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18 Dec 2019

Question 5)

Write the balanced equations and expressions for Ksp for the dissolution of the following ionic compounds

a. PbCl2 b. AgI c.Mg(OH)2 d. CaF2

Using the values given in table 17.4, determine the molar solubilities for each of the compounds in question 5. Also determine the solubility in g/l for each of these compounds.

From table 17.4 Ksp values

a. = 2.4x10^-4

b.= 8.3x10^-17

c.= 1.2x10^-11

d.= 4.0x10^-11

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31 Dec 2019

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Related questions

Solubility:

1. The volume of water needed to dissolve 0.0589 grams of calcium chromate is ____ L.

(Assume no volume change upon addition of the solid.)

2. The mass of magnesium hydroxide that is dissolved in 225 mL of a saturated solution is ______ grams.

3. Consider these compounds:

A. MgCO3
B. CuS
C. Mn(OH)2
D. Cu(OH)2

Complete the following statements by entering the letter corresponding to the correct compound.

Without doing any calculations it is possible to determine that iron(II) carbonate is more soluble than __, and iron(II) carbonate is less soluble than __.

It is not possible to determine whether iron(II) carbonate is more or less soluble than __ by simply comparing Ksp values.

4.

A. PbCrO4
B. AgBr
C. Zn3(PO4)2
D. Ca3(PO4)2

Complete the following statements by entering the letter corresponding to the correct compound.

Without doing any calculations it is possible to determine that barium phosphate is more soluble than __, and barium phosphate is less soluble than __.

It is not possible to determine whether barium phosphate is more or less soluble than __ by simply comparing Ksp values.

5. For each of the salts on the left, match the salts on the right that can be compared directly, using Ksp values, to estimate solubilities.

(If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g, ABC.)

1. lead sulfate ____ A. MnS
2. lead phosphate ____ B. BaSO4
C. Ba3(PO4)2
D. Mn(OH)2



Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water.

lead sulfate

lead phosphate

Ksp = ____

Ksp = ____

Note: Multiply out any number and put it first in the Ksp expression. Combine all exponents for s.

Write the chemical equations for the dissociation of each of the following substances and determine their molar solubilities. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer. See the appendix.)

(a) BaSO4

BaSO4(s) ? Ba2+(aq)+SO

2-
4

(aq)

Correct.


M

(b) Ba(OH)2

Ba(OH)2(s) ? Ba2+(aq)+2OH-(aq)

Correct.


M

Substance Ksp at 25 oC
Aluminum
Al(OH)3 1.9 x 10-33
Barium
Ba(OH)2 5.0 x 10-3
BaCO3 8.1 x 10-9
BaSO4 1.1 x 10-10
Ba3(PO4)2 3.4 x 10-23
Cadmium
Cd(OH)2 2.5 x 10-14
CdCO3 5.2 x 10-12
CdS 8.0 x 10-27
Calcium
Ca(OH)2 5.5 x 10-6
CaCO3 4.8 x 10-9
Ca3(PO4)2 1.0 x 10-26
CaF2 3.9 x 10-11
Chromium
Cr(OH)3 6.3 x 10-31
Cobalt
Co(OH)2 1.6 x 10-15
CoS 4.0 x 10-21
Copper
Cu(OH)2 2.2 x 10-20
Cu2S 1.6 x 10-48
CuCO3 1.4 x 10-10
CuS 6.3 x 10-36
Iron
Fe(OH)2 8.0 x 10-16
FeS 6.3 x 10-18
Fe(OH)3 2.5 x 10-39
FePO4 9.9 x 10-29
Lead
Pb(OH)2 2.8 x 10-16
PbF2 3.7 x 10-8
PbCl2 1.7 x 10-5
PbBr2 6.3 x 10-6
PbI2 6.5 x 10-9
PbCrO4 1.8 x 10-14
PbSO4 1.7 x 10-8
PbS 8.4 x 10-28
Magnesium
Mg(OH)2 1.8 x 10-11
Manganese
Mn(OH)2 1.9 x 10-13
MnCO3 8.8 x 10-11
MnS 5.6 x 10-16
Nickel
Ni(OH)2 1.6 x 10-14
Silver
AgCl 1.8 x 10-10
AgBr 5.0 x 10-13
AgI 8.3 x 10-17
AgCN 1.2 x 10-16
Ag2S 6.3 x 10-50
Ag2CrO4 1.1 x 10-12
Ag3PO4 2.6 x 10-18
Tin
Sn(OH)2 1.4 x 10-28
SnS 1.3 x 10-23
Zinc
ZnCO3 1.0 x 10-10
Zn(OH)2 4.5 x 10-17
ZnS 1.1 x 10-21

Groundwater at a temperature of 250C flows through strata containing abundant fluorite (CaF2) mineralization and becomes saturated with respect to that mineral. The equilibrium solubility product, Ksp, for this reaction is 10^-10.4.

a) Calculate the concentrations of Ca2+ and F- once the water has reached saturation with respect to fluorite assuming that prior to entering the mineralized strata the water had an ionic strength of less than 10-5 mol/L and contained negligible Ca2+ and negligible F-. For this part of the problem, neglect activity corrections. (Note that for each mole of CaF2 that is dissolved, you will get one mole of Ca2+ and two moles of F-.

b) Calculate the ionic strength for the groundwater that has the concentrations of Ca2+ and F- that you determined in part a) assuming that Ca2+ and F- are the only major ions in the groundwater. Then calculate the activity coefficients for Ca2+ and F- at this ionic strength. Were you justified in neglecting activity corrections?

c) Repeat the calculations from part a) but this time including activity corrections for water with the ionic strength you determined in part b). Does the calculation including these activity corrections predict more or less dissolution of fluorite?

d) Repeat the calculations from part a) but this time assuming that the groundwater has an initial ionic strength of 0.01 and an initial concentration of Ca2+ of 0.55 x 10^-3 mol/L. (Note that you will need to use the extended Debye-Huckel equation for activities at this ionic strength. Also, remember that each mole of fluorite that dissolves will add one mole of Ca2+ and two moles of F- to what is already in solution.)

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