Solubility

Question 1

Solubility of Compound

Answer 1

• Dependent on physiochemical properties: physical/chemical of solute and solvent
• Influenced by temperature, pressure, and pH

Question 2

Solute-Solvent Interactions: Polar Solvents

Answer 2

• Ionic solutes and polar substances
• Decrease attractive forces between opposite charged ions
• Break covalent bonds of potentially strong electrolytes by acid-base reactions
• Form H-bonds for partial solubility of weak acids to ratio of polar:non-polar

Question 3

Semi-Polar Solvents

Answer 3

-Water = most polar
-Then ketones and alcohols (polyethylene glycol 400 => glycerol)
Then olive oil and octane are non-polar

Question 4

Solute-Solvent Interactions: Semi-Polar

Answer 4

• Dissolve ionic solutes and polar substances
• Ketones and alcohols induce a degree of polarity
• Utilize solvent blending of different polar solvents to create an optimum polarity to dissolve the solute (must all be miscible)
• Use dielectric constant to guide systemic development

Question 5

Completely Miscible

Answer 5

Solvents mix completely in all proportion

Question 6

Partial Miscible

Answer 6

• Certain amounts of 2 liquids form distinct phases which each contain some of the other liquid in dissolved state
• Influenced by temperature, surface area of solute, etc.

Question 7

Immiscible

Answer 7

No mixing of liquids at all

EX: octane and water

Question 8

Temperature Review

Answer 8

• 0 K = -273 degrees C, absolute zero
• Freezing point (Water) = 0 degrees C or 273K
• Standard room temperature = 20 degrees Celsius or 293K
• Boiling point (water) = 100 degrees Celsius, or 373 K

Question 9

Ideal Solubility of Solids in Liquid

Answer 9

• Review equation on PowerPoint

- When T>To the equation no longer applies since the solute is liquid and miscible in all proportions

Question 10

Solubility Product

Answer 10

• Describe solubility of slightly soluble electrolyte in water to make saturated solution
• Ksp = [Ag+][Cl-] (example for AgCl)
• If [Ag][Cl] is larger than Ksp then the solid will precipitate
• *Know how to calculate this value and interpret these values**

Question 11

Common Ion Effect

Answer 11

• Addition of common ion to decrease the solubility of slightly soluble electrolyte
• Net result is a reduction in solubility of compound since precipitates are created to reach equilibrium again
• Salts with no common ions at moderate concentrations increase solubility
• *Know how to calculate and interpret these values**