This question asks how a statement is correct that claims that whendensity of th

Question

This question asks how a statement is correct that claims that whendensity of the solution is equal to density of the pure solvent themolarity of the solution is equal to the molality. It wantsan answer supporting a .010M aqueous urea (NH2)2CO solution.
I'm not sure about how to go through with the proof... thanks:) I need to know the logic behind the question, not just that .01Mequals .01m.
I'm not sure about how to go through with the proof... thanks:) I need to know the logic behind the question, not just that .01Mequals .01m.

Explanation / Answer

                      Molarityof the urea solution = 0.01 M        0.01 M ureasolution has 0.01 moles in 1 L ( 1000 mL )soltion.       Molality is the number of molesof solute pesent in 1 Kg of the solution.                 Molality = (number of moles of ures /  mass of solution (g) ) x 1000                                   = (number of moles of ures /  density ofsolution x volume of solution ) x 1000             Sinceit is an aqeous solution , density of puresolvent ( water ) = 1 g/ mL            If the density of the solution is equal to the density ofthe pure solvent then ,                Molality = 0.01 mol/ 1 g/mL x  1000 mL )x 1000                                = 0.01 m          Hence the molarity of solution is equal to the molality .

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