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To what volume should you dilute 0.200 L of a 18 M HCl solution to obtain 1.0 M HCl?

Question:

To what volume should you dilute 0.200 L of a 18 M HCl solution to obtain 1.0 M HCl?

Dilution Equation:

The dilution equation is often used to determine the volumes and concentrations of a stock solution to prepare a more dilute solution. Aside from acquiring these values, the dilution equation also shows that the moles of solute present does not change. Dilution is a technique that involves adding solvent to a certain volume. As a consequence, the moles of solute remains unchanged. The dilution equation is written as:

solution. The equation for dilution is given below.

{eq}\rm C_1V_1~=~C_2V_2 {/eq}

Where:

  • C1 is the concentration of the initial solution
  • C2 is the concentration of the final solution
  • V1 is the initial volume of the solution.
  • V2 is the final volume of the solution.

Answer and Explanation:


We can begin by identifying the given values. Based on the question, we are interested in determining V2

{eq}\rm V_2 = \dfrac{C_1V_1}{C_2} {/eq}

Given:

  • C1 = 18 M
  • C2 = 1.0 M
  • V1 0.200 L


Plugging in the given values, we get the volume to dilute the 0.200 L of 18 M HCl.

{eq}\rm V_2 = \dfrac{(18~M)(0.200~L)}{(1.0~M)} \\ \boxed{ \; \rm V_2 = 3.6~L \; } {/eq}


Learn more about this topic:

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Calculating Dilution of Solutions

from

Chapter 8 / Lesson 5
69K

Learn what a solution is and how to properly dilute a new solution from a stock solution. Learn the dilution equation that combines molarity, the volume of stock solution and desired solution to determine how much stock solution is needed for the new solution.


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