AP Chemistry : Solutions and States of Matter

Study concepts, example questions & explanations for AP Chemistry

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Example Questions

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Example Question #171 : Solutions And States Of Matter

Which of these WILL be soluble in water?

Possible Answers:

FeCl2

Ca2(PO4)3

AgCl

CsCl

CuCl

Correct answer:

CsCl

Explanation:

Solubility Rules: the only soluble ionic compound listed is CsCl; the rest are insoluble due to solubility rules

Example Question #11 : Solubility

Which of the following compounds is insoluble in water?

Possible Answers:

Correct answer:

Explanation:

Unless paired with an alkali metal, carbonate compounds are generally insoluble. Compounds that contain nitrate or an alkali metal will generally be soluble in water, and hydroxides are soluble when paired with heavier alkaline earth metals (such as calcium).

Example Question #11 : Solubility

Which of the following will form a precipitate in solution?

Possible Answers:

None of these will form a precipitate

Correct answer:

None of these will form a precipitate

Explanation:

Standard solubility rules tell us that group I elements and ammonium cations will always result in soluble salts. Lithium, sodium, and potassium are all group I elements, indicating that none of the given answer options will form a precipitate in solution.

Example Question #21 : Solubility

Which of the following ionic compounds is soluble in water?

I. 

II. 

III. 

Possible Answers:

II and III

I, II, and III

I only

I and II

Correct answer:

I and II

Explanation:

Solubility rules determine which ionic compounds are soluble. All nitrates and group I compounds (those containing alkali metals) are soluble. This means that compounds I and II must be soluble; compound I is a nitrate and compound II contains sodium, an alkali metal.

Compound III, calcium fluoride, is not soluble. Most fluoride compounds are soluble, with the exceptions of: .

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