Welcome to Westonci.ca, the place where your questions are answered by a community of knowledgeable contributors. Get immediate answers to your questions from a wide network of experienced professionals on our Q&A platform. Experience the ease of finding precise answers to your questions from a knowledgeable community of experts.
Sagot :
To determine the volume of a 1.5 M [tex]\( CaCl_2 \)[/tex] solution that can be made using 1200.0 grams of [tex]\( CaCl_2 \)[/tex], follow these steps:
1. Identify the molar mass of [tex]\( CaCl_2 \)[/tex]:
[tex]\[ \text{Molar mass of \( CaCl_2 \)} = 110.98 \, \text{g/mol} \][/tex]
2. Calculate the moles of [tex]\( CaCl_2 \)[/tex] needed:
First, divide the given mass of [tex]\( CaCl_2 \)[/tex] by its molar mass to find the number of moles.
[tex]\[ \text{Moles of \( CaCl_2 \)} = \frac{\text{Mass of \( CaCl_2 \)}}{\text{Molar mass of \( CaCl_2 \)}} \][/tex]
[tex]\[ \text{Moles of \( CaCl_2 \)} = \frac{1200.0 \, \text{g}}{110.98 \, \text{g/mol}} \][/tex]
From the previous analysis, it can be affirmed that:
[tex]\[ \text{Moles of \( CaCl_2 \)} \approx 10.812759055685708 \, \text{moles} \][/tex]
3. Use the molarity to find the volume of the solution:
Molarity (M) is defined as the number of moles of solute per liter of solution. Rearranging this definition, we find the volume:
[tex]\[ \text{Volume of solution (in liters)} = \frac{\text{Moles of solute}}{\text{Molarity}} \][/tex]
Given that the molarity is 1.5 M:
[tex]\[ \text{Volume of solution} = \frac{10.812759055685708 \, \text{moles}}{1.5 \, \text{M}} \][/tex]
4. Calculate the volume:
[tex]\[ \text{Volume of solution} = \frac{10.812759055685708}{1.5} \][/tex]
[tex]\[ \text{Volume of solution} \approx 7.208506037123805 \, \text{liters} \][/tex]
Therefore, using 1200.0 grams of [tex]\( CaCl_2 \)[/tex], you can prepare approximately 7.2085 liters of a 1.5 M [tex]\( CaCl_2 \)[/tex] solution.
1. Identify the molar mass of [tex]\( CaCl_2 \)[/tex]:
[tex]\[ \text{Molar mass of \( CaCl_2 \)} = 110.98 \, \text{g/mol} \][/tex]
2. Calculate the moles of [tex]\( CaCl_2 \)[/tex] needed:
First, divide the given mass of [tex]\( CaCl_2 \)[/tex] by its molar mass to find the number of moles.
[tex]\[ \text{Moles of \( CaCl_2 \)} = \frac{\text{Mass of \( CaCl_2 \)}}{\text{Molar mass of \( CaCl_2 \)}} \][/tex]
[tex]\[ \text{Moles of \( CaCl_2 \)} = \frac{1200.0 \, \text{g}}{110.98 \, \text{g/mol}} \][/tex]
From the previous analysis, it can be affirmed that:
[tex]\[ \text{Moles of \( CaCl_2 \)} \approx 10.812759055685708 \, \text{moles} \][/tex]
3. Use the molarity to find the volume of the solution:
Molarity (M) is defined as the number of moles of solute per liter of solution. Rearranging this definition, we find the volume:
[tex]\[ \text{Volume of solution (in liters)} = \frac{\text{Moles of solute}}{\text{Molarity}} \][/tex]
Given that the molarity is 1.5 M:
[tex]\[ \text{Volume of solution} = \frac{10.812759055685708 \, \text{moles}}{1.5 \, \text{M}} \][/tex]
4. Calculate the volume:
[tex]\[ \text{Volume of solution} = \frac{10.812759055685708}{1.5} \][/tex]
[tex]\[ \text{Volume of solution} \approx 7.208506037123805 \, \text{liters} \][/tex]
Therefore, using 1200.0 grams of [tex]\( CaCl_2 \)[/tex], you can prepare approximately 7.2085 liters of a 1.5 M [tex]\( CaCl_2 \)[/tex] solution.
Thank you for choosing our service. We're dedicated to providing the best answers for all your questions. Visit us again. We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. Westonci.ca is here to provide the answers you seek. Return often for more expert solutions.