Chapter 13: Problem 119
A mixture of
Short Answer
Expert verified
The mass percent of in the mixture is approximately 22.3%.
Step by step solution
01
Write down the given information
The total mass of the mixture is 10.2 g. The osmotic pressure is 7.32 atm. The volume of the solution is 250 mL (or 0.250 L). The temperature is , converted to Kelvin as .
02
Recall the formula for osmotic pressure
The osmotic pressure formula is given by , where is the van't Hoff factor, is molarity, is the ideal gas constant (0.0821 L·atm/mol·K), and is temperature in Kelvin.
03
Relate osmotic pressure to molarity
Convert the osmotic pressure formula to solve for molarity: . For , (since it dissociates into and ), and for sucrose, .
04
Calculate the total molarity for the mixture
Using , , and , calculate : Let . You need the total for both components.
05
Use the mass and moles relationship
Write the expressions for the number of moles: and , where and are masses of and sucrose respectively. From the problem statement: .
06
Setup and solve the system of equations
Using the relations: and , solve these two equations simultaneously to find .
07
Calculate the mass percent of NaCl
Once you have the mass , calculate the mass percent:
08
Verify your result
Ensure your calculated masses satisfy both the initial mass constraint and the osmotic pressure-derived moles constraint.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Van't Hoff Factor
The Van't Hoff factor, denoted by , is a key concept used in calculating colligative properties, such as osmotic pressure. This factor is crucial as it accounts for the effect of solute particles that are produced when a compound is dissolved in a solution.
For non-ionic compounds like sucrose, the Van't Hoff factor is typically 1, because sucrose stays intact and does not dissociate into multiple particles. This implies that each molecule of sucrose contributes a single particle to the solution's effect. Conversely, for ionic compounds like , . Upon dissolving, dissociates into two ions: and .
To calculate osmotic pressure, is multiplied by the molarity , the ideal gas constant , and the temperature in Kelvin . Therefore, understanding and calculating the Van't Hoff Factor is necessary to predict the behavior of a solution, especially when dealing with mixtures of ionic and non-ionic substances.
For non-ionic compounds like sucrose, the Van't Hoff factor is typically 1, because sucrose stays intact and does not dissociate into multiple particles. This implies that each molecule of sucrose contributes a single particle to the solution's effect. Conversely, for ionic compounds like
To calculate osmotic pressure,
Molarity Calculation
Molarity, represented as , is a measure of concentration, indicating the amount of solute present in a given volume of solution. It is calculated in terms of moles of solute per liter of solution.
In the context of osmotic pressure, molarity is integrated into the equation , where is the osmotic pressure. Rearrange this equation to solve for molarity: . This way, you can identify how much solute is dissolved in the solution based on the observed osmotic pressure and the conditions given, like temperature.
When calculating molarity for a mixture, as in the case of and sucrose, you need the combined effect of all solutes. Each contributes to the total molarity based on their respective Van't Hoff factors and the amount present in the solution. This approach clarifies how a mixture's overall concentration impacts properties like the osmotic pressure.
In the context of osmotic pressure, molarity is integrated into the equation
When calculating molarity for a mixture, as in the case of
Ideal Gas Constant
The ideal gas constant, , is a central figure in the world of chemistry, especially in calculations involving gases and solutions. In the context of osmotic pressure, is used in the formula to relate pressure, solubility, and temperature.
Constant typically takes the value when calculations are done using the units of pressure in atmospheres and volume in liters. While derived from the ideal gas law , its application extends to numerous other states of matter, including solutions.
By drawing a connection between the gas laws and colligative properties of solutions, the ideal gas constant helps in calculating how solute particles contribute to osmotic pressure in a solution. Given its universal application, understanding is essential for assessing how changes in temperature or volume affect the concentration and pressure in any system.
Constant
By drawing a connection between the gas laws and colligative properties of solutions, the ideal gas constant helps in calculating how solute particles contribute to osmotic pressure in a solution. Given its universal application, understanding