Calculate the number of moles of solute present in each of the following aqueous solutions: (a) 600 \(\mathrm{mL} .\) of 0.250 \(M \operatorname{SrBr}_{2},(\mathbf{b}) 86.4 \mathrm{g}\) of \(0.180 \mathrm{m} \mathrm{KCl},(\mathrm{c}) 124.0 \mathrm{g}\) of a solution that is 6.45\(\%\) glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) by mass.

To find the number of moles in this solution, we will use the molarity formula: \(moles = Molarity * Volume\). Given: Molarity, M = 0.250 mol/L Volume, V = 600 mL = \(600 *10^{-3}\) L (Converting milliliters to liters) Now, let's plug the values into the formula: \(moles = (0.250) * (600 *10^{-3})\) Calculating the moles, we get: \(moles = 0.15\) mol There are 0.15 moles of SrBr₂ in the solution.

In this case, we are given the mass (Mass_sol) and molality (m) of a KCl solution. The molality formula is: \(molality = moles(sol) / mass(kg) \). We can rearrange this formula to find the moles of solute as: \(moles(sol) = molality * mass(kg) \). Given: Molality, m = 0.180 mol/kg Mass of the solution, Mass_sol = 86.4 g Now, let's plug the values into the formula: \(moles(KCl) = (0.180) * (86.4 *10^{-3})\) (Converting grams to kg) Calculating the moles, we get: \(moles(KCl) = 0.01553\) mol There are 0.01553 moles of KCl in the solution.

In this case, we are given the mass of a glucose solution and its mass percent concentration. We can calculate the mass of glucose in the solution by multiplying the mass of the solution by the mass percent. Then we can use the molar mass of glucose to calculate the number of moles. Given: Mass of solution, Mass_sol = 124.0 g Mass percent of glucose = 6.45 % The mass of glucose in the solution: Mass_glucose = \(124 g * \frac{6.45}{100}\) Calculating the mass, we get: Mass_glucose = 7.998 g The molar mass of glucose, \(C_6 H_{12} O_6\), is calculated as: Molar_mass = \(6 * (12.01 g/mol) + 12 * (1.01 g/mol) + 6 * (16.00 g/mol) = 180.18 g/mol\) Now we can use the mass of glucose and the molar mass to find the moles of glucose: \(moles(glucose) = \frac{Mass_{glucose}}{Molar_{mass}}\) Plugging in the values: \(moles(glucose) = \frac{7.998}{180.18}\) Calculating the moles, we get: \(moles(glucose) = 0.0444\) mol There are 0.0444 moles of glucose in the solution.