Solution
Molality of AgCl=0.135 m
Density of 0.135 m solution = 1.22 g/mL
Volume of solution in mL = 244 mL
mass of solution in g = volume of solution x Density = 244 mL x 1.22 g/mL
mass of solution in g = 297.68 g (i.e. 297.68 / 1000 = 0.298 kg)
we know
molality = number of mole solute / volume of solution in kg
0.135 mol /kg = number of mole AgCl / 0.298 kg
Number of mole AgCl = 0.135 mol /kg x 0.298 kg
Number of mole AgCl = 0.04023 moles
Number of mole AgCl = 4.023 x 10-2 moles
so ans 2 is correct
The correct answer is 3.49e-2
How many moles of AgCl are contained in 244 ml of 0.135 m AgCl solution? The density of the solution is 1.22 g/mL...
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