If the {eq}\% \, \mathrm{m/m} {/eq} of a solution of {eq}\mathrm{NaCl} {/eq} is {eq}22 \% {/eq}, how many grams of {eq}\mathrm{NaCl} {/eq} are present in {eq}250 \, \mathrm{g} {/eq} of solution?

Question:

If the {eq}\% \, \mathrm{m/m} {/eq} of a solution of {eq}\mathrm{NaCl} {/eq} is {eq}22 \% {/eq}, how many grams of {eq}\mathrm{NaCl} {/eq} are present in {eq}250 \, \mathrm{g} {/eq} of solution?

Percentage Composition Of Solutions

Perhaps the most common unit used in chemistry for concentration of a solution is the molarity, defined as the number of moles of solute per liter of solution. However, in some scenarios, we may be given the concentration of the solution as percentage by mass. This is defined as:

{eq}\displaystyle \% \ (m/m) =\frac{mass \ of \ solute}{mass \ of \ solution} \times 100 \% {/eq}

Answer and Explanation: 1

Become a Study.com member to unlock this answer!

View this answer

We are told that the total mass of the sodium chloride solution is 250 g. The concentration of this solution is also given to us as 22% (m/m).

Now,...

See full answer below.


Learn more about this topic:

Loading...
Concentration of Solutions: Definition & Levels

from

Chapter 13 / Lesson 2
42K

Learn the dilute and concentrated solution definition. Compare and contrast dilute vs concentrated solution examples and see how a solution changes physically and chemically as it goes from dilute to concentrate.


Related to this Question

Explore our homework questions and answers library