Ammonium

NH₄⁺

Soluable

H₂PO₄^-

Insoluble

NO₂^-

Soluble except

NO₃^-

Soluble

SO₃^2-

Insoluble

SO₄^2-

Insoluble

HSO₄^-

Insoluble

PO₄^3-

• All Group 1 (alkali metals and ammonium salts), all nitrates, all chlorates (ClO₃^-), all perchlorates (ClO₄-), all acetates 
• All common chlorides, bromides, and iodides are soluble except, Ag, Mg, Pb
• MOST sulfates are soluble

• All phosphates, carbonates, hydroxides, and oxalates are insoluble except those of NH₄⁺ and Group 1A metals
• All sulfides are insoluble except those of NH₄⁺, Group 1A, and Group 2A

Coulomb’s Law

This law is used to determine the Forces of Attraction in an ionic compound.

K=Q₁Q₂    

       D²

K= Forces of attraction

Q₁=Charge of the first ion

Q₂=Charge of the second ion

D= Distance

Lead, Mercury, and Silver don’t play nice with others.

What does this mean in terms of solubility?

Meaning that they precipitate when combined with a halide

In aqueous reactions some of the ions don’t react/change from one side of the equation to the other we call these ions Spectator ions.

Net ionic equation

The net ionic equation is the equation of a reaction without the spectator ions, it only includes the ions that reacted in the equation.

What is an acid?

An acid is any species that increases the H+ concentration in a solution.

Any acid that fully ionizes is a strong acid. This means that when it is placed in solution all of the acid reacts not just part.

Strong acids are usually inorganic.

An acid that doesn’t fully ionize is a weak acid. Meaning that the acid only reacts with part of the total amount some or most of the acid will not react at all.

Weak acids are usually organic.

A base is any species that increases the Hydroxide ion  (OH-) concentration in a solution.

Like acids strong ionize fully and are inorganic, weak bases are organic.

 “an acid plus a base equals a salt plus water”

In ionic reactions we know that:

for the elements to combine they have to gain or lose an electron from one side of the equation to the other. This is what happens in a redox reaction.

When an ion loses (an) electron(s) it _________

When an ion gains (an) electron(s) it _________

When an ion loses (an) electron(s) it oxidizes.

When an ion gains (an) electron(s) it reduces.

LEO: Loss of electrons is oxidation

goes

GER: Gain of electrons is reduction.

_________are reduced, reduction is gaining electrons. These are Non-metals.

__________ are oxidized, oxidation is gaining electrons. These are Metals.

Oxidizing agents are reduced, reduction is gaining electrons. These are Non-metals.

Reduction Agents are oxidized, oxidation is gaining electrons. These are Metals.

An oxidation number is?

An oxidation number is the charge on the species or ion in a redox reaction

• (1)    The oxidation number or an elemental species is always zero…
• (2)    The oxidation number can usually be predicted by the position of the periodic table…
  • (2a)… except when an atom of a given element is bonded to another atom of the same element.
  • (2b) Halides are normally 1+ except when bonded to Oxygen and Fluorine.
• (3)The overall species must be charged balanced (this is not always zero).

Precipitation Reactions

            Step 1 – consider what each species looks like in solution

            Step 2 – Make a solubility grid

            Step 3 – Apply solubility rules

Ions that don’t change from reactants to products – __________

Anything that does – __________

Ions that don’t change from reactants to products – Spectator ions

Anything that does – Net ions and form net ionic equation

   Most inorganic (mineral) acids are strong, give examples:

HCl       hydrochloric acid

HBr      hydrobromic acid

HI           hydroiodic acid

H2S04       sulfuric acid

HNO3          nitric acid

  CH3COOH             acetic acid

    HCOOH                 formic acid

    C6H5COOH           benzoic acid

        H2CO3                   carbonic acid

Solubility

• Dissociation:
• Solute:
• Solvent:
• Strong electrolyte:

Solubility

• Dissociation: the process when an ionic compound dissolves in water, its ions separate and become surrounded by water molecules.
• Soluble free ions are called electrolytes, which cause water to conduct electricity.
• Solute: the substance being dissolved
• Solvent:  the substance doing the dissolving
• Strong electrolyte: completely converted to ions when it forms an aqueous solution.