unit 6 ib chem

Solute

Substance being dissolved

Solvent

Substance doing the dissolving

Solution

Solute and solvent combined

Solubility

The amount of solute that can be dissolved in a given amount at a certain temperature

Unsatured

More solute can be dissolved

Saturated

No more solute can be dissolved

Supersaturated

No more solute than the maximum amount can be dissolved

Immiscible

Liquids that are insoluble in one another

Miscible

Liquids that can dissolve into eachother

Solubility of Non-Polar solutes

• Soluble in non-polar solvents

• Insoluble in polar solvents

Solubility of Polar and Ionic solutes

• Soluble in polar solvents

  • Insoluble in non-polar solvents

4 factors that affect solubility

• Stirring - increases solubility rate

• Particle size - smaller the particle the faster it dissolves

• Temperature - Solids increase solubility as temperature increases and gases decrease solubility as temp increases

• Pressure - Solids have little effect on solubility and gases increase solubility as pressure increases (Henry’s law)

Above, On, and Below the line in solubility curves. What does it mean?

Above the curve - supersaturated

On the line - saturated

Below the line - unsaturated

What are the three colligative properties

• Vapor Pressure Lowering

• Boiling point elevation

• Freezing point depression

Vapor Pressure Lowering

• More particles/ions in solution decrease vapor pressure

• Less particles/ions in solution increase vapor pressure

Boiling Point Elevation

• More particles/ions increases BP

• Less particles/ions lowers BP

Freezing Point Depression

• More ions/particles decrease freezing point

• Less ions/particles increase freezing point

What is 1 dm³ equal to?

1000 cm³

Rules of Equilibrium

Adding a catalyst: no effect

Equilibrium constant: no effect

How does pressure work in an equilibrium

If pressure is increased, the equilibrium shifts towards the side with fewer moles.

if pressure is decreased, the equilibrium shifts towards the side with more moles.

Where is heat in an endothermic reaction?

Heat is a reactant / heat is positive kJ

Where is heat in an exothermic reaction?

Heat is a product / heat is negative kJ

6 properties of Acids

• Sour

• Conduct electricity

• Strong/weak electrolytes

• React w/ metals to form H2 gas

• React w/ OH bases to form water and a salt

• Turns blue litmus paper red

6 properties of bases

• Bitter

• Slippery

• Conduct electricity

• Strong/weak electrolytes

• React with acid to form water and a salt

• Turn red litmus paper blue

How do strong acids/bases act in solutions?

They completely dissociate/ionize

How do weak acids/bases act in solutions?

They partially/barely dissociate/ionize

Arrhenius Definitions

• Acids produce H+ in aqueous solutions

• Bases produce OH- when dissolved in water

Bronsted-Lowry Definitions

• Acids donate hydrogen ions (protons)

• Bases accept hydrogen ions (protons)

What is a pH < 7

acidic

What is a pH > 7

basic

What is a pH = 7

neutral

Formulas to find pH/pOH when concentration (M) is given

-log[H+]

pH + pOH = 14

Formulas to find concentration when pH is given

10^-(pH)

10^-(pOH)

[H+][OH-] = 1 × 10^-14

Equation to find uncertainties when doing multiplication/division

(uncertainty/measurement) x 100

How to find uncertainty when adding or subtracting

Add the uncertainties