1. If a solution contains 4.37g of C6H6 and 9.42g of CCl4. What is the molarity of the solution if the solution density is 1.59 g/mL?
A) 7.09
B) 6.45
C) 5.93
D) 0.405
E) 9.44
Please show the steps to solve it as I do not know, thank you for your time.
In the given solution, C6H6 is solute and CCl4 is the solvent.
Mass of solution = Mass of solute (C6H6) + mass of solvent (CCl4)
= 4.37 g + 9.42 g
= 13.79 g
Density of solution = 1.59 g/mL
Calculate the volume of solution as given below
Volume of solution = mass of solution / density of solution
= (13.79 g)/(1.59 g/mL)
= 8.67 mL
= (8.67/1000) L
= 0.00867 L
Volume of solution = 0.00867 L
Molar mass of C6H6 = 78.11 g/mol
No. of moles of C6H6 = (mass of C6H6)/(molar mass of C6H6)
= (4.37 g)/(78.11 g/mol)
= 0.0559 mol
Now, calculate the molarity of the solution using following formula
Molarity of solution = (No. of moles of C6H6)/(Volume of the solution)
= (0.0559 mol)/(0.00867 L)
= 6.45 M
Molarity of solution = 6.45 M
Thus, Option B) = 6.45 M is correct.
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