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Describe how {eq}500\ ml {/eq} of {eq}0.1\ M {/eq} solution of {eq}\rm NaOH {/eq} can be prepared from {eq}\rm 2.0\ M\ NaOH {/eq}?

Question:

Describe how {eq}500\ ml {/eq} of {eq}0.1\ M {/eq} solution of {eq}\rm NaOH {/eq} can be prepared from {eq}\rm 2.0\ M\ NaOH {/eq}?

Dilution:

In chemistry applications, test solutions are usually prepared from stock or more concentrated solutions. Dilution is the process of reducing the concentration of a solution by adding an appropriate amount of solvent. The dilution equation, {eq}C_1 \times V_1 = C_2 \times V_2{/eq}, is used to calculate for the amount ({eq}V_1{/eq}) of the stock solution ({eq}C_1{/eq}) to be diluted, in order to prepare a less concentrated solution ({eq}C_2{/eq}) with volume {eq}V_2{/eq}.

Answer and Explanation: 1

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{eq}C_1{/eq} = 2.0 M

{eq}V_1{/eq} = ?

{eq}C_2{/eq} = 0.5 M

{eq}V_2{/eq} = 500 ml


Rearrange the dilution equation to calculate for {eq}V_1{/eq}...

See full answer below.


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Calculating Dilution of Solutions

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Chapter 8 / Lesson 5
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Want 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.


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