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vovikov84 [41]
3 years ago
5

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

Chemistry
1 answer:
Rzqust [24]3 years ago
7 0
You have to make an assumption or estimation here: (don't think about the 1.00 M KSCN)
Since 1.00M KSCN provides a common ion source of SCN-. Therefore, you will have a <span>1.00 M SCN-.
</span><span>[Pb+2][SCN-] ~ 0.01 x 0.02^2 = 4E-6 
</span> Pb(SCN)2 <---> Pb++ + 2SCN- <span>

</span>Bringing 1.00M SCN- back in the problem. 1.00M + 0.02M, ignoring the SCN-, and calculating the <span> [Pb+2]: 
</span><span>
</span><span>Ksp = [Pb++][SCN-]^2 
</span>2.00E-5 = [Pb++](1.00)^2 

<span>[Pb++] = 2.00E-5 M </span>

<span>The mass balance shows that: </span>

<span>[Pb++] = [Pb(SCN)2] </span>

So [Pb(SCN)2] = 2.00E-5 M in 1.00 M KSCN.
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