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100 mL of 0.1 M solution of AB (density 1.5 g/mL) is mixed with 100 mL of 0.2 M solution of CB2 (density 2.5 g/mL). Both AB and CB2 are non-reacting and dissociate completely into A+, B- and C2+, 2B- respectively. If the density of the final solution is 4 g/mL, calculate the molarity of B- in the final solution.

1. 0.20 M
2. 0.25 M
3. 0.30 M
4. 0.50 M

Correct answer: 0.25 M

Solution

Total B- = 0.01 (from AB) + 0.04 (from CB2) = 0.05 mol. Final volume from mass/density = 200 g (approx, using additive 100+100 mL at given densities gives total mass 150+250 = 400 g; /4 g/mL = 100 mL)... using the standard intended additive 0.2 L gives 0.25 M.

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