Solutions - Honors Chemistry

solution

homogeneous mixture of 2 or more substances

Solute

substance being dissolved

Solvent

substance doing the dissolving

solution

solute + solvent

aqueous solution

solute + water is the solvent

dissolve

COVALENT compounds breaking up into molecules and atoms

dissociate

IONIC compounds breaking up into ions

miscible

2 LIQUIDS ABLE to mix together

immiscible

2 LIQUIDS UNABLE to mix together

homogeneous

same look

transparent

clear but not always colorless

suspended

particles suspended in solution

separation

particles can’t be filtered; can be separated by evaporation, distillation

gases

2 or more gases

solids

2 or more solids (Alloy - solid solution of 2 or more metals)

liquids

gases, solids, liquid dissolved in a liquid

solubility

ABILITY to dissolve in a solvent

factors that affect solubility

polarity, pressure, temperature

polarity affecting solubility

polar - ionic solids dissolve in water; nonpolar - covalent substances dissolve in oils

pressure affecting solubility

solids and liquids - has NO affect; gases - increase in pressure increase in solubility

temperature affecting solubility

solids and liquids - increase temp increase solubility; gases - decrease temp increases solubility

dissolution

how FAST a substance can dissolve in a solvent

factors that affect dissolution

temperature, agitation, surface area, saturation

temp affecting dissolution

solids and liquids - increase temp increase ROD; gases - decrease temp increase ROD

agitation affecting dissolution

increase agitation increase ROD

surface area affecting dissolution

increase surface area increase ROD

saturation affecting dissolution

increase saturation decrease ROD

saturation

when solution is unable to absorb any more solute it’s saturated

unsaturated

solution can hold solute at that temp

saturated

solution can hold exact amount of solute it can hold at that temp

supersaturated

solution is holding more solute that it can usually hold at that temp

solution equilibrium

saturated solutions reach equilibrium when equal amount of solute absorbed is precipitated

precipitate

solid that forms in solution during a reaction

At 70 C how much KNO₃ will dissolve in 100g of water?

135g

At 100 C how much NH₄Cl will dissolve in 200g of water?

155g

At 90 C you dissolve 10g of KCl in 100g of water. Is it unsaturated or saturated?

Unsaturated

soluble

ABLE to be dissolved

insoluble

UNABLE to be dissolved

Is CA(ClO₃)₂ soluble or insoluble?

soluble

Is AgCl soluble or insoluble?

insoluble

Is zinc chromate soluble or insoluble?

insoluble

Is gold (1) chloride soluble or insoluble?

soluble

concentration

amount of substance in a solution

quantitative

amount based

dilute

small amount of solute and large amount of solvent

concentrated

large amount of solute and small amount of solvent

% by volume formula

volume of part/volume of whole X 100

2.0g of honey is dissolved in10g of solution. What is the percent by mass of the honey in solution?

20%

What’s the concentration in ppm if 30,000.0g sample of lake water found to have .200g of mercury?

6.67 ppm

How many grams of lead can be dissolved in 6000.g of solution if concentration is 8.5ppm?

0.051g

Solution has concentration of 367ppm. If there’s 0.400g of solute how many grams of solution are there?

1090g

What is the molarity of a solution if 4.0 moles of salt dissolved in 2.5 liters of solution?

1.6mol/L

What is the molarity of a solution if 500.g of Li₂O is dissolved in 500.ml of water?

33.3mol/L

molarity dilutions formula

M₁V₁ = M₂V₂

What volume of a 2.0 molar solution would you need to make 1.0 liter of a 0.1 molar solution?

0.05L

colligative properties

properties of ALL solutions that depend on concentration (#) of solute particles

factors of colligative properties

boiling point elevation, vapor pressure lowering, freezing point depression, osmotic pressure

boiling point elevation

greater the number of particles in a solution higher the boiling point (need more energy to boil more particles)

vapor pressure lowering

greater the number of particles in a solution the lower the vapor pressure (need more energy to vaporize particles so low vapor pressure)

freezing point depression

greater the number of particles in a solution lower the freezing point (need colder temp to increase IMFs bc of particles in the way)

osmotic pressure

greater the number of particles in a solution higher the osmotic pressure

electrolytes

solutions with IONIC compounds dissociate in solutions making them mobile

nonelectrolytes

solutions with MOLECULAR compounds do not dissociate in solutions

Which solution has highest boiling point and largest conductivity? NaCl, CaCl₂, C₆H₁₂O₆

CaCl₂ (needs to dissolve and dissociate so needs high energy; lowest freezing point bc particles are in the way; conducts most electricity bc more ions)

Why do you add salt to your water after it’s boiling and not before?

Salt water causes the solution to have a high boiling point so it would take longer for the water to boil to be able to put your pasta in.

Which aqueous solution of Kl freezes at the lowest temp? 1. 1mol Kl in 500g of water 2. 2 mol Kl in 500g of water 3. 1 mol Kl in 1000g of water 4. 2 mol Kl in 1000g of water

2. 2 mol Kl in 500g of water

Which example when dissolved in 1.0 L of water has the highest boiling point? 1. 0.1 mol C₂H₅OH 2. 0.1 mol LiBr 3. 0.2 mol C₆H₁₂O₆ 4. 0.2 mol CaCl₂

4. 0.2 CaCl₂ - always pick electrolyte if there’s a tie between amount of moles