# Question #4e23c

##### 1 Answer

#### Answer:

#### Explanation:

The first thing to do here is to pick a **volume** of this ammonium sulfate, **density** to find its *mass*.

Since **molarity** is defined as moles of solute **per cubic decimeters of solution**, pick a

This

#1 color(red)(cancel(color(black)("dm"^3))) * (10^3"mL")/(1color(red)(cancel(color(black)("dm"^3)))) = 10^3"cm"^3#

sample has a density of **for every cubic centimeter** of solution. In your case, the sample will have a mass of

#10^3 color(red)(cancel(color(black)("cm"^3))) * "1.10 g"/(1color(red)(cancel(color(black)("cm"^3)))) = "1100 g"#

Now, this solution is said to be **by mass**. This tells you will get **for every**

#1100color(red)(cancel(color(black)("g solution"))) * ("18 g"color(white)(a)("NH"_4)_2"SO"_4)/(100color(red)(cancel(color(black)("g solution")))) = "198 g"color(white)(a)("NH"_4)_2"SO"_4#

To find the **number of moles** of ammonium sulfate present in **molar mass**

#198 color(red)(cancel(color(black)("g"))) * ("1 mole"color(white)(a)("NH"_4)_2"SO"_4)/(132.14color(red)(cancel(color(black)("g")))) = "1.4984 moles"color(white)(a)("NH"_4)_2"SO"_4#

Finally, the molarity of the solution will be -- keep in mind that your sample has a volume of

#c = "1.4984 moles"/"1 dm"^3 = color(green)(|bar(ul(color(white)(a/a)color(black)("1.5 mol dm"^(-3))color(white)(a/a)|)))#

The answer is rounded to two **sig figs**, the number of sig figs you have for the concentration of the soltuion.