Solubility and Ionic Compounds

The video tutorial explains solubility rules, focusing on which ions are soluble or insoluble in water and how these rules apply to chemical reactions. It covers examples of soluble and insoluble ions, exceptions to these rules, and provides practice problems to reinforce understanding. The tutorial also demonstrates how to derive net ionic equations from given reactions.

What does it mean if a substance is soluble?

• It forms a solid in water.

• It evaporates in water.

• It dissolves in water.

• It reacts with water.

Which of the following ions will always form a soluble compound?

• Hg2+

• Ag+

• Pb2+

• Na+

What is the solubility rule for nitrates?

• They are soluble only with alkali metals.

• They are insoluble.

• They are soluble only with halogens.

• They are always soluble.

Which ion combination will result in an insoluble compound?

• K+ and NO3-

• Ag+ and Cl-

• Na+ and Cl-

• NH4+ and Br-

What happens when Ag+ is combined with Cl-?

• A soluble compound is formed.

• A gas is released.

• No reaction occurs.

• An insoluble compound is formed.

Which of the following is an insoluble ion?

• Sulfate

• Nitrate

• Ammonium

• Carbonate

What is the difference between sulfates and sulfites in terms of solubility?

• Both are soluble.

• Both are insoluble.

• Sulfates are insoluble, sulfites are soluble.

• Sulfates are soluble, sulfites are insoluble.

Which compound is likely to be insoluble in water?

• KNO3

• MgCO3

• NH4Cl

• NaOH

What is the net ionic equation for the reaction between AgNO3 and KBr?

• Ag+ + Br- → AgBr

• K+ + NO3- → KNO3

• K+ + Br- → KBr

• Ag+ + NO3- → AgNO3

Which of the following compounds will dissolve in water?

• PbSO4

• AgCl

• Na2CO3

• CaCO3