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If you dilute 10.0 mL of the stock solution to a final volume of 0.350 L, what will be the...

Question:

If you dilute {eq}10.0\ mL {/eq} of the stock solution to a final volume of {eq}0.350\ L {/eq}, what will be the concentration of the diluted solution?

Dilution of Solution

A diluted solution is attained when water is added to an initial concentrated solution. The volume and concentrations relation is defined by an equation {eq}M_1V_1 = M_2V_2 {/eq}, where {eq}M_1{/eq} is the intial concentration, {eq}V_1{/eq} is the intial volume, {eq}M_2{/eq} is the final concentration, {eq}V_2{/eq} is the intial volume.

Answer and Explanation: 1

Assuming that the concentration of the stock solution is 1 M. The concentration of the diluted solution is calculated using

{eq}M_1V_1 = M_2V_2 {/eq}

where,

  • {eq}M_1 = 1 M {/eq} is the intial concentration,
  • {eq}V_1 = 10.0 \ mL {/eq} is the intial volume
  • {eq}M_2 {/eq} is the final concentration
  • {eq}V_2 = 0.350\ L= 350 \ mL {/eq} is the final volume.

Putting {eq}M_2 {/eq} on one side of the equation and substituting all given values. Therefore,

{eq}M_2 = \dfrac{M_1V_1}{V_2}\\ M_2 = \dfrac{(1\ M)(10.0\ mL)}{350\ mL}\\ \boxed{M_2 = 0.0286\ M} {/eq}


Learn more about this topic:

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Calculating Dilution of Solutions

from

Chapter 8 / Lesson 5
93K

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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