Acids, Bases, Concentration, + pH Test: Chem. Per. 8 Mileham

define: solubility, solute, solvent, + solution

solubility: ability to be dissolved

solute: substance being dissolved (smaller concentration)

solvent: substance doing the dissolving (higher concentration)

solute + solvent = solution

What is a Homogeneous solutions + give the 3 examples

definition: an evenly mixed solution

Ex. gas, liquid, and solid solutions

What is Heterogeneous + give an example.

definition: a solution with uneven distribution of solvent and solute

Ex. colloids: solution where solute is suspended in the mixture + don’t settle or seperate

Colloids exhibit the Tyndall Effect: What is this?

• when light bounces off a solution instead of through

example: fog

What are the 4 factors affecting solubility?

1. surface area of solute

2. temperature

3. concentration of solvent

4. movement: stirring, mixing, or shaking

definition of saturation, saturated, unsaturated, + supersaturated

the amount of solute in a solvent

saturated: perfect amount of solute dissolved

unsaturated: more can be dissolved

supersaturated: more solute dissolved than possible b/c of special conditions

Why is the temperature on the x-axis on the saturation graph between 0-100*C?

water freezes at 0 and boils at 100*C: solubility no longer possible

For SOLIDS, how is solubility affected by temperature?

as temp. increases, so does solubility

For GASES, how is solubility affected by temperature?

as temp. increases, solubility decreases

What does concentration mean?

ratio of solute:solvent

What does it mean if a solution is concentrated? How about a Dilute?

there’s a large amount of solute present relative to the amount of solvent

dilute: small amount of solute relative to the solvent

What does molarity measure?

moles of solute per liters of solution

What is a Dilution?

reducing concentration by adding solvent

What are the key differences between acids and bases (4)?

acids: sour, 0-6.9 pH, conductive, reactive w/ bases

bases: bitter, 7.1-14 pH, reactive w/ acids

What do Arhenius solutions do when they’re acids vs. bases?

acids: produce H+ in water

bases: produces OH- in water

What do Bronston-Lowry solutions do when they’re acids vs. bases?

acids: H+ donor

bases: H+ acceptor

example: NH3 is a base because it accepts H+ to become NH4

What do Lewis solutions do when they’re acids vs. bases?

acids: accepts electron pair

bases: donates electron pair

What do strong acids/bases do? Weak ones?

fully break apart

• weak ones partially break apart

Amphoteric Substances / Neutralization Reactions

• acts as an acid or a base

• reaction: between an acid + base —> produce water and a salt

What is the difference in OH- and H+ concentration in acids and bases?

acids: high H+

bases: high OH-