Chem 105 Exam 2

Strong electrolytes

Ionic compounds soluble in water, strong acids, strong bases

strong acids

HCl, HBr, HI, H2SO4, HNO3, HClO4- Ionizes

Strong bases

Forms OH in water – OH plus group one or two metals

precipitation reaction

Forms precipitate (solid), not soluble

acid base reaction

Results information of H2O and salt

complete ionic equation

Split everything into ions except for solids because they cannot be separated

net ionic equations

All ions that make up a solid; aqueous ions are considered spectators here

arrhenius

Acid-base theory that defines acids as substances that increase hydrogen ion concentration and bases as substances that increase hydroxide ion concentration in aqueous solutions.

bronsted lowry

Acid-base theory that defines acids as proton donors and bases as proton acceptors.

molarity

A measure of concentration defined as the number of moles of solute per liter of solution. M= mole of solute/ Liter of solution

Temperature

measure of thermal energy

heat

Exchange of thermal energy between system and surroundings

Thermal equilibrium

Same temperature

Temperature change

Final temperature minus initial temperature

Heat capacity

Relates heat and change in temperature

Specific heat capacity

How much heat required to raise temperature of 1 g of the substance by 1°C

Exothermic

Release, exit

Endothermic

Absorb, enter

Reaction stoichiometry

Relationship between chemical amounts and a balanced equation

Limiting reactant/reagent

Reactant that limits amount of product formed during a chemical reaction

Theoretical yield

Amount of product that can be made in a chemical reaction based on the amount of limiting reactant

Actual yield

Amount of product actually produced by reaction

Percent yield

Actual yield divided by theoretical yield times 100%

Solution dilution

M1V1=M2V2