What Volume of a 0.120 M CaI2 Solution Would Contain 0.078 mol of the Solute?: Mole Calculation
What Volume of a 0.120 M CaI2 Solution Would Contain 0.078 mol of the Solute?
Have you ever wondered how to calculate the volume of a solution that contains a specific amount of solute? Well, in this article, I’ll walk you through the process step by step. Today, we’ll focus on finding the volume of a 0.120 M CaI2 solution that would contain 0.078 mol of the solute.
To determine the volume, we first need to understand what these numbers mean. The concentration of a solution is given in moles per liter (M), while the amount of solute is measured in moles (mol). So, we’re essentially looking for the volume (in liters) required to hold 0.078 mol of CaI2 in our 0.120 M solution.
By using a simple formula involving concentration and volume, we can find our answer. This calculation will help us determine exactly how much solution is needed to achieve our desired concentration and amount of solute.
So, if you’re ready to dive into some chemistry calculations and learn how to find the right volume for your solution, let’s get started!
Calculating the Molar Mass of CaI2
Let’s dive into the process of calculating the molar mass of CaI2. Molar mass is a crucial concept in chemistry as it helps us determine the amount of substance present in a given sample.
To calculate the molar mass of CaI2, we need to consider the individual atomic masses of calcium (Ca) and iodine (I). The atomic mass represents the average mass of an atom, taking into account its isotopes and their abundances.
Here’s how we can calculate the molar mass step by step:
- Identify the atomic masses: The atomic mass of calcium is approximately 40.08 grams per mole (g/mol), while iodine has an atomic mass of around 126.90 g/mol.
- Determine the number of atoms: In one molecule of CaI2, there is one calcium atom and two iodine atoms.
- Multiply and sum: Multiply each atomic mass by its respective number of atoms, then sum these products together to find the molar mass.
- Calcium: 1 atom * 40.08 g/mol = 40.08 g/mol
- Iodine: 2 atoms * 126.90 g/mol = 253.80 g/mol
- Total molar mass: 40.08 g/mol + 253.80 g/mol = 293.88 g/mol
Therefore, we find that the molar mass of CaI2 is approximately 293.88 grams per mole.
Understanding how to calculate molar masses is essential for various applications in chemistry, such as determining stoichiometry proportions or preparing solutions with precise concentrations.
By utilizing this knowledge, you’ll be able to solve problems like determining what volume of a solution contains a specific number of moles, just like our initial question regarding a particular volume containing 0.078 mol solute in a 0.120 m CaI2 solution.
Remember, the molar mass of a compound provides valuable information that enables us to make accurate calculations and predictions within the realm of chemistry.
Determining the Number of Moles in the Solution
To find out what volume of a 0.120 M CaI2 solution would contain 0.078 mol of the solute, we need to calculate the number of moles present in the given solution. This information will then help us determine the required volume.
Here’s how we can go about it:
- Start with the given data: We are provided with a concentration of 0.120 M and a certain number of moles, which is 0.078 mol.
- Recall the formula for calculating moles: Moles = Concentration × Volume.
- Rearrange the formula to solve for volume: Volume = Moles / Concentration.
- Substitute the given values into the equation: Volume = 0.078 mol / 0.120 M.
- Perform the calculation: Volume = 0.65 L (rounded to two decimal places).
So, to contain 0.078 mol of CaI2 solute, we would need approximately 0.65 liters (or 650 milliliters) of a CaI2 solution with a concentration of 0.120 M.
In summary:
- Given concentration: 0.120 M
- Given number of moles: 0.078 mol
- Required volume: Approximately 650 mL or 0.65 L
Remember that this calculation assumes ideal behavior and no change in volume upon mixing components.
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