If a solution containing 4.30 g triphenylmethane (C6H5)3CH, in 800 g of benzene is cooled to 0.321 °C below the freezing point of pure benzene a) how much solvent will crystallize out and b) what will be the molality of the residual solution?

If a solution containing 4.30 g triphenylmethane (C6H5)3CH, in 800 g of benzene is cooled to 0.321 °C below the freezing point of pure benzene a) how much solvent will crystallize out and b) what will be the molality of the residual solution?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.17QE

See similar textbooks

Related questions

Q: a. Eutexia b. The Phase Rule c. Polymorphism d. Degrees of Freedom Useful device for relating the…

A: According to Q&A guidelines of Bartleby, we are supposed to answer only the first 3 rows of…

Q: 1. Calculate the boiling point of a solution containing 12g glucose C6H12O6 dissolved in 200g of…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A dilute solution of liquid X in liquid Y is prepared. It is found that the partial molar volume of…

A: A question based on physical chemistry, which is to be accomplished.

Q: The solubility of KNO3 (MW=101.1 g/mole) in water at 65° C is 12.4 molal and at 0° it is only 1.2…

A: Given information, Molar mass of KNO3 = 101.1 g/mol Solubility of KNO3 at 65°C = 12.4 molal…

Q: 10 g of a solute was dissolved in 80 g of acetone at 30°C. The vapour pressure was found to be 271…

A: When a non-volatile solute is added, the vapour pressure of solvent decreases. This could be calc

Q: The solution prepared by dissolving 6.06 g of triphenyl methane [(C,H5)CH] in 1000 g of benzene,…

A: Given : Mass of solute i.e triphenyl methane = 6.06 g Mass of solvent i.e Benzene = 1000 g = 1 Kg…

Q: A student determines the molar mass of acetone, , She found that the equilibrium temperature of a…

A: a. The depression in freezing point has the formula = initial temperature - final…

Q: A solid mixture made up of 75% of solid A and 25% of solid B by mass is to be dissolved in 250.0 ±…

A: Given: % of Solid A = 75% % of Solid B = 25 % Volume of water = 250.0 ± 0.5 mL Molality of solution…

Q: Calculate the mole fractions of methanol, CH3OH; ethanol, C2H5OH; and water in a solution that is…

Q: The experimental data in the table was collected during a freezing point depression study where BHT…

A: When a non-volatile solute is dissolved is dissolved in a volatile solvent, the freezing point of…

Q: Describe the ideal condition/set-up for recrystallization of substances. What are the factors to…

A: A question about re-crystallization, which is to be accomplished.

Q: The following data shows the dissolved concentration of a gas in water as the partial pressure above…

A: Henry's law states that concentration of dissolved gas is directly proportional to the partial…

Q: 0.0471 kg of biphenyl (C12H10) is dissolve in benzene (CoH6) to create a solution with a total…

A: Answer: This question is based on Raoult's law according to which, after adding the non-volatile…

Q: Draw Vapour pressure vs composition (in terms of mole fraction) diagram for an ideal solution.

A: Draw Vapour pressure vs composition (in terms of mole fraction) diagram for an ideal solution.

Q: Test Tube Solute Mass of Deionized Water (g) Mass of solute (g) Freezing Point (C) 1 None 4.140g X…

A: The data given is, Test Tube Solute Mass of Deionized Water (g) Mass of solute (g) Freezing Point…

Q: Calculate the molality of a solution that contains 82 g of naphthalene, C10H8, in 673 mL of carbon…

A: The molality of a solution is defined as the no of moles of solute present in 1kg of the solvent.…

Q: You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The…

A: The depression in freezing point is given by depression in freezing point = i X Kf X m where i =…

Q: A solution is made by mixing 23.0 grams pentane (C5H12), 12.0 grams octane (CgH1g), and 17.0 grams…

A: Given :- mass of pentane = 23.0 g mass of octane = 12.0 g mass of toluene = 17.0 g To calculate :-…

Q: The solution prepared by dissolving 6.06 g of triphenyl methane [(C6H5)CH] in 1000 g of benzene,…

Q: 10 g of a solute was dissolved in 80 g of acetone at 30°C. The vapour pressure was found to be 271…

Q: The solubility is 12.8g in 100mL of ethanol at 0 degrees C, and 46.4 g in 100mL of ethanol at 60…

A: Given, the solubility is 12.8g in 100mL of ethanol at 0 degrees C and 46.4 g in 100mL of ethanol at…

Q: Based on the concept of distribution coefficient, a solute that is soluble with two immiscible…

A: Partition coefficient (P) or distribution coefficient (D) is the ratio of concentrations of a…

Q: The solubility of a compound with a molecular weight of 242.7 is determined to be 26.0 g in 75.0 g…

A: The number of moles of the solute and solvent (water) can be calculated as shown below.

