Question

What is the molarity of an aqueous solution that contains 0.072 g C2H6O2 per gram of solution? The density of the solution is 1.40 g/mL.

Answer 1

Answer:

1.626 M

Explanation:

Let's start by calculating how many grams of C₂H₆O₂ are there per mL of solution:

• 1 mL of solution weighs 1.40 g.

• 1.40 g of solution * $\frac{0.072gC_2H_6O_2}{1gsolution}$ =0.1008 g C₂H₆O₂

So the C₂H₆O₂ concentration can be expressed as 0.1008 g/mL.

Now we convert g/mL to molarity, using the molar mass of C₂H₆O₂:

• 0.1008 g C₂H₆O₂ ÷ 62 g/mol = 1.626x10⁻³ mol C₂H₆O₂

(1 mL = 0.001 L)

• 1.626x10⁻³ mol C₂H₆O₂ / 0.001 L = 1.626 M

Answer 2

The molarity of the solution is given as 1.626M

We can calculate the mass of C₂H₆O₂ in  mL of solution:

1 mL of solution weighs 1.40 g.

1.40 g of solution × 0.072/1

=0.1008 g C₂H₆O₂

C₂H₆O₂ concentration =  0.1008 g/mL.

Conversion of  g/mL to molarity

0.1008 g C₂H₆O₂ ÷ 62 g/mol = 1.626x10⁻³ mol C₂H₆O₂

(1 mL = 0.001 L)

1.626x10⁻³ mol C₂H₆O₂ / 0.001 L = 1.626 M

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