Solubility of Ionic Compounds

The video tutorial explains how to determine the solubility of various compounds using a solubility table. It covers the general rules for solubility, including exceptions, and provides examples with compounds like silver nitrate, potassium iodide, nickel II chloride, calcium sulfate, lithium hydroxide, and sodium acetate. The tutorial demonstrates how to identify whether a compound will dissolve in water and break into ions or remain a solid.

What does a solubility table help determine?

• The solubility of ions in compounds

• The melting point of compounds

• The density of compounds

• The boiling point of compounds

Which ion in silver nitrate makes it soluble?

• Iodide (I)

• Potassium (K)

• Nitrate (NO3)

• Silver (Ag)

What is the exception for iodide ions in terms of solubility?

• When paired with calcium

• When paired with potassium

• When paired with silver

• When paired with sodium

Why is nickel(II) chloride considered soluble?

• It contains a sulfate ion

• It is a solid at room temperature

• It contains a chloride ion

• It is paired with an exception ion

What makes calcium sulfate insoluble?

• It is paired with a sulfate ion

• It is paired with an exception ion

• It is a gas at room temperature

• It contains a nitrate ion

Which condition makes lithium hydroxide soluble?

• When paired with calcium

• When paired with lead

• When paired with mercury

• When paired with sodium

What is the solubility status of sodium acetate?

• Not determined

• Insoluble

• Slightly soluble

• Soluble

Which ions in sodium acetate ensure its solubility?

• Sodium and chloride

• Sodium and acetate

• Acetate and nitrate

• Nitrate and chloride

What happens to a compound when it is soluble?

• It remains unchanged

• It forms a solid

• It evaporates

• It breaks down into ions

Which of the following is not an exception for sulfate solubility?

• Potassium

• Calcium

• Strontium

• Barium