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0.13 mol of TiCl4 is dissolved in water to produce a solution with a concentration of 2 M. What is the volume of this solution in liters?

Question

What is the volume of the solution in liters if 0.13 mol of TiCl4 is dissolved in water to produce a solution with a concentration of 2 M?

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Solution

1. Break Down the Problem

To find the volume of the solution, we need to use the relationship between moles, concentration, and volume. The formula that relates these is:

Concentration (M)=Number of moles (mol)Volume (L) \text{Concentration (M)} = \frac{\text{Number of moles (mol)}}{\text{Volume (L)}}

2. Relevant Concepts

We rearrange the formula to solve for volume:

Volume (L)=Number of moles (mol)Concentration (M) \text{Volume (L)} = \frac{\text{Number of moles (mol)}}{\text{Concentration (M)}}

3. Analysis and Detail

We know:

  • The number of moles of TiCl4 = 0.13 mol
  • The concentration of the solution = 2 M

Now, substituting the values into the rearranged formula:

Volume (L)=0.13mol2M \text{Volume (L)} = \frac{0.13 \, \text{mol}}{2 \, \text{M}}

4. Verify and Summarize

Calculating the volume:

Volume (L)=0.132=0.065L \text{Volume (L)} = \frac{0.13}{2} = 0.065 \, \text{L}

Final Answer

The volume of the solution is 0.065L0.065 \, \text{L}.

This problem has been solved

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