Question

A student correctly determines that 17.1 grams of sucrose are needed to make 50 ml of a 1m sucrose solution. when making the solution in the lab, the student measured 50ml of solution and then adds the 17.1 grams of sucrose to the beaker. the student’s resulting solution was not 1m as intended. after the student mixed the solution, the resulting solution was measured at 62ml.

Answer 1

The initial and final molarity are 0.860 molars and 0.694 molars, respectively.

How to calculate molarity in a solution

In chemistry, molarity ($M$), in molars, is described by the following expression:

$M = \frac{n}{V}$   (1)

Where:

• $n$ - Molar amount of the solute, in moles
• $V$ - Volume of the solution, in liters

The molar amount of the solute is determined by this formula:

$n = \frac{m}{M}$   (2)

Where:

• $m$ - Mass of the solute, in grams
• $M$ - Molar mass, in moles per grams

If we know that $m = 17.1\,g$, $M = 397.64\,\frac{g}{mol}$, $V_{1} = 0.050\,L$ and $V_{2} = 0.062\,L$, then the initial and final molarities are, respectively:

$n = \frac{17.1\,g}{397.64\,\frac{g}{mol} }$

$n = 0.043\,mol$

Initial molarity

$M_{1} = \frac{0.043\,mol}{0.050\,L}$

$M_{1} = 0.860\,M$

Final molarity

$M_{2} = \frac{0.043\,mol}{0.062\,L}$

$M_{2} = 0.694\,M$

The initial and final molarity are 0.860 molars and 0.694 molars, respectively. $\blacksquare$

Remark

The statement is incomplete, complete form is described below:

A student correctly determines that 17.1 grams of sucrose are needed to make 50 ml of a 1m sucrose solution. when making the solution in the lab, the student measured 50ml of solution and then adds the 17.1 grams of sucrose to the beaker. the student’s resulting solution was not 1m as intended. after the student mixed the solution, the resulting solution was measured at 62ml. What are the initial and final concentrations of the solution?

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