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Which of the following slightly soluble compounds has a solubility greater than that calculated from its solubility product because of hydrolysis of the anion present: AgCl, BaSO 4 , CaF 2 , Hg 2 I 2 , MnCO 3 , ZnS, PbS?
CaF 2 , MnCO 3 , and ZnS
Write the ionic equation for dissolution and the solubility product ( K sp ) expression for each of the following slightly soluble ionic compounds:
(a) PbCl 2
(b) Ag 2 S
(c) Sr 3 (PO 4 ) 2
(d) SrSO 4
Write the ionic equation for the dissolution and the K sp expression for each of the following slightly soluble ionic compounds:
(a) LaF 3
(b) CaCO 3
(c) Ag 2 SO 4
(d) Pb(OH) 2
(a)
(b)
(c)
(d)
The Handbook of Chemistry and Physics gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.
(a) BaSiF 6 , 0.026 g/100 mL (contains ions)
(b) Ce(IO 3 ) 4 , 1.5 10 –2 g/100 mL
(c) Gd 2 (SO 4 ) 3 , 3.98 g/100 mL
(d) (NH 4 ) 2 PtBr 6 , 0.59 g/100 mL (contains ions)
The Handbook of Chemistry and Physics gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.
(a) BaSeO 4 , 0.0118 g/100 mL
(b) Ba(BrO 3 ) 2 ·H 2 O, 0.30 g/100 mL
(c) NH 4 MgAsO 4 ·6H 2 O, 0.038 g/100 mL
(d) La 2 (MoO 4 ) 3 , 0.00179 g/100 mL
(a)1.77 10 –7 ; (b) 1.6 10 –6 ; (c) 2.2 10 –9 ; (d) 7.91 10 –22
Use solubility products and predict which of the following salts is the most soluble, in terms of moles per liter, in pure water: CaF 2 , Hg 2 Cl 2 , PbI 2 , or Sn(OH) 2 .
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product:
(a) KHC 4 H 4 O 6
(b) PbI 2
(c) Ag 4 [Fe(CN) 6 ], a salt containing the ion
(d) Hg 2 I 2
(a) 2 10 –2 M ; (b) 1.5 10 –3 M ; (c) 2.27 10 –9 M ; (d) 2.2 10 –10 M
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product:
(a) Ag 2 SO 4
(b) PbBr 2
(c) AgI
(d) CaC 2 O 4 ·H 2 O
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected.
(a) AgCl( s ) in 0.025 M NaCl
(b) CaF 2 ( s ) in 0.00133 M KF
(c) Ag 2 SO 4 ( s ) in 0.500 L of a solution containing 19.50 g of K 2 SO 4
(d) Zn(OH) 2 ( s ) in a solution buffered at a pH of 11.45
(a) 6.4
10
−9
M = [Ag
+ ], [Cl
− ] = 0.025
M
Check:
an insignificant change;
(b) 2.2
10
−5
M = [Ca
2+ ], [F
− ] = 0.0013
M
Check:
This value is less than 5% and can be ignored.
(c) 0.2238
M =
[Ag
+ ] = 7.4
10
–3
M
Check:
the condition is satisfied.
(d) [OH
– ] = 2.8
10
–3
M ; 5.7
10
−12
M = [Zn
2+ ]
Check:
x is less than 5% of [OH
– ] and is, therefore, negligible.
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