decrease

• Solubility will not be affected

K_sp for PbF₂ is 4.0 ×10^–8. If a 0.032 M NaF solution is saturated with PbF₂, what is [Pb²⁺] in solution?

• 4.1x10^-11 M

• 1.3x10^-9 M

• 3.9x10^-5 M

• 1.2x10^-6 M

hat is the minimum mass of Na₂CO₃ that must be added to 75.9 mL of a 9.0 × 10^–4 M AgNO₃ solution in order for precipitation to occur? For Ag₂CO₃, K_sp = 8.6 × 10^–12

• 7.2x10^-3 g

• 8.5x10^-5 g

• 3.1x10^-4 g

• 8.9x10^-6 g