# Question #27485

##### 1 Answer

Here's what I got.

#### Explanation:

For starters, the density given to you is too high for a

https://wissen.science-and-fun.de/chemistry/chemistry/density-tables/density-of-potassium-hydroxide/

I'll do the calculations with the actual value of the density, but feel free to redo the calculations with the value given to you if needed.

Now, assuming that your goal here is to figure out the **molarity** of the solution, start by picking a sample of this potassium hydroxide solution.

To make the calculations easier, let's pick a sample that has a volume of

#"1 dm"^3 = 10^3# #"cm"^3#

In order to find the molarity of the solution, you must find the number of *moles* of solute present in this sample.

Use the **density** of the solution to determine its mass

#10^3 color(red)(cancel(color(black)("cm"^3color(white)(.)"solution"))) * "1.52 g"/(1color(red)(cancel(color(black)("cm"^3color(white)(.)"solution")))) = "1520 g"#

The solution is said to be

You can thus say that your sample will contain

#1520 color(red)(cancel(color(black)("g solution"))) * "50 g KOH"/(100color(red)(cancel(color(black)("g solution")))) = "760 g KOH"#

To convert the mass of potassium hydroxide to *moles*, use the **molar mass** of the compound

#760 color(red)(cancel(color(black)("g"))) * "1 mole KOH"/(56.11color(red)(cancel(color(black)("g")))) = "13.54 moles KOH"#

Since this represents the number of moles of solute present in **molarity** of the solution will be

#color(darkgreen)(ul(color(black)("molarity = 14 mol dm"^(-3))))#

I'll leave the answer rounded to two **sig figs**, but don't forget that you only have one significant figure for the percent concentration of the solution.