Solutions

Question 1

What is the K_sp of a soluble salt with MX (ex: NaCl)?

Answer 1

K_sp = x²

x = Cation or Anion (Na⁺ or Cl^-)

Question 2

What is the K_sp of a salt with MX₂ (ex: PbI₂)?

Answer 2

K_sp = 4x³

x = Concentration of Pb²⁺

(x)(2x)2

Question 3

What is the K_sp of an MX₃ soluble

Answer 3

K_sp = 27x⁴

x = concentration of cation

Question 4

As K_sp increase….?

Answer 4

Solubility increases

Question 5

What is roults law?

Answer 5

P_A = X_AP^º_A

P_A = vapor pressure when solutes present

X_A = mole fraction of solvent A

P^º_A = Vapor pressure of A in pure state

Question 6

What do solutes do to evaporation? What about condensation?

Answer 6

blocks evaporation but not condensation

Question 7

What is M in the osmosis equation?

Answer 7

molarity

Question 8

What is the ion produce?

Answer 8

Current state of soluble products

for example if IP > K_sp the solution will be supersaturated and precipitate forms

Question 9

What happens if K_sp < IP?

Answer 9

The products will move toward saturation, the solution is unsaturated

Question 10

If K_f is formed by complex ions, what will happen to the K_sp?

Answer 10

It will be much higher (more soluble)

Question 11

When solutes are in a solution, the evaporation is blocked by solutes but it doesn’t do anything to condensation. What does this do cause?

Answer 11

Causes a decrease in vapor pressure