4. An experiment similar to the one described in this module was performed to determine the solubility and solubility product constant of lead(ll) chloride (gmm = 278.10). The equilibrium involved is PbCl2(s) Pb2+ (aq)+2 CI¯(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO, solution. The solid AgCl was filtered from solution, dried, and weighed. The following data were obtained for three samples of the filtered, saturated solution. determination 1 temperature of solution, °C volume of PbCl2 solution analyzed, mL mass of dry AgCI, g 20.2 20.4 20.1 25.00 22.00 20.10 0.2543 0.2276 0.2051 Calculate the following: number of moles of: AgCl(s) Cl- (aq) Pb2*(aq) (CI"] in PbCl2 solution, M [Pb2+1 in PbCl2 solution, M Ksp average Ksp solubility of P6C12, in g per 100 mL chemistry handbook value for solubility at 20°, g per 100 mL

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Chapter1: Chemical Foundations
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4. An experiment similar to the one described in this module was performed to determine the solubility
and solubility product constant of lead(1l) chloride (gmm = 278.10). The equilibrium involved is
PbCl2(s) =
Pb2+ (aq) +2 CI¯(aq)
The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition
of excess AgNO3 solution. The solid AgCI was filtered from solution, dried, and weighed. The
following data were obtained for three samples of the filtered, saturated solution.
determination
1
2
temperature of solution, °C
volume of PbCl2 solution analyzed, mL
mass of dry A£CI, g
20.2
20.4
20.1
25.00
22.00
20.10
0.2543
0.2276
0.2051
Calculate the following:
number of moles of:
AgCl(s)
CI- (aq)
Pb2*(aq)
[CI"] in PbCl2 solution, M
[Pb2+] in PbCl, solution, M
Ksp
average Ksp
solubility of PbCl2, in g per
100 mL
chemistry handbook value for
solubility at 20°, g per 100 mL
Transcribed Image Text:4. An experiment similar to the one described in this module was performed to determine the solubility and solubility product constant of lead(1l) chloride (gmm = 278.10). The equilibrium involved is PbCl2(s) = Pb2+ (aq) +2 CI¯(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO3 solution. The solid AgCI was filtered from solution, dried, and weighed. The following data were obtained for three samples of the filtered, saturated solution. determination 1 2 temperature of solution, °C volume of PbCl2 solution analyzed, mL mass of dry A£CI, g 20.2 20.4 20.1 25.00 22.00 20.10 0.2543 0.2276 0.2051 Calculate the following: number of moles of: AgCl(s) CI- (aq) Pb2*(aq) [CI"] in PbCl2 solution, M [Pb2+] in PbCl, solution, M Ksp average Ksp solubility of PbCl2, in g per 100 mL chemistry handbook value for solubility at 20°, g per 100 mL
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