WorksheetsSolubility equilibrium
Total questions: 10
Worksheet time: 10mins
The concentration of OH– in a saturated solution of Mg(OH)2 is 3.6 x 10–4 M. The Ksp of Mg(OH)2 is
1.3 x 10–7
4.7 x 10–11
3.6 x 10–4
2.3 x 10–11
The correct mathematical expression for finding the molar solubility (X) of Sn(OH)2 is:
2(X)3 = Ksp
108(X)5 = Ksp
4(X)3 = Ksp
8(X)3 = Ksp
Barium carbonate has a measured solubility of 4.0 x 10–5 at 25°C. Determine the Ksp.
5.3 x 10–10
6.1 x 10–5
9.1 x 10–7
1.6 x 10–9
The [IO3–] in a saturated solution of Ce(IO3)3 is 5.55 x 10–3 M. Calculate the Ksp for Ce(IO3)3.
3.16 x 10–10
1.03 x 10–5
2.56 x 10–8
3.51 x 10–11
Determine the concentration of the Ag+ ion in a saturated solution of silver phosphate (Ag3PO4). The solubility of silver phosphate at 25°is 1.6 x 10–5 mol/L.
1.6 x 10–5 M
3.2 x 10–5 M
4.8 x 10–5 M
6.4 x 10–5 M
The molar solubility of PbI2 is 1.5 x 10-3 M. Calculate the value of Ksp for PbI2.
1.5 x 10-3
2.3 x 10-6
1.4 x 10-8
3.4 x 10-9
What is the equilibrium expression for the solubility product (Ksp) of the following salt :
MgCO3
Ksp = [Mg2+] [CO3-]
Ksp = [Mg2+] [CO32-]
Ksp = [Mg2+]2 [CO32-]
Ksp = [Mg2+] [CO32-]2
What is the equilibrium expression for the solubility product (Ksp) of the following salt :
Al(OH)3
Ksp = [Al+] [OH-]3
Ksp = [Al2+] [OH-]3
Ksp = [Al+]3 [OH3-]
Ksp = [Al3+] [OH-]3
What is the equilibrium expression for the solubility product (Ksp) of the following salt :
Fe2S3
Ksp = [Fe2+]3 [S3-]2
Ksp = [Fe+]2 [S-]3
Ksp = [Fe3+]2 [S2-]3
Ksp = [Fe2+] [S3-]
Which of the following equation represents the equilibrium equation of solubility of BaSO4 in water ?
BaSO4(s) ↔ Ba2+(aq) + 2SO4-(aq)
BaSO4(s) ↔ Ba+(aq) + 4SO-(aq)
BaSO4(s) ↔ Ba+(aq) + SO4-(aq)
BaSO4(s) ↔ Ba2+(aq) + SO42-(aq)
