50.36 mL 2.74 ✕ 10−2M Pb(NO3)2 is mixed with 25.08 mL 4.68 ✕ 10−5M NaBr. (molar solubility of PbBr2 = 1.2 ✕ 10−2M)
Ksp= 6.912e-6
calculate the Qsp
Someone previously gave me the answer Qsp= 3.66e-10 but this is INNCORRECT
Lets find the concentration after mixing for Pb(NO3)2
Concentration after mixing = mol of component / (total volume)
M(Pb(NO3)2) after mixing = M(Pb(NO3)2*)V(Pb(NO3)2)/(total volume)
M(Pb(NO3)2) after mixing = 0.0274 M*50.36 mL/(50.36+25.08)mL
M(Pb(NO3)2) after mixing = 1.829*10^-2 M
Lets find the concentration after mixing for NaBr
Concentration after mixing = mol of component / (total volume)
M(NaBr) after mixing = M(NaBr*)V(NaBr)/(total volume)
M(NaBr) after mixing = 4.68*10^-5 M*25.08 mL/(25.08+50.36)mL
M(NaBr) after mixing = 1.556*10^-5 M
The salt dissolves as:
PbBr2 <----> Pb2+ + 2 Br-
Qsp = [Pb2+][Br-]^2
Qsp = (1.829*10^-2)*(2*1.556*10^-5)^2
Qsp = 1.771*10^-11
we have,
Ksp = 6.912*10^-6
Since Qsp is less than ksp, precipitate will not form
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