1) Imagine that saturated solutions of barium chloride (BaCl 2 ) and potassium s

Question

1) Imagine that saturated solutions of barium chloride (BaCl2) and potassium sulfate (K2SO4) are mixed. A white precipitate forms, and the solution is found to contain potassium chloride.

a) What is the name of the precipitate?

b) Write an equation for the reaction that occurs.

c) Which are the specator ions in this reaction?

2) Consider the compound naphthalene.

Based in the rule "Like Dissolves Like:, which should be a good solvent for naphthalene and why: benzene, water, acetone?

3) When mixing the ionic solution pairs, is the quantity of each solution added to the test tube important? Why or not?

4) Predict the water solubility of the following compounds: RbCl, NH4NO3, PbS, BaSO4, AgBr

5) Define a homogenous solution

Explanation / Answer

BaCl2 + K2SO4 --> BaSO4 + 2KCl

a) according to precipitate and solubility rules, BaSO4 will be precipitated

b)

BaCl2 + K2SO4 --> BaSO4 + 2KCl

Ba+2(aq) + SO4-2(aq) --> BaSO4(s)

c)

spectator ions are thos that do not react:

BaCl2 + K2SO4 --> BaSO4 + 2KCl

K+ and Cl- are not reacting

2)

naphthalene is nonpolar, use benzene since it is also nonpolar, water and acetone are polar and wont mix pretty good

3)

In general, not, but you may form complexes (usually ignored)

4)

RbCl --> Soluble since Rb is alkali

NH4NO3 --> All NO3- and NH4 are pretty soluble in water

PbS --> Sulfides are not solubles

BaSO4 --> sulfates are rarely solubles when bonded to Group IIA

AgBr --> Silver Hallides are not soluble

5)

Homogeneous solution ---> It is the same phase, i.e. aqueous and aqueous, solid solid, vapor vapor, etc...

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