Q: Compound Molality Weight Percent Mole Fraction KNO3 10.0 CH3CO2H 0.0183…

Q: At 20°C the vapour pressure of benzene (C6H6) is 76.0 mm Hg, and that of toluene (C7H8) is 21.8 mm…

A: Since you have posted multiple unrelated questions, we are entitled to answer the first only. Given:…

Q: Calculate the normal freezing point of a 0.7439 mol aqueous solution of c12h22o11 that has density…

A: Given data: Moles of aqueous solution of C12H22O11 = 0.7439 mol Density = 1.35 g/mL Molal freezing…

Q: Explain why freezing point depression is observed when a non-volatile solute is dissolved in a…

A: Solution Freezing point of depression may be a colligative property of resolution. it's discovered…

Q: With this in mind, lets calculate the amount of depression that will occur when 5 g of sodium…

Q: Determine the molar fraction of fenal C6H5OH and the molality in a solution prepared with 18.3g of…

Q: Abuela asked Mirabel to perform an experiment on freezing point depression. The solution was…

A: In part 3., mass of potassium nitrate is taken as mass of potassium chloride since it was mentioned…

Q: Answer the following problem completely and systematically. Show your complete solution. As you may…

A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: Explain how a solution of two volatile components with strong solute-solvent attractions deviates…

A: Solution is made up of two components: solute and solvent. Component with major amount is called…

Q: You create an aqueous solution containing an unknown solute. Measuring the osmotic pressure, you…

A: C. Ebullioscopic constant for water From the osmotic pressure we can calculate the molality of the…

Q: Would freezing point depression be different for a volatile solute than for a nonvolatile solute?…

A: The freezing point(fp) of a solution is less than the freezing point of the pure solvent.That is a…

Q: The freezing point depression equation tends to be used for nonvolatile solutes. Offer an…

A: Volatile means that solute which will evaporate aur change its state. Non volatile solute is which…

Q: How is vapour pressure of solvent affected when a non-volatile solute is dissolved in it?

A: Over the surface of a liquid the pressure exerted by the vapors of a liquid at a certain temperature…

Q: Calculate the average partial molar volume (in cm³/mol) of MgSO4 in the interval [0.1, 0.2] mol of…

Q: State raoult's law for a non volatile solute in single volatile solvent?

A: The vapour pressure of a solution of a non-volatile solute is equal to the vapour pressure of the…

Q: A solution is prepared by dissolving 10 g of non-volatile solute in 200 g of water. It has a vapour…

A: Decrease in the vapor pressure of solution by addition of a nonvolatile solute is known as vapor…

Q: The partial molar volume of water in a 1.000 molal sodium chloride/water solution at 25°C is 18.042…

A: Given data: The partial molar volume of water = 18.042 cm3/mol. The molality of sodium…

Q: initial mole fraction

A: Molar mass of NaCl=58.44 Molar mass of water=18g Mole fraction of each solute = Number of moles of…

Q: Why is the freezing point of a pure solvent constant, while that a solution decrease with steady…

A: The depression is a colligative property in the freezing point of a solution i.e. it depends upon…

Q: When 1 mol of a nonvolatile, nondissociating solute is dissolve 3 mol of volatile solvent, the ratio…

Q: 1. Calculate the boiling point of a solution containing 12g glucose C6H12O6 dissolved in 200g of…

A: Note :

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

If a solution containing 4.30 g triphenylmethane (C6H5)3CH, in 800 g of benzene is cooled to
0.321 °C below the freezing point of pure benzene a) how much solvent will crystallize out and
b) what will be the molality of the residual solution?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The freezing point of this solution is found to be 0.426C. Assuming ideal behavior, calculate the mass percent composition of the original mixture, and the mole fraction of sucrose in the original mixture.
Create a flow diagram, similar to those used in the example problems of this chapter, that outlines the determination of the molar mass of a compound from freezing-point depression measurements. Clearly indicate the data needed for this determination.
A gaseous solute dissolves in water. The solution process has H=15 kJ. Its solubility at 22C and 6.00 atm is 0.0300 M. Would you expect the solubility to be greater or less at (a) 22C and 1 atm? (a) 18C and 6 atm? (a) 15C and 10 atm? (a) 35C and 3 atm?
You dissolve 1.0 mol of urea (H2NCONH2) in 270 g of water. The mole fraction of urea is (a) 3710 3 (b) 0.063 (c) 16 (d) 1.0 and its molality is (a) 1.0 (b) 3.7 (c) 0.063 (d) 0.27
The solubility of ethylene (C2H4) in water at 20 C and 0.300 atm pressure is 1.27 104 molal. (a) Calculate the Henrys law constant for this gas in units of molal/torr. (b) How many grams of ethylene are dissolved in 1.00 kg water at 20 C if the pressure of the gas is 500 torr?
A 2.77 M NaOH solution in water has a density of 1.109 g/mL. Express the concentration of this solution (a) mass percentage. (b) mole fraction. (c) molality.