Ch 4 Aqueous Solutions

Precipitation Reaction

Aqueous solution + Aqueous solution → insoluble precipitate + aqueous solution

Oxidation Reaction

an oxidation agent gains a electrons (is reduced) and a reducing agent loses electrons (is oxidized)

Acid/Base reaction

Strong Acid + Strong Base → H₂O + salt

Weak Acid + Weak Base → conjugate base + conjugate acid

*carbonate, sulfite, and sulfate salts/bases will react with acids to form water, a gas, and a new salt

Solution Concentration

Molarity = mol/L

Sodium (Na), Potassium (K), and Ammonium (NH4) salts are…

always soluble

Nitrate (NO₃^-), Acetate (CH₃COO^-), and perchlorate (ClO₄) salts are…

always soluble

Chloride, Bromide, and Iodide salts are…

soluble EXCEPT when they contain Silver (Ag⁺), Mercury II (Hg²⁺), or Lead II (Pb²⁺) ions

Hydroxide (OH^-) and oxide salts are…

insoluble except when they contain sodium, potassium, or barium ions (since those are always soluble)

All sulfide and sulfite salts are…

insoluble except when they contain sodium, potassium, ammonium, or barium ions

All carbonate (CO₃^2-) and phosphate (PO₄^3-) salts are…

insoluble except when they contain sodium, potassium, or ammonium ions

Strong Acid Definition

H⁺ donating substance which disassociate completely into ions in water

Weak Acid definition

compounds which disassociate somewhat in water and donate H+

Strong Base definition

OH^- donating substances which disassociate completely in water

Weak Base definition

compounds which disassociate in water somewhat and accept H+ ions

Strong Acids typically contain…

halogens

Strong Bases contain

OH- ions

HCl (hydrochloric Acid)

Strong Acid

HF (hydrofluoric acid)

Weak Acid

HBr (hydrobromic acid)

Strong Acid

HI (hydriodic acid)

Strong Acid

H₂S (hydrosulfuric acid)

Weak Acid

HNO₃ (nitric acid)

Strong Acid

H₂SO₄ (sulfuric acid)

Strong Acid

H₂CO₃ (carbonic acid)

Weak Acid

H₃PO₄ (phosphoric acid)

Weak Acid

HClO₄ (perchloric acid)

Strong Acid

HNO₂ (nitrous acid)

Weak Acid

H₂SO₃ (sulfurous acid)

Weak Acid

NH₃

Weak Base

pH acidity scale

measure of concentration of H+ in a solution

pH = -log₁₀[H+]

OIL RIG

Oxidation reaction = compound loses electron

Reduction reaction = compound gains electron

Oxidation number rule 1

Pure elements have an oxidation number of 0

Oxidation number rule 2

If the compound is ionic, the oxidation number for each element is its ion’s charge

Oxidation number rule 3

Oxidation number of non-elemental H is +1 except for hydrides which are -1

Oxidation number rule 4

Oxidation number of non-elemental O is -2 except for peroxides which are -1

Oxidation number rule 5

the sum of the oxidation numbers in a compound is 0

Oxidation number rule 6

the sum of the oxidation numbers in a polyatomic ion is equal to that ion’s charge