C4 - Aqueous Solutions (Gen. Chem 1)

solute

the “dissolved”

solvent

the “dissolver”

electrolyte

substance which forms ions upon dissolution

metathesis reaction

two polyatomic ions exchanging eachother’s cations & anions

molecular equation

standard, no ionic characters

complete ionic equation

splits all aqueous solutions into their respective ions

net ionic equation

complete ionic solution w/o spectator ions

redox reaction

exchange of electrons between reactants

• oxidizer: receives electrons, gets reduced

• reducer: donates electrons, gets oxidized

oxidized

the loss of electrons in a redox reaction (+ charge)

reduced

the gain of electrons in a redox reaction (- charge)

oxidation # rules

• O = -2

  • peroxides: O = -1

• H

  • nonmetals: +1

  • metals: -1

• F = -1

• Halogens (excluding F):

  • binary: halogen = -1

  • w/ O: halogen = +1

• neutral compound: ∑ = 0

• ion: ∑ = charge

displacement reaction

AB + X → AX + B

activity series

list of metals in order from easiest to hardest to oxidize

molarity

M = mols solute/L solvent

concentration equation

(MV)_concentrated = (MV)_dilute

Titration (steps)

1. Add initial (unknown) solution + acid-base indicator

2. Drip in standard solution w/ buret

3. Calculate values once equivalence point is reached