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Multiple Choice questions on solubility

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1. What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl?
(Ksp PbCl2 = 1.6 x 10-5)

a. 7.1 x 10-4
b. 1.1 x 10-4
c. 2.0 x 10-3
d. 1.8 x 10-4
e. 1.6 x 10-5

2. In which aqueous system is PbI2 least soluble?

a. H2O
b. 0.2 M HI
c. 0.5 M HI
d. 1.0 M HNO3
e. 0.8 M KI

3. AgCl dissolves in aqueious solutions of ammonia via formation of a
complex, Ag(NH3)2+:
AgCl(s) + 2NH3(aq) → Ag(NH3)2+(aq) + Cl-(aq).
Let z denote the molar solubility of AgCl in 2.0 M NH3. Given that
Kc = KspKf (where Ksp is for AgCl and Kf is for Ag(NH3)2+), the
value of z can be calculated according to which of the following
equations?

a. KspKf = (2.0 + 2z)2/z
b. KspKf = z/(2.0 + 2z)2
c. KspKf = z2/(2.0 - z)
d. KspKf = z/(2.0 - z)2
e. KspKf = z2/(2.0 - 2z)2

4. Which one of the following compounds will increase in solubility if
the pH of a saturated solution of the compound is lowered?

a. AgCl
b. NaCl
c. Cr(OH)3
d. PbCl2
e. AgI

5. Consider a solution containing 0.181 M lead ions and 0.174 M
mercury(II) ions. The Ksp for lead sulfide is 3.4 x 10-28 and that
for mercury(II) sulfide is 4.0 x 10-53. Calculate the concentration
(in M) of sulfide ions required to reduce the concentration of
mercury(II) ions to 1.0 x 10-6 M.

a. 3.4 x 10-22
b. 1.2 x 10-25
c. 4.0 x 10-47
d. 5.6 x 10-13
e. 3.4 x 10-28

6. If treatment of a solution, known to contain at least one type of
cation, with dilute HCl did not result in the formation of a
precipitate, which ion below might the solution contain?

a. Ag
b. Pb
c. Cd
d. Hg22+
e. The solution could contain any of these

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https://brainmass.com/chemistry/acids-and-bases/multiple-choice-questions-on-solubility-52726

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Multiple Choice questions on solubility

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General Chemistry

A saturated solution _______________.

a. cannot be attained
b. contains dissolved solute in equilibrium with undissolved solid
c. contains as much solvent as it can hold
d. will rapidly precipitate if a seed crystal is added
e. contains no double bonds

Which one of the following is most soluble in water?

a. CH3CH2OH
b. CH3CH2CH2OH
c. CH3CH2CH2CH2OH
d. CH3OH
e. CH3CH2CH2CH2CH2OH

Which one of the following substances would be the most soluble in CCI4?

a. CH3CH2OH
b. C10H22
c. H2O
d. NaCI
e. NH3

A supersaturated solution ____________.

a. is one that has been heated
b. must be in contact with undissolved solid
c. is one with more than one solute
d. is one with a higher concentration than the solubility
e. exists only in theory and cannot actually be prepared

The molality of a benzene solution prepared by mixing 12.0 g C6H6 with 38.0 g CCl4 is _____________.

a. 0.316
b. 0.240
c. 0.622
d. 0.508
e. 4.04

Pressure has an appreciable effect on the solubility of ___________ in liquids.

a. liquids
b. salts
c. gases
d. solids
e. solids and liquids

As the concentration of a solute in a solution increases, the freezing point of the solution _________ and the vapor pressure of the solution _________.

a. increases, decreases
b. increases, increases
c. decreases, is unaffected
d. decreases, increases
e. decreases, decreases

Which liquid will have the lowest freezing point?

a. aq. 0.050 m glucose
b. aq. 0.030 m NaI
c. pure H2O
d. aq. 0.030 m AlI3
e. aq. 0.030 m CoI2

What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO3)2 (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for water is 1.86°C/m.

a. -3.34
b. -1.11
c. 3.34
d. 1.11
e. 0.00

Which one of the following 0.1 M aqueous solutions would have the lowest freezing point?

a. NaCl
b. Sucrose
c. K2CrO4
d. Na2SO4
e. Al(NO3)3

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