To what volume must {eq}10.0 \ ml{/eq} of {eq}5.00 \ M \ HCl{/eq} be diluted to make a {eq}0.500 \ M \ HCl{/eq} solution ?

## Question:

To what volume must {eq}10.0 \ ml{/eq} of {eq}5.00 \ M \ HCl{/eq} be diluted to make a {eq}0.500 \ M \ HCl{/eq} solution ?

## Diluting solutions

The concentration of a solution is typically reported by molarity. Molarity (M) is the concentration of the solute based on moles of solute per liter of solution. A solution of higher concentration may be diluted to create a solution of lesser concentration. In order to perform these calculations the molarity and volume of the first solution are set equal to that of the second solution as shown:

{eq}M_1 \times V_1 = M_2 \times V_2{/eq}

## Answer and Explanation: 1

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View this answerUse the following equation to determine the volume of the second solution ({eq}V_2{/eq}) .

{eq}M_1 \times V_1 = M_2 \times V_2{/eq}

{eq}M_1= 5.00 \,...

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Chapter 8 / Lesson 5Want to know how to calculate dilution factor? See dilution equations, the dilution formula, and learn how to dilute acid and how to dilute a solution.