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Answer :
Sure, let's go through the solution step-by-step to determine the molarity of the LiBr solution.
### Step 1: Find the Number of Moles of LiBr
Given:
- Mass of LiBr = 97.7 g
- Molar Mass (MW) of LiBr = 86.85 g/mol
To find the number of moles of LiBr, we use the formula:
[tex]\[
\text{Number of moles} = \frac{\text{Mass}}{\text{Molar Mass}}
\][/tex]
[tex]\[
\text{Number of moles of LiBr} = \frac{97.7 \, \text{g}}{86.85 \, \text{g/mol}} \approx 1.1249 \, \text{mol}
\][/tex]
### Step 2: Convert Volume from mL to L
Given:
- Volume of the solution = 750.0 mL
To convert this to liters:
[tex]\[
\text{Volume in liters} = \frac{\text{Volume in mL}}{1000}
\][/tex]
[tex]\[
\text{Volume in liters} = \frac{750.0 \, \text{mL}}{1000} = 0.75 \, \text{L}
\][/tex]
### Step 3: Calculate the Molarity
Molarity (M) is defined as the number of moles of solute per liter of solution:
[tex]\[
\text{Molarity} = \frac{\text{Number of moles of solute}}{\text{Volume of solution in liters}}
\][/tex]
[tex]\[
\text{Molarity} = \frac{1.1249 \, \text{mol}}{0.75 \, \text{L}} \approx 1.5 \, \text{M}
\][/tex]
### Conclusion:
The molarity of the solution is approximately [tex]\( 1.5 \, \text{M} \)[/tex].
So, the correct answer is:
[tex]\[ 1.50 \, \text{M} \][/tex]
This matches the given options, confirming that our calculations were done correctly.
### Step 1: Find the Number of Moles of LiBr
Given:
- Mass of LiBr = 97.7 g
- Molar Mass (MW) of LiBr = 86.85 g/mol
To find the number of moles of LiBr, we use the formula:
[tex]\[
\text{Number of moles} = \frac{\text{Mass}}{\text{Molar Mass}}
\][/tex]
[tex]\[
\text{Number of moles of LiBr} = \frac{97.7 \, \text{g}}{86.85 \, \text{g/mol}} \approx 1.1249 \, \text{mol}
\][/tex]
### Step 2: Convert Volume from mL to L
Given:
- Volume of the solution = 750.0 mL
To convert this to liters:
[tex]\[
\text{Volume in liters} = \frac{\text{Volume in mL}}{1000}
\][/tex]
[tex]\[
\text{Volume in liters} = \frac{750.0 \, \text{mL}}{1000} = 0.75 \, \text{L}
\][/tex]
### Step 3: Calculate the Molarity
Molarity (M) is defined as the number of moles of solute per liter of solution:
[tex]\[
\text{Molarity} = \frac{\text{Number of moles of solute}}{\text{Volume of solution in liters}}
\][/tex]
[tex]\[
\text{Molarity} = \frac{1.1249 \, \text{mol}}{0.75 \, \text{L}} \approx 1.5 \, \text{M}
\][/tex]
### Conclusion:
The molarity of the solution is approximately [tex]\( 1.5 \, \text{M} \)[/tex].
So, the correct answer is:
[tex]\[ 1.50 \, \text{M} \][/tex]
This matches the given options, confirming that our calculations were done correctly.
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Rewritten by : Jeany
