What volume, in liters, of 4.0 M LiBr solution can be made using 100.0 g LiBr?
[tex]LiBr : 86.44 g / mol[/tex]
Answer (2)
The volume of the 4.0 M LiBr solution that can be made using 100.0 g of LiBr is approximately 0.289 liters. This is calculated by first determining the number of moles of LiBr and then using that value to find the solution's volume. The process involves applying formulas for moles and volume based on molarity.
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0.289 L
Explanation
Problem Analysis We are given the mass of L i B r (100.0 g), the molar mass of L i B r (86.44 g/mol), and the molarity of the L i B r solution (4.0 M). We need to find the volume of the solution in liters.
Calculating Moles of LiBr First, we need to calculate the number of moles of L i B r using the formula: m o l es = m o l a r _ ma ss ma ss Substituting the given values: m o l es = 86.44 g/mol 100.0 g = 1.157 mol
Calculating Volume of Solution Next, we can calculate the volume of the solution using the formula: v o l u m e = m o l a r i t y m o l es Substituting the calculated moles and given molarity: v o l u m e = 4.0 M 1.157 mol = 0.289 L
Final Answer Therefore, the volume of the 4.0 M L i B r solution that can be made using 100.0 g of L i B r is approximately 0.289 L.
Examples
In a chemistry lab, you might need to prepare solutions of specific concentrations for experiments. Knowing how to calculate the volume of a solution given the mass of the solute and the desired molarity is crucial. For example, if you need to prepare a 4.0 M LiBr solution for a reaction, you can use this calculation to determine the exact volume of solution you can make with a given amount of LiBr. This ensures accurate and reproducible results in your experiments. The calculation of molarity and volume is fundamental in fields like pharmaceuticals, environmental science, and materials science, where precise concentrations are essential for research and development.
