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

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

samueladesida43 samueladesida43 · Answer 2 · 2022-01-24T12:59:45+01:00

The molarity of 2.0 liters of an aqueous solution that contains 0.50 mol of potassium iodide is 0.25M.

HOW TO CALCULATE MOLARITY:

The molarity of a solution can be calculated by dividing the number of moles by its volume. That is;

Molarity = no. of moles ÷ volume

According to this question, 2.0 liters of an aqueous solution that contains 0.50 mol of potassium iodide. The molarity is calculated as follows:

Molarity = 0.50mol ÷ 2L

Molarity = 0.25M

Therefore, the molarity of 2.0 liters of an aqueous solution that contains 0.50 mol of potassium iodide is 0.25M.

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