Calculate the number of moles of solute present in each of the following aqueous solutions: (a) \(750 \mathrm{~mL}\) of \(0.120 \mathrm{M}\) \(\operatorname{SrBr}_{2},(\mathbf{b}) 70.0 \mathrm{~g}\) of $0.200 \mathrm{~m} \mathrm{KCl},(\mathbf{c}) 150.0 \mathrm{~g}\( of a solution that is \)5.75 \%$ glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) by mass.

Short Answer

Expert verified
In summary, we have the following number of moles of solute in each solution: (a) \(0.090\) moles of \(\mathrm{SrBr_2}\) in \(750 \mathrm{~mL}\) of \(0.120 \mathrm{M}\) solution. (b) \(0.0112\) moles of \(\mathrm{KCl}\) in \(70.0 \mathrm{~g}\) of \(0.200 \mathrm{~m}\) solution. (c) \(0.0479\) moles of glucose (\(\mathrm{C_6H_{12}O_6}\)) in \(150.0 \mathrm{~g}\) of a solution that is \(5.75\%\) glucose by mass.

Step by step solution

01

Part (a): Calculate moles of SrBr2

To find the number of moles, use the formula: Number of moles = Molarity × Volume (in Liters) Molarity (M) of SrBr2 = 0.120 M Volume (V) of the solution = 750 mL = 0.750 L Number of moles of SrBr2 = 0.120 M × 0.750 L = 0.090 moles
02

Part (b): Calculate moles of KCl

To find the number of moles, use the formula: Number of moles = Molality × Mass of Solvent (in kg) Molality (m) of KCl = 0.200 m Mass of the solvent = 70.0 g - (70.0 g × 0.200) = 56.0 g = 0.056 kg Number of moles of KCl = 0.200 m × 0.056 kg = 0.0112 moles
03

Part (c): Calculate moles of glucose

To find the number of moles, use the formula: Number of moles = Mass of Solute (g) / Molar mass of Solute (g/mol) Molar mass of glucose = 6(12.01) + 12(1.01) + 6(16.00) = 180.18 g/mol Percentage of glucose = 5.75% Total mass of solution = 150.0 g Mass of glucose in the solution = 150.0 g × 0.0575 = 8.625 g Number of moles of glucose = 8.625 g / 180.18 g/mol = 0.0479 moles

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