solutions chemistry quest

Water molecule

Water molecule

Hydrogen bonding

The strongest intermolecular force

Is water polar or nonpolar at room temperature?

Polar

Water has very ____ intermolecular forces because of hydrogen bonding (strong/weak)

strong

Water has a ____ boiling point (high/low)

High

High surface tension

The hydrogen bond between water molecules is strong enough to form a thin film and have a specific shape

When water freezes, it is ________ than water (more dense/less dense)

Less dense- the hydrogen bonds push the molecules apart when the liquid freezes

Solvation

How a solute dissolves

Factors that affect the rate of solvation

• Increasing the temperature (energizes the particles)

• Agitate the solution (mix it, eg. stirring kool-aid with a spoon)

• Increase the surface area of the solute (eg. crushing up your pill)

  • Solvent particles have an easier access to the “fresh” solute

Suspension

A heterogenous mixture that does exhibit the Tyndall effect and settles out over time into its components (eg. muddy water, orange)

Colloid

A mixture that does exhibit the Tyndall effect and does not settle out. (eg. foam, milk, fog)

Do solutions settle out?

No

Do solutions exhibit the Tyndall effect?

No

Do colloids settle out?

No

Do colloids exhibit the Tyndall effect?

Yes

Do suspensions settle out?

Yes

Do suspensions exhibit the Tyndall effect?

Yes

Solution

A homogenous mixture where one substance is dissolved by another

Solution

Solute + solvent

Solute

Substance that is dissolved

Solvent

Substance that does the dissolving

Solubility

The maximum amount of solute that will dissolve in a given amount of solvent at a specific temperature

Increasing the temperature of a solid ______ solubility (increases/decreases)

Increases

Increasing the temperature of a gas _____ solubility

Decreases

How do pressure affect gases?

More pressure increases solubility

Types of solutions

Saturated, unsaturated, super saturated

Unsaturated solutions

The solvent can still dissolve more solute

Saturated solution

The solvent cannot dissolve more solute- if you add more solute, it would just remain at the bottom

Supersaturated solution

The solvent contains more solute than it can handle- eventually returns to an unsaturated solution

Molarity

A unit of concentration

Concentration

Relatively how strong something is

How to calculate Molarity?

Molarity = moles of solute / liters of solution

Liters of solution

Liters of solute + Liters of solvent

“How do you prepare”

Dissolve (Molarity) g in enough water until you reach (L of solution)

Dilution

When the water is added to a strong solution to make it weaker

Dilution equation

M₁V₁= M₂V₂

Salts

Ionic compounds that separate into ions in water like acids and bases. But they do NOT produce H⁺ or OH^- ions

Properties of acids

• pH < 7

• Sour taste or tart

• Corrosive on metals

• Release H⁺ ions after dissociation

• Turns litmus paper red

• eg. lemon juice, vinegar, soda

Properties of bases

• pH > 7

• Taste bitter

• Corrosive on metals

• Release OH^- ions after dissociation

• Turns litmus paper blue

• Feels slippery

• eg. drain cleaner, soap, household ammonia

Arrhenius Theory (Acid & Base Theory)

Acids ionize to produce H⁺ ions in water (AKA spare proton), bases ionize to produce OH^- ions in water

When acids are proton donors…

Hydrogen will decrease

When bases are proton acceptors…

Hydrogen will increase

pH + pOH = ?

14

Neutralization equation

A double replacement reaction where an acid and a base react to produce a salt (ionic compound) and water

Titration

A lab technique that Is used to determine the molarity of an acid/base in a solution from a neutralization equation

Indicator

A chemical dye that changes color at a certain pH

Equivalence point

When moles of acid = moles of base

End point

When the indicator permanently changes the solution color once at the equivalence point

Titration equation

M_aV_a/C_a = M_bV_b/C_b (a = acids, b = base)