Chemistry: Solutions

heterogeneous and homogeneous

What are the 2 types of mixtures?

homogeneous mixtures

Mixture that is the same throughout; uniform

heterogeneous mixtures

Mixtures that you can pick apart; easier to separate

soluble

Capable of being dissolved

solvent and solute

What are the 2 components of a solution?

solute

the substance being dissolved in a solution

solvent

dissolving medium in a solution

solvation

The process of dissolving where the solvent molecules surround the solutes particles to cause them to dissolve

hydration

solvation where the solvent is water

solute & solvent; solute-solute

Solvation (dissolving) occurs when the attraction between ________ and ________ is stronger than the ________-________ attraction. Generally this is: “like dissolves like”; polar dissolves polar or nonpolar dissolves nonpolar.

like solvents will dissolve like solutes

Explain the rule of thumb for “like dissolves like” for solutions.

increasing surface area of solute, agitating a solution, heating a solvent

What are 3 factors that affect the rate of dissolving

ionic

Water is a good solvent for ________ compounds.

water

What is known as the universal solvent?

polar

Water solutions are noted as aqueous solutions in chemical equations (aq). Water is a ________ molecule!

unequal

Polar compounds have _______ electron sharing creating a positive and negative molecule. The positive and negative of each substance attract and the water pulls the ionic compounds apart.

molecules or ions

Substances that dissolve in water are classified according to whether they yield __________ or ______ in a solution.

electrolyte

Substance that dissolves in water and conducts electric current. Ex: NaCl and HCl

ionic (ions are free to move, causing current)

What kind of compound is an electrolyte?

strong

Do electrolytes have a strong or weak acid or base?

non-electrolytes

Substance that dissolves in water and does not conduct an electric current. Ex: sugar

neutral

Do non-electrolytes have a positive, negative, or neutral solute molecule?

weak

Do non-electrolytes have a strong or weak acid or base?

dissociation

Separation of ions from each other in a compound when in a solvent.

ionic

Dissociation will happen typically with what type of compounds?

solutions, suspensions, colloids

Name the 3 different types of mixtures.

solutions

Homogeneous mixture of two or more substances in a single phase. Ex: lemonade, salt water.

they are very small and cannot be seen

Describe what the particles in a solution look like.

no

Can particles in a solution be separated by filtering?

suspensions

Particles in a solvent are so large that they settle out unless the mixture is constantly stirred or agitated. Ex: jar of muddy water.

colloids

Particles are intermittent (does not remain constant/the same) in size between those in solutions and suspensions. Ex: mayo, gelatin, cheese, butter, fog, paints.

Tyndall Effect

Light is scattered by colloidal particles dispersed in a transparent medium.

Brownian motion

Random motion due to collisions of rapidly moving molecules.

solubility

Amount of a substance required to form a saturated solution with a specific amount of solvent at a specific temperature.

temperature; pressure

Solubility varies with _________. For gases, solubility varies with _________ also.

100g; 100mL

Solubility values are usually in grams of solute per ______ of solvent or per ______ of solvent at a given temperature.

This depends on intermolecular forces, type of bonding, and polarity or non-polarity of molecules.

How does nature of solute and solvent affect solubility?

has effect on the solubility of a gas but little to none on solubility of solids and liquids

How does pressure affect solubility?

average kinetic energy increases: solubility of gases in liquids decreases and solubility of solids in liquids mainly increase but there are exceptions

How does temperature affect solubility?

immiscible

Liquid solutes and solvents not dissolvable in each other. Ex: salad dressing.

miscible

Liquids that dissolves freely in one another in any proportion. Ex: alcohol and water.

increases

Increase in pressure _________ gas solubility in liquids.

decreases

Increase in temperature usually _________ solubility of gases and increases solubility of solids in liquids.

saturated solution

A solution that contains the maximum amount of dissolved solute.

unsaturated solution

A solution that contains less solute than a saturated solution under the existing conditions

supersaturated solution

A solution that contains more dissolved solute than a saturated solution contains under the same conditions.

concentration

Is the measure of the amount of solute in a given amount of solution.

dilute

There is a relatively small amount of solute in a solvent

concentrated

There is a relatively large amount of solute in a solvent.

dilution

Solutions can be made less concentrated through a ________.

molarity

Concentration is measured in terms of _________.

concentration

The __________ of a solution is a measure of the amount of solute that has been dissolved in a given amount of solvent.

large

A concentrated solution is one that has a relatively _______ amount of dissolved solutes. The solution may appear darker or has a stronger taste or smell.

small

A dilute solution is one that has a relatively _______ amount of dissolved solute. The solution appear lighter or has a weaker/lighter taste or smell.

molar concentration

Is the most effective way of describing a solute concentration in a solution.

Molarity

Is described as the total number of moles of solute dissolved in a liter of solution or moles of solute per liter of solution.

M = moles (of solute) / liters (of solution)

What is the formula equation for Molarity?

dilution

• Reduces the concentration of a solution

• There is a smaller amount of solute dissolved in the solvent.

• To make this, you add more of the solvent to the solution. The final volume of the solution will be higher.

M₁V₁ = M₂V₂

Formula for Dilutions.