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The density of 10% by mass of KCl soluti...

The density of 10% by mass of KCl solution in water is 1.06 g `mL^(-1)`. Calculate molarity and molality of the solution.

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To calculate the molarity and molality of a 10% by mass KCl solution with a density of 1.06 g/mL, we can follow these steps: ### Step 1: Understand the Given Data - Mass percentage of KCl solution = 10% - Density of the solution = 1.06 g/mL ### Step 2: Calculate the Mass of the Solution Assume we have 100 g of the solution (since the mass percentage is based on 100 g). - Mass of KCl (solute) = 10% of 100 g = 10 g - Mass of water (solvent) = 100 g - 10 g = 90 g ### Step 3: Calculate the Number of Moles of KCl To find the number of moles of KCl, we need its molar mass. - Molar mass of KCl = Atomic mass of K (39 g/mol) + Atomic mass of Cl (35 g/mol) = 74 g/mol - Number of moles of KCl (n) = Mass of KCl / Molar mass of KCl = 10 g / 74 g/mol ≈ 0.1351 mol ### Step 4: Calculate the Mass of the Solvent in kg - Mass of water = 90 g = 90 g / 1000 = 0.090 kg ### Step 5: Calculate Molality (m) Molality (m) is defined as the number of moles of solute per kilogram of solvent. - Molality (m) = Number of moles of solute / Mass of solvent in kg = 0.1351 mol / 0.090 kg ≈ 1.50 mol/kg ### Step 6: Calculate the Volume of the Solution To find the volume of the solution, we can use the density formula: - Density = Mass / Volume - Volume = Mass / Density = 100 g / 1.06 g/mL ≈ 94.34 mL = 0.09434 L ### Step 7: Calculate Molarity (M) Molarity (M) is defined as the number of moles of solute per liter of solution. - Molarity (M) = Number of moles of solute / Volume of solution in L = 0.1351 mol / 0.09434 L ≈ 1.43 mol/L ### Final Results - Molality of the solution ≈ 1.50 mol/kg - Molarity of the solution ≈ 1.43 mol/L ---

To calculate the molarity and molality of a 10% by mass KCl solution with a density of 1.06 g/mL, we can follow these steps: ### Step 1: Understand the Given Data - Mass percentage of KCl solution = 10% - Density of the solution = 1.06 g/mL ### Step 2: Calculate the Mass of the Solution Assume we have 100 g of the solution (since the mass percentage is based on 100 g). ...
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