Solubility Rules

What is the solubility rule for nitrate (NO3-) salts?

Most nitrate salts are soluble.

Are Na+ salts soluble?

Most sodium salts are soluble.

Are K+ salts soluble?

Most potassium salts are soluble.

Are NH4+ salts soluble?

Most ammonium salts are soluble.

What is the solubility rule for chloride (Cl-) salts?

Most chloride salts are soluble, except those containing Ag+, Hg2^2+, and Pb2+.

Which chloride compounds are notable exceptions to the solubility rule?

AgCl, PbCl2, and Hg2Cl2.

Is AgCl soluble or insoluble?

Insoluble.

Is PbCl2 soluble or insoluble?

Insoluble.

Is Hg2Cl2 soluble or insoluble?

Insoluble.

What is the solubility rule for sulfate (SO4^2-) salts?

Most sulfate salts are soluble, except those containing Ba2+, Pb2+, and Ca2+.

Which sulfate compounds are notable exceptions?

BaSO4, PbSO4, and CaSO4.

Is BaSO4 soluble or insoluble?

Insoluble.

Is PbSO4 soluble or insoluble?

Insoluble.

Is CaSO4 soluble or insoluble?

Slightly soluble.

What is the solubility rule for hydroxide (OH-) compounds?

Most hydroxide compounds are only slightly soluble.

Which hydroxides are important exceptions to the general hydroxide solubility rule?

NaOH, KOH, Ba(OH)2, and Ca(OH)2.

How soluble are NaOH and KOH?

Very soluble.

How soluble are Ba(OH)2 and Ca(OH)2 according to the slides?

Moderately soluble.

What is the solubility rule for sulfide (S2-) salts?

Most sulfide salts are only slightly soluble.

What is the solubility rule for carbonate (CO3^2-) salts?

Most carbonate salts are only slightly soluble.

What is the solubility rule for phosphate (PO4^3-) salts?

Most phosphate salts are only slightly soluble.

Which three types of salts are generally slightly soluble?

Sulfides, carbonates, and phosphates.

Which ions form generally soluble compounds?

NO3-, Na+, K+, and NH4+.

Which ions form generally insoluble or slightly soluble compounds?

S2-, CO3^2-, PO4^3-, and OH-.

What happens when two soluble ionic compounds are mixed and an insoluble product forms?

A precipitation reaction occurs.

What happens if both possible products are soluble?

No precipitate forms.

How do you identify a precipitate using solubility rules?

Determine which possible product is insoluble or slightly soluble.