Final answer:
To calculate the molar concentration of the metal (ii) ion from an absorbance measurement, the Beer-Lambert law would be used, requiring knowledge of the molar absorptivity and path length. However, these values are not provided. Instead, an example of calculating molar concentration is given where the moles of solute and volume of solution are used.
Step-by-step explanation:
The student is asking about determining the molar concentration of a metal (ii) ion in a solution given an absorbance measurement. Absorbance can be related to concentration through the Beer-Lambert law, which states that absorbance (A) is equal to the molar absorptivity (epsilon, ε), the path length of the sample (l), and the concentration (c) of the absorbing species in solution; this relationship is given by A = εl…c.
To calculate the molar concentration from absorbance, you would need the molar absorptivity and path length, neither of which are provided here. However, sample problems generally use similar principles. For example, in calculating molar concentrations, if we know the amount of substance in moles and the volume of the solution, we can use the formula:
Molar Concentration (M) = Moles of solute (mol) ÷ Volume of solution (L)
Example Calculation:
A 355-mL soft drink sample contains 0.133 mol of sucrose. We can convert the volume from milliliters to liters (355 mL = 0.355 L) and then substitute these values into the formula:
M = 0.133 mol ÷ 0.355 L = 0.375 M