Final answer:
Using the given molality (0.0710 m), density of solution (1.1 g/mL), and density of water (0.997 g/mL), the molarity of the KBr solution is calculated. The answer, however, does not match any of the provided options, leading to the conclusion 'e) None of the above'.
Step-by-step explanation:
To calculate the molarity of the aqueous solution of KBr from its molality, you need to use the given data: the solution's molality (0.0710 m), the density of the solution (1.1 g/mL), and the density of water (0.997 g/mL). The molality of a solution is defined as the number of moles of solute per kilogram of solvent, whereas molarity is the number of moles of solute per liter of solution.
To find the molarity (M), you can convert mass to moles using the molar mass of KBr (119 g/mole). First, we calculate the total mass of 1 liter of solution, which is 1.1 g/mL × 1000 mL = 1100 g. Next, deduct the mass of KBr to find the mass of the solvent (water). Assuming molality and molarity for dilute solutions are roughly equivalent, 1 kg of water is approximately 1 L, we can use the molality directly to calculate moles of KBr. Hence, 0.0710 mol of KBr is present in 1 kg of water. To calculate molarity, divide moles of solute by the volume of the solution in liters. If 0.0710 moles of KBr is in 1 L, the molarity is also 0.0710 M. Since we're given a non-standard density, we'll need to find the actual volume of the solvent water in our solution after accounting for the mass of KBr dissolved in it.
To find the mass of KBr, we use the mass fraction obtained by dividing the density of the solution by the density of water: 1.1 g/mL ÷ 0.997 g/mL, yielding a mass of KBr of approximately 71 g (since 1000 mL × (1.1 - 0.997) g/mL). Using the molar mass of KBr, we convert this mass to moles, divide by the volume of the solution in liters to find the molarity. However, neither option a) 0.0541 M, b) 0.0774 M, c) 0.0517 M, nor d) 0.0580 M matches the calculations made, so our answer would be e) None of the above.