Ksp Problem Set - Widener University
Ksp Problem Set - Widener University
Ksp Problem Set - Widener University
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.0.3295 g BaF 2 dissolves in 250.0 mL of water at 25 °C<br />
mass :=<br />
0.3295⋅gm<br />
V :=<br />
250.0⋅mL<br />
MW BaF2 := ( 137.329 + 18.998⋅2) ⋅gm⋅<br />
mole − 1<br />
mass<br />
mole BaF2 := mole BaF2 = 1.879 × 10 − 3 mol<br />
MW BaF2<br />
M<br />
mole BaF2<br />
:= M 7.517 10 − 3 − 1<br />
= × mole⋅liter<br />
V<br />
The molar solubility is simply the concentration of the solution at equlibrium:<br />
M 7.517 × 10 − 3 − 1<br />
=<br />
mole⋅liter<br />
Since BaF 2 --> Ba 2+ + 2 F -<br />
K sp_BaF2 := 4⋅M 3<br />
K sp_BaF2 = 1.699 × 10 − 6<br />
⎛<br />
⎜<br />
⎝<br />
mole<br />
liter<br />
⎞<br />
⎟<br />
⎠<br />
3<br />
ksp_a.mcd<br />
3/25/2004<br />
2 S.E. Van Bramer<br />
svanbram@science.widener.edu