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Perform the following calculations:
(a) Calculate [Ag + ] in a saturated aqueous solution of AgBr.
(b) What will [Ag + ] be when enough KBr has been added to make [Br – ] = 0.050 M ?
(c) What will [Br – ] be when enough AgNO 3 has been added to make [Ag + ] = 0.020 M ?
The solubility product of CaSO 4 ·2H 2 O is 2.4 10 –5 . What mass of this salt will dissolve in 1.0 L of 0.010 M
Mass (CaSO 4 ·2H 2 O) = 0.72 g/L
Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products).
(a) TlCl
(b) BaF 2
(c) Ag 2 CrO 4
(d) CaC 2 O 4 ·H 2 O
(e) the mineral anglesite, PbSO 4
Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products):
(a) AgI
(b) Ag 2 SO 4
(c) Mn(OH) 2
(d) Sr(OH) 2 ·8H 2 O
(e) the mineral brucite, Mg(OH) 2
(a) [Ag + ] = [I – ] = 1.3 10 –5 M ; (b) [Ag + ] = 2.88 10 –2 M , = 1.44 10 –2 M ; (c) [Mn 2+ ] = 3.7 10 –5 M , [OH – ] = 7.4 10 –5 M ; (d) [Sr 2+ ] = 4.3 10 –2 M , [OH – ] = 8.6 10 –2 M ; (e) [Mg 2+ ] = 1.3 10 –4 M , [OH – ] = 2.6 10 –4 M .
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate K sp for each of the slightly soluble solids indicated:
(a) AgBr: [Ag + ] = 5.7 10 –7 M , [Br – ] = 5.7 10 –7 M
(b) CaCO 3 : [Ca 2+ ] = 5.3 10 –3 M , = 9.0 10 –7 M
(c) PbF 2 : [Pb 2+ ] = 2.1 10 –3 M , [F – ] = 4.2 10 –3 M
(d) Ag 2 CrO 4 : [Ag + ] = 5.3 10 –5 M , 3.2 10 –3 M
(e) InF 3 : [In 3+ ] = 2.3 10 –3 M , [F – ] = 7.0 10 –3 M
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate K sp for each of the slightly soluble solids indicated:
(a) TlCl: [Tl + ] = 1.21 10 –2 M , [Cl – ] = 1.2 10 –2 M
(b) Ce(IO 3 ) 4 : [Ce 4+ ] = 1.8 10 –4 M , = 2.6 10 –13 M
(c) Gd 2 (SO 4 ) 3 : [Gd 3+ ] = 0.132 M , = 0.198 M
(d) Ag 2 SO 4 : [Ag + ] = 2.40 10 –2 M , = 2.05 10 –2 M
(e) BaSO 4 : [Ba 2+ ] = 0.500 M , = 2.16 10 –10 M
(a) 2.0 10 –4 ; (b) 5.1 10 –17 ; (c) 1.35 10 –4 ; (d) 1.18 10 –5 ; (e) 1.08 10 –10
Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for K sp values.)
(a) KClO 4 : [K + ] = 0.01 M , = 0.01 M
(b) K 2 PtCl 6 : [K + ] = 0.01 M , = 0.01 M
(c) PbI 2 : [Pb 2+ ] = 0.003 M , [I – ] = 1.3 10 –3 M
(d) Ag 2 S: [Ag + ] = 1 10 –10 M , [S 2– ] = 1 10 –13 M
Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for K sp values.)
(a) CaCO 3 : [Ca 2+ ] = 0.003 M , = 0.003 M
(b) Co(OH) 2 : [Co 2+ ] = 0.01 M , [OH – ] = 1 10 –7 M
(c) CaHPO 4 : [Ca 2+ ] = 0.01 M , = 2 10 –6 M
(d) Pb 3 (PO 4 ) 2 : [Pb 2+ ] = 0.01 M , = 1 10 –13 M
(a) CaCO
3 does precipitate.
(b) The compound does not precipitate.
(c) The compound does not precipitate.
(d) The compound precipitates.
Calculate the concentration of Tl + when TlCl just begins to precipitate from a solution that is 0.0250 M in Cl – .
Calculate the concentration of sulfate ion when BaSO 4 just begins to precipitate from a solution that is 0.0758 M in Ba 2+ .
3.03 10 −7 M
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