27 November, 15:02

# What is the molarity of 2.0 liters of an aqueous solution that contains 0.50 mol of potassium iodide

+1
1. 27 November, 16:11
0
0.25mol/L

Explanation:

Data obtained from the question include:

Mole of solute (KI) = 0.50 mol

Volume of solution = 2L

Molarity = ?

Molarity is simply the mole of solute per unit litre of the solution. It is represented mathematically as:

Molarity = mole of solute / Volume of solution

Molarity = 0.50mol/2L

Molarity = 0.25mol/L

Therefore, the molarity of the solution is 0.25mol/L
2. 27 November, 16:33
0
[KI] = 0.25 M

Explanation:

Solute: KI

Mass of solute: 0.50 mol. 166 g / 1mol = 83 g

Our solution volume is 2L

Molarity is a kind of concentration, defined as the moles of solute contained in 1L of solution. It is the most common concentration for all solutions while there are any other kind, for example molality, mole fraction or ppm.

In this case molarity (mol/L) is 0.5 mol / 2L = 0.25 M

In conclussion, solution is 0.25 molar whichs is the same to say, that 0.25 moles of potassium iodide are contained in 1L of solution.

With the data given, we can also make a rule of three:

2L of solution contain 0.5 moles of KI

Then, 1L of solution may contain (0.5. 1) / 2 = 0.25 moles of Ki