Explanation Given: Density (solution) = 1 .063 g/mL Molarity = 0 .438 M Vapor pressure of pure water , P H 2 O ° = 0 .0313 atm (at 298 K) To assume: K 2 C r O 4 dissociates completely. Explanation: (1) Molarity of a solution is the number of moles of solute per liter of the solvent. Therefore, the number of moles of K 2 C r O 4 dissolved in 1000 mL solution is equal to the molarity of this solution. n K 2 CrO 4 = 0 .438 mol (2) Calculate the mass of K 2 C r O 4 in the solution as follows: m K 2 CrO 4 = n K 2 CrO 4 × Molar mass (K 2 CrO 4 ) = 0.438 mol × 194.1896 g/mol = 85 .055 g (3) Density ( d ) is defined as mass per unit volume. d = m / V Here, m is the mass of the solution and V is the volume of the solution. Rearrange this equation to calculate the mass of the solution: m = V × d (1) Calculate the mass of the solution by substituting the values in equation (1) as follows: m s o l u t i o n = V × d = 1000 m L × 1.063 g/mL = 1063 g (4) Calculate the mass of water in the solution as follows: m H 2 O = m s o l u t i o n − m K 2 C r O 4 = 1063 g − 85 .055 g = 977 .945 g (5) Calculate the number of moles of water in the solution as follows: n H 2 O = m H 2 O Molar mass (H 2 O) = 977

Chemistry: A Molecular Approach (4th Edition)

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Chapter 13, Problem 116E

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To determine: Pressure of water vapors above the given solution of K2CrO4 at 298 K.

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Chapter 13, Problem 115E

Chapter 13, Problem 117E

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Chapter 13 Solutions

Chemistry: A Molecular Approach (4th Edition)

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Pressure of water vapors above the given solution of K 2 C r O 4 at 298 K .

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Chapter 13 Solutions