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Calculate the molar solubility of lead thiocyanate in 1.00 M KSCN.

Karen Wright

in Chemistry

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Ashley Howard on February 11, 2018

You have to make an assumption or estimate here: (I don't think that around the 1.00 M KSCN)From 1.00 M KSCN provides a source of ions, SCN-. Therefore, you will have a 1.00 M of SCN-.[Pb+2][SCN-] ~ 0.02 0.01 x^2 = 4E-6 Pb(SCN)2 <---> Pb++ + 2SCN - Bring 1.00 M SCN - new in the problem. 1.00 M + 0.02 M, ignoring the SCN-, and the calculation of the [Pb+2]: Ksp = [Pb++][SCN-]^2 2.00 E-5 = [Pb++](1.00)^2 [Pb++] = 2.00 E-5 M The mass balance shows that: [Pb++] = [Pb(SCN)2] [Pb(SCN)2] = 2.00 E-5 M 1.00 M KSCN.


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