Textbook Question
Nalorphine 1C19H21NO3 2, a relative of morphine, is used to combat withdrawal symptoms in narcotics users. How many grams of a 1.3 * 10-3 m aqueous solution of nalor-phine are needed to obtain a dose of 1.5 mg?
Ch.13 - Solutions & Their Properties
Chapter 13, Problem 78b
A 0.944 M solution of glucose, C6H12O6, in water has a density of 1.0624 g/mL at 20 °C. What is the concentration of this solution in the following units? (b) Mass percent
Verified step by step guidance1
Step 1: Understand the concept of mass percent. Mass percent is a way of expressing the concentration of a solution, defined as the mass of the solute divided by the total mass of the solution, multiplied by 100%. The formula is: .
Step 2: Calculate the mass of glucose in 1 liter of solution. Use the molarity of the solution, which is 0.944 M, meaning there are 0.944 moles of glucose per liter of solution. Find the molar mass of glucose, C6H12O6, by adding the atomic masses of its constituent atoms: . Multiply the molar mass by the number of moles to find the mass of glucose.
Step 3: Calculate the total mass of the solution. Use the density of the solution, which is 1.0624 g/mL, to find the mass of 1 liter (1000 mL) of solution. Multiply the density by the volume: .
Step 4: Substitute the values into the mass percent formula. Use the mass of glucose calculated in Step 2 and the total mass of the solution from Step 3. Plug these values into the mass percent formula: .
Step 5: Interpret the result. The mass percent will give you the concentration of glucose in the solution as a percentage, indicating how much of the solution's mass is due to glucose.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molarity
Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is commonly used in chemistry to express the concentration of a solution. In this case, the 0.944 M solution of glucose indicates that there are 0.944 moles of glucose dissolved in every liter of the solution.
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Molarity
Mass Percent
Mass percent is a way to express the concentration of a component in a mixture, calculated as the mass of the solute divided by the total mass of the solution, multiplied by 100. This unit is useful for understanding the composition of solutions in terms of mass rather than volume, which can be important for reactions and properties that depend on mass.
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Density
Density is defined as mass per unit volume and is an important property of substances. In this context, the density of the glucose solution (1.0624 g/mL) allows us to convert between volume and mass, which is essential for calculating mass percent. Knowing the density helps determine the total mass of the solution when the volume is known.
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Related Practice
Textbook Question
A 0.944 M solution of glucose, C6H12O6, in water has a density of 1.0624 g/mL at 20 °C. What is the concentration of this solution in the following units? (a) Mole fraction
Textbook Question
A 0.944 M solution of glucose, C6H12O6, in water has a density of 1.0624 g/mL at 20 °C. What is the concentration of this solution in the following units? (c) Molality
Textbook Question
Lactose, C12H22O11, is a naturally occurring sugar found in mammalian milk. A 0.335 M solution of lactose in water has a density of 1.0432 g/L at 20 °C. What is the concentra- tion of this solution in the following units?(b) Mass percent
Textbook Question
Look at the solubility graph in Figure 13.7, and estimate which member of each of the following pairs has the higher molar solubility at the given temperature.(b) CH3CO2Na or glucose at 20 °C