Question

1: Define strong, weak and none-electrolyte Name 2: Strong and 2 weak and 2 none-electrolyte.

2: I: Silver nitrate react with sodium bromide:   

A: Write a net ionic equation for this reaction.

B: Identify all spectator and none spectator ions.

Answer 1

Strong Electrolytes

Sodium hydroxide is a strong base and strong electrolyte. (Ben Mills)

Strong electrolytes completely ionize in water. This means 100% of the dissolved chemical breaks into cations and anions. However, it does not mean the chemical completely dissolves in water! For example, some species are only slightly soluble in water, yet are strong electrolytes. This means that not very much dissolves, but all that does dissolve breaks into ions. An example is the strong base strontium hydroxide, Sr(OH)2. It has a low solubility in water, but dissociates completely into Sr2+ and OH–ions. While a flask of sodium hydroxide (NaOH) in water would contain Na+ and OH– ions in water, but no actual NaOH, a flask of aqueous strontium hydroxide would contain Sr2+ and OH– ions, Sr(OH)2, and water.

Examples: Strong acids, strong bases, and salts are strong electrolyte

Weak Electrolytes

Ammonia is a weak base and a weak electrolyte. (Ben Mills)

Weak electrolytes partially ionize in water. Pretty much any dissociation into ions between 0% and 100% makes a chemical a weak electrolyte, but in practice, around 1% to 10% of a weak electrolyte breaks into ions.

Examples: Weak acids and weak bases are weak electrolytes. Most nitrogen-containing molecules are weak electrolytes. Water is considered a weak electrolyte by some sources because it partly dissociates into H+ and OH– ions, but a nonelectrolyte by other sources because only a very small amount of water dissociates into ions.

Nonelectrolytes

If a substance doesn’t ionize in water at all, it’s a nonelectrolyte.

Examples: Most carbon compounds are nonelectrolytes. Fats, sugars, and alcohols are largely nonelectrolytes.

Sodium bromide and silver nitrate are both soluble, so they form their constituent ions.

Na+(aq) + Br-(aq) + Ag+(aq) + NO3- (aq)

Double replacement reaction, producing silver bromide and sodium nitrate. Silver bromide is not water soluble, sodium nitrate is.

AgBr(s) + Na+(aq) + NO3-(aq)

So the only things that change are silver and bromide, and that's what goes into the net ionic equation.

Ag+(aq) + Br-(aq) --> AgBr(s)