Consider the equilibrium shown.
PbBr2(s)−⇀↽− Pb2+(aq)+2Br−(aq)Ksp=2.10×10−6
Determine the concentrations of Pb2+ and Br− in a saturated
solution of PbBr2 in pure water (assume μ=0 M).
[Pb2+]=
M
[Br−]=
M
Determine the concentrations of Pb2+ and Br− in a saturated
solution of PbBr2 in a solution with an ionic strength of 0.010
M.
[Pb2+]=
M
[Br−]=
M
Determine the concentrations of Pb2+ and Br− in a saturated
solution of PbBr2 in a solution with an ionic strength of 0.10
M.
[Pb2+]=...
Determine the concentrations of BaBr2, Ba2 , and Br– in a
solution prepared by dissolving 1.76 × 10–4 g BaBr2 in 2.50 L of
water. Express all three concentrations in molarity. Additionally,
express the concentrations of the ionic species in parts per
million (ppm).
[BaBr2]= ______M
[Ba2+]=_______M = _______ ppm
[Br-]=________M = ________ppm
(Please show steps!)
The Ksp of PbBr2 is 6.60x10-6.
A) What is the molar solubility of PbBr2 in Pure
water?
B) what is the molar solubility of PbBr2 in .500M KBr
solution?
C) what is the molar solubility of PbBr2 in a .500M
Pb(No3)2 Solution?
The Ksp of PbBr2 is 6.60*10^-6 M^3. What is the molar solubility
of PbBr2 in pure water?
What is the molar solubility of PbBr2 in 0.500 M KBr
solution?
What is the molar solubility of PbBr2 in 0.500 M Pb(NO3)2
solution?
Determine the concentrations of the ionic species present in a
0.268 M solution of the
NaO2CCOCH2CO2Na.
(pKa1=3.40, pKa2=5.11 for
HO2CCOCH2CO2H).
a) [HO2CCOCH2CO2H]
b)[HO2CCOCH2CO2-]
c)
[-O2CCOCH2CO2-]
d) [H3O+]
e) [OH-]
Determine the concentrations of K2SO4, K , and SO42– in a
solution prepared by dissolving 2.20 × 10–4 g K2SO4 in 1.50 L of
water. Express all three concentrations in molarity. Additionally,
express the concentrations of the ionic species in parts per
thousand (ppt). Note: Determine the formal concentration of SO42–.
Ignore any reactions with water.
K2SO4 = __ M?
K+ = __ M ? --> ppt?
SO4^2- = __ M? --> ppt?
Determine the concentrations of K2SO4, K , and SO42– in a
solution prepared by dissolving 2.72 × 10–4 g K2SO4 in 1.00 L of
water. Express all three concentrations in molarity. Additionally,
express the concentrations of the ionic species in parts per
million (ppm). Note: Determine the formal concentration of SO42–.
Ignore any reactions with water.
Determine the concentrations of Na2CO3, Na , and CO32– in a
solution prepared by dissolving 2.61 × 10–4 g Na2CO3 in 2.25 L of
water. Express all three concentrations in molarity. Additionally,
express the concentrations of the ionic species in parts per
million (ppm). Note: Determine the formal concentration of CO32–.
Ignore any reactions with water.
Determine the concentrations of MgCl2, Mg2 , and Cl– in a
solution prepared by dissolving 2.51 × 10–4 g MgCl2 in 2.00 L of
water. Express all three concentrations in molarity. Additionally,
express the concentrations of the ionic species in parts per
million (ppm).