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A(n) _____ is an unstable physical mixture of undissolved particles in a liquid.
6. Chemical Quantities & Aqueous Reactions
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What is the molarity of methanol in the solution prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25°C, given that the final volume of the solution is 118 mL and the density of methanol is 0.782 g/mL?
A
0.134 M
B
0.172 M
C
0.156 M
D
0.198 M
Verified step by step guidance1
Calculate the mass of methanol using its volume and density. Use the formula: mass = volume × density. Here, the volume of methanol is 20.2 mL and the density is 0.782 g/mL.
Convert the mass of methanol to moles. Use the molar mass of methanol (CH3OH), which is approximately 32.04 g/mol. Use the formula: moles = mass / molar mass.
Determine the total volume of the solution in liters. The final volume of the solution is given as 118 mL. Convert this volume to liters by dividing by 1000.
Calculate the molarity of the methanol solution. Molarity (M) is defined as the number of moles of solute (methanol) divided by the volume of the solution in liters. Use the formula: Molarity = moles of solute / liters of solution.
Compare the calculated molarity with the given options to identify the correct answer.
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