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Calculate the ionic strength in a solution that contains 0.010 mol KCl, 0.005 mol MgCl2, 0.002...

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Chemistry

Calculate the ionic strength in a solution that contains 0.010mol KCl, 0.005 mol MgCl2, 0.002 mol MgSO4, and 100g H2O.

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3.9 Ratings (650 Votes)

density of water =1 g/cc

volume of water (v) = m/D = 100/1 = 100 ml

concentration of Kcl = n/V in L

                     = 0.01/0.1 = 0.001 M

concentration of MgCl2 = n/Vin L

                         = 0.005/0.1

                        = 0.0005 M

   concentration of MgSO4 = n/Vin L

                         = 0.002/0.1

                        = 0.0002 M

Ionic strength(I) = 1/2*epsilon(Ci*Zi^2)

Ci = molarconcentration of ion i

Zi = charge number of ion i

I = 1/2([K+]*(+1)^2+[Cl-]*(-1)^2+[Mg^2+]*(+2)^2+[Cl-]*(-1)^2+[Mg^2+]*(+2)^2+[SO4^2-]*(-2)^2)

    = 1/2*((0.001*(+1)^2)+(0.001*(-1)^2)+(0.0005*(+2)^2)+(0.0005*2*(-1)^2)+(0.0002*(+2)^2)+(0.0002*(-2)^2))

Ionicstrength(I) = 0.0033 M
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