Answers:
a. 1.28 mol/L; b. 17.0 %; c. 0.0227; d. 1.29 mol/kg
Explanation:
a. Molar concentration
c = moles/litres
Moles = 167 × 1/159.61 Do the calculation
Moles = 1.046 mol
Litres = 820 × 1/1000 Do the calculation
Litres = 0.8200 L Calculate the molar concentration
c = 1.046/0.8200 Do the division
c = 1.28 mol·L⁻¹
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b. Percent by mass
Mass % = mass of solute /mass of solution × 100 %
Mass of solution = volume × density Insert the values
Mass of solution = 820 × 1.195 Do the multiplication
Mass of solution = 979.9 g Calculate the mass %
Mass % = 167/979.9 × 100 Do the operations
Mass % = 17.0 %
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c. Mole fraction
χ = moles of solute/(moles of solvent + moles of solute)
Mass of solvent = mass of solution – mass of solute
Mass of solvent = 979.9 – 167 Do the subtraction
Mass of solvent = 812.9 g Convert to moles
Moles of water = 812.9 × 1/18.02 Do the calculation
Moles of water = 45.11 mol Calculate the total moles
Total moles = 1.046 + 45.11 Do the addition
Total moles = 46.16 mol Calculate the mole fraction
χ = 1.046/46.16 Do the division
χ = 0.0227
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d. Molal concentration
b = moles of solute/kilograms of solvent
Mass of solvent = 812.9 g = 0.8129 kg Calculate the molal concentration
b = 1.046/0.8129 Do the division
b = 1.29 mol/kg
From the calculations, the final molality of the solution is 1.06 m.
Mass of the solvent can be obtained from;
Mass = density × volume
Mass = 1.195 g/mL × 820 mL =979.9 g
a) molarity of the solution = number of moles of solute/volume of solution
= 167 g/160 g/mol × 1000/820 = 1.27 M
b) percent by mass of the solute = 167 g/(167 g + 979.9 g) ×100/1
= 14.6%
c) Number of moles of water = 979.9 g/18 g/mol = 54 .4 moles
mole fraction = 1.04 moles/(1.04 moles + 54 .4 moles)
= 0.019
d) molality of the solution = number of moles of solute/mass of solvent in Kg
= 1.04 moles/979.9 ×10^-3 Kg
= 1.06 m
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