From the information given below, determine the molality and the molecular weight of the solute; Freezing Point Depression (*C) 5.81 Molality= 3.21 Molecular Weight = 3.21 Van't Hoff Factor 1.00 m X g/mole Solvent Water Mass of Solvent (kg) 0.100 Mass of Solute (g) 10.0

From the information given below, determine the molality and the molecular weight of the solute; Freezing Point Depression (*C) 5.81 Molality= 3.21 Molecular Weight = 3.21 Van't Hoff Factor 1.00 m X g/mole Solvent Water Mass of Solvent (kg) 0.100 Mass of Solute (g) 10.0

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A ‍aluminum sulfide solution at 23∘C has an osmotic pressure of 19 atm and a density of 1.218 g/mL.…

Q: Suppose that the freezing point of a 1.0 m electrolyte solution is normally 10.521 C with a Kb of…

A: Colligative properties are properties of a solution that depend on the number of solute particles…

Q: Aqueous ethanol solutions are prepared by mixing measured weights of assayed ethanol and…

Q: Determine the van't hoff factor of the following solute given the supplementary information provided…

A: Can't Hoff factor depends on the Nature of solute. If solute is non-electrolytic and non- ionizable…

Q: The molality of ethyl alcohol in a solution of water (H2O, MW = 18.02 g/mol) and ethanol (C2H5OH,…

A: Answer:Mole fraction of a compound in a solution is equal to the ratio of its number of moles and…

Q: When 236. mg of a certain molecular compound X are dissolved in 70.0 g of benzonitrile (C6H,CN), the…

A: The mass of compound X = 236 mg = 0.236 gThe mass of benzonitrile = 70.0 gThe freezing point of…

Q: A 0.058 g sample of a unknown substance was dissolved in 2.635 g of benzene, C6H6. The molality of…

A: Given: The given mass of unknown substance, (m1)= 0.058 g. The given mass of benzene, (m2)= 2.635 g.…

Q: The density of an aqueous solution containing 20.0 percent of ethanol by mass is 0.986 g/mL. (a)…

Q: Aqueous ethanol solutions are prepared by mixing measured weights of assayed ethanol and…

A: We have to calculate the molality.

Q: If the mole fraction of C*H_{3} * O * H in a solution with only water is 0.0250, what is the…

Q: An aqueous H2SO4 solution has a mole fraction of H2SO4 = 0.103 and a density of 1.26 g/mL. Calculate…

A: Given: Mole fraction of H2SO4 in aq soln. = 0.103 Density of solution = 1.26 gms/ml

Q: Calculate the freezing point of solution given below. A solution is prepared by condensing 4.00 Lof…

A: Option 1 should be the correct answer (-10.930C)

Q: A student creates an aqueous solution that is 0.200 m K2S. Assuming complete dissociation of the…

A: NOTE: In question, there is a typing error. Instead of molality, molarity is written to be found…

Q: Aqueous ethanol solutions are prepared by mixing measured weights of assayed ethanol and…

A: Molality = moles of solute/weight of solvent Moles of solute =given mass/ molar mass

Q: You have a aqueous solution of NaCl that has a freezing point of -6.55°C. Assuming a van't Hoff…

A: Given that, Freezing point of NaCl solution ∆Tf = -6.55°C Kf of water = 1.86°C.Kg/mol = 1.86°C/m…

Q: determine the van't hoff factor of the following solute given the supplementary information provided…

A: To identify: The van't Hoff factor for the solutes given.

Q: A 1.383 g1.383 g sample contains only vitamin C (C6H8O6)(C6H8O6) and sucralose…

A: Given,mass of a sample containing vitamin C and sucralose = 1.383 gvolume of the solution = 31.1 mL…

Q: Please provide detailed solution give the explanation of correct and incorrect options..

A: We know that there is a lowering of vapor pressure when we add some non-volatile solutes in the…

Q: A student dissolves 8.0 g of stibene (C₁4H12) in 300. ml. of a solvent with a density of 0.81 g/mL..…

Q: Use the following information to calculate the molar mass of the unknown Mass of unknown solute =…

A: The relation between depression in freezing point and molality of a solution is given as follows;…

Q: 3. Ms Lauren R. Davis prepared three aqueous solutions of sucrose (C12H22011) in proportions as…

A: Exp 2molar mass of sucrose=342.3g/molNo. of moles of sucrose=given massmolar…

Q: The boiling point of a solution of 2.056 moles of an electrolyte dissolved in 1399 g of benzene is…

Q: Connected to DESKTOP-VKHKVG3 1.0 m C₂H₁₂O Disconnect X Which one of the following aqueous solutions…

A: Freezing point is the temperature at which a substance start converting from solid to liquid form.

Q: Which of the following statements is true? 11 J2.0 y suviryou up you ww vuððu uwnew, rw rv www…

Q: Calculate the molality and van’t Hoff factor (i) for the fol-lowing aqueous solutions:(a) 0.500 mass…

A: Molality: Molality is defined as the moles of solute in 1 kilogram of solvent. It is given by,…

Q: When 66.8 grams of a solute (molar mass = 56.8 g mol–1) was dissolved in 375.4 grams of water, the…

A: Given data: To (boiling point of water) is 100.0°C. Tb (boiling point of solution) is 105.1°C. Kb of…

Q: Aqueous ethanol solutions are prepared by mixing measured weights of assayed ethanol and…

Q: For a solution to be ideal, which of the following statements is true? A) The solute and solvent…

A: The solutions which obey Raoult's law at all temperatures and pressures are called ideal solutions.

Q: Aqueous ethanol solutions are prepared by mixing measured weights of assayed ethanol and…

A: Given that - Mass percentage of ethanol = 18.5% , which means that Solution contains 18.5 gram of…

Q: I have to figure out van't Hoff factor from the following information. I tried 1.0 and 2.0 but it…

A: The depression in the freezing of a solvent when a non volatile solute is added is expressed as…

Q: A solution with 1.0 mol C2H5OH in 100g of solvent has the same molality as a solution with 1.0 mol…

Q: What is the molality of a4.60%v/vsolution of isopropanol. The density of water is0.9978 g/mLand the…

A: To calculate the molality of the solution, we need to first determine the moles of isopropanol in 1…

Q: Calculate the boiling temperature of the following solution of 0.50 M glucose (a covalent compound).…

A: Given that, Molality of Glucose solution = 0.50 m Von't Hoff factor for Glucose = 1 (non…

Q: 20.3 g of Urca NHCONH2 was dissolved in 100 g of water. The volume of the resulting solution is…

A: Part d is mass percent of NaOH but NaOH is not used in the formation of solution. So i have…

Q: Aqueous ethanol solutions are prepared by mixing measured weights of assayed ethanol and…

A: Given that : % mass of ethanol in the aqueous solution = 26.8 % Atomic mass of C = 12.01 g/mol…

Q: A solution of 0.870 g of an organic compound in 100.0 g of benzene has a freezing point of 5.227°C.…

A: From given data Kf = 5.12°C/m Freezing point of solution T1 = 5.227 °C Freezing point of pure…

Q: 6. Calculate the molality of each of the following solutions: (a) 14.3 g of sucrose (C12H22011) in…

A: Calculate the molality of each of the following solutions: (a) 14.3 g of sucrose (C12H22O11) in…

Q