Chemistry (Acids and Bases)

Question 1

Solute and Solvent

Answer 1

Solute dissolved + phase change

Solvent in greater amount

Question 2

Solubility Factors

Answer 2

Measure of how much something dissolves

• Solute in liquid or liquid in liquid. Temp inc.= Solubility inc.
• Gas in liquid. Temp inc. Solubility dec.
• Polarity: polar dissolves polar and non-polar dissolves non-polar
• Size: Size inc. solubility dec.

Question 3

Precipitation

Answer 3

Add too much compound and hits solubility limit/saturation

• solute drops out of solution.
• liquid-liquid undergo phase split => 2 liquid phases with least dense on top.

Question 4

Units of concentration

Answer 4

Percentage composition: mass of x/ total mass or moles of x/total moles

Molarity: moles of solute / liters of solution.

Molality: moles of solute/ kg of solvent.

Normality: Equivalents of X/ liters of solution.

Question 5

Mole fraction

Answer 5

Moles/ total moles

Question 6

Oxidation numbers

Answer 6

• Pure elements =0
  e. g Zn, O₂, F₂

Ions
Zn ²+—> +2
Fe ³+—> +2
Hg₂ ²+—> +1 for each Hg atom
O ₂ ²- (peroxide)—> -1
O ₂ ¹-

Compounds
F=-1
O=-2
H is +1 with nonmetal and -1 with metal.

Examples
MgCl ₂= +2 + 2(-1)= 0
AlF ₃= +3 + 3(-1)= 0
SO4 ²- = 6 + 4(-2) = 2-

Question 7

Dilutions

Answer 7

Calculating # of moles in a system and divide by total volume.

M1V1=M2V2

Question 8

Solubility product Ksp

Answer 8

• Extent to which a solid dissolves.
• Will only be used for salts with a low solubility.

Ksp= [Products] => concentrations of the ions that are formed when the solid dissociates

Question 9

Common Ion Effect and Molar solubility

Answer 9

What if there is already common ion present between the solute added and substance already dissolved in the water—> common ion effect

Molar solubility: amount of solute required to reach saturation.

Question 10

Ksp and Qsp

Answer 10

Ksp > Qsp: unsaturated (no precipitate)

Ksp = Qsp: equilibrium ( no precipitate)

Ksp< Qsp: past saturation (precipitate will form until equilibrium)

Question 11

Lewis, Bronsted-Lowry, and Arrhenius

Answer 11

Bronsted-Lowry Acid: proton donor
Bronsted-Lowry Base: proton acceptor

Arrhenius Acid: Release H+ in solution
Arrhenius Base: Release OH- in solution

Lewis Acid: Electron pair acceptor
Lewis Base: Electron pair donor

Question 12

Titrations

Answer 12

Finding concentration of unknown substance