The Ksp of Al(OH)3 is 1.0 x 10-33. What is the solubility of
Al(OH)3 in 0.0010...
The Ksp of Al(OH)3 is 1.0 x 10-33. What is the solubility of
Al(OH)3 in 0.0010 M Al(NO3)3? Give your answer using scientific
notation and to 2 significant figures (i.e., one decimal
place).
The solubility product, Ksp, of Al(OH)3(s)
is 1.0 x 10-33. What is its solubility (in g/L) in an
aqueous solution of NaOH with a pH of 12.54 ? The temperature is
25oC.
1. The solubility product, Ksp, for aluminum
hydroxide, Al(OH)3, is 1.9 ✕ 10−33 at 25°C.
What is the molar solubility of aluminum hydroxide in a solution
containing 0.066 M KOHat 25°C?
(a) The solubility product, Ksp, of
Sn(OH)4(s) is 1.0 x 10-57. What is its
solubility (in g/L) in an aqueous solution of NaOH with a pH of
12.80 ? The temperature is 25oC.
(b) For the reaction 2 A(g) ⇋ 3 B(g) + 2 C(g), we start off with
just pure A(g) (there is no B(g) or C(g)). When we reach
equilibrium, the partial pressure of C(g) is 4.19 atm. The
equilibrium constant for this reaction is 8.39 . What...
a) Determine the molar solubility of Fe(OH)3 in pure water. Ksp
= 2.79 × 10-39 for Fe(OH)3.
(b) Determine the molar solubility of Fe(OH)3 if the pH of the
solution is 8.0.
(c) Determine the molar solubility of Fe(OH)3 if the pH of the
solution is 2.0.
The solubility product, Ksp, for cobalt(III) hydroxide, Co(OH)3,
is 1.6 ✕ 10−44 at 25°C. What is the molar solubility of cobalt(III)
hydroxide in a solution containing 0.062 M KOH at 25°C?
Use the solubility-product constant for Cr (OH) 3 (
Ksp = 6.7×10?31) and the formation constant for
Cr (OH) ?4 from the following table to determine the concentration
of Cr (OH) ?4 in a solution that is buffered at pH= 11 and is in
equilibrium with solid Cr (OH) 3.
Table Formation Constants for Some Metal Complex Ions in Water at
25 ?C
Complex Ion
Kf
Equilibrium Equation
Ag(NH3)+2
1.7×107
Ag+(aq)+2NH3(aq)?Ag(NH3)+2(aq)
Ag(CN)?2
1×1021
Ag+(aq)+2CN?(aq)?Ag(CN)?2(aq)
Ag(S2O3)3?2
2.9×1013
Ag+(aq)+2S2O2?3(aq)?Ag(S2O3)3?2(aq)
CdBr2?4
5×103
Cd2+(aq)+4Br?(aq)?CdBr2?4(aq)...