AQUEOUS STOICH

Acid/Base Neutralization

Acid + Base → Water + Salt; double replacement

CO₂ Formation

Any CO₃^2- or HCO₃^- + Acid → Solution + CO₂ + H₂O; double replacement

NH₃ Formation

Any NH₄⁺ salt + Strong base → Solution + NH₃ + H₂O; double replacement

SO₂ Formation

Any SO₃^2- salt + acid → Solution + SO₂ + H₂O

H₂CO₃ →

CO₂ + H₂O

NH₄OH →

NH₃ + H₂O

H₂SO₃ →

SO₂ + H₂O

Oxidizing Agent

The ion/molecule gaining electrons, allowing for something else to be oxidized

Reducing Agent

The ion/molecule losing electrons, allowing for something else to be reduced.

Electrolysis

Breaks down compound into pure elemental forms. Uses electricity to drive non-spontaneous rxn; type of decomposition

Metal Replacement

metal 1 + metal 2 compound → metal 1 compound + metal 2; only occurs if metal 1 is lower than metal 2 on the SRPC; single replacement

Hydrogen Replacement

only occurs with H₂O if metal is below H₂O on SRPC; forms H₂ + 2OH^-. occurs with H⁺ (actual acid like HCl) if metal is below H⁺ on SRPC; forms H₂

Unreactive Metals

Unreactive metal + OxyAcid → Nonmetallic oxide gas + H₂O + salt; only occurs with nitric and sulfuric acid.

metal oxides + non-metallic oxide →

yield a salt;synthesis

metal oxide + water →

yield a metal hydroxide;synthesis

nonmetal oxide + water →

yield an acid;synthesis

metal chlorates →

yield metal chlorides + O₂;decomposition

metal carbonates →

yield metal oxide + CO₂;decomposition

What makes some solutes electrolytes and some not?

The level of hydration (amount of ions)

Hydration

The process in which an ion or molecule is surrounded by water molecules.

Dissolve

Surrounded by enough water to look like water (clear)

Dissociate

When a compound separates into its ions

Strong electrolytes

Completely dissociate; include soluble ionic salts, the 6 strong acids, and the 8 strong bases

Hydration shell

A structured group of water molecules surrounding a dissolved ion or polar solute, oriented by electrostatic interactions

Strong Acids

HCl, HBr, HI, HNO₃, HClO₄, H₂SO₄

Strong Bases

Alkali metal hydroxides, CaBaSr hydroxides

Soluble Ionic Compounds

Alkali metals, NH₄⁺, CH₃COO^-, HCO₃^-, ClO₃^-, NO₃^-, ClO₄^-

Usually Soluble (*Insoluble)

[Cl^-, Br^-, I^-]*(MLS)
[F^-]*(MLS, CaBaSr, Mg)
[SO₄^2-]*(MLSCaBaSr)

Insoluble Ionic Compounds

metal oxides*(alkali + ammonium), metal hydroxides, phosphates, chromates, dichromates, carbonates, sulfides*(CaBaSr)

Electrolysis

using electricity to drive a nonspontaneous redox reaction

What is the left side called?

Anode

What is the right side called?

Cathode

Anode

electrons leave here in the Hoffman apparatus

Cathode

electrons enter here in the Hoffman apparatus

Bromothymol blue

pH indicator; yellow in acidic conditions <7, blue in basic conditions >7, and green in neutral conditions =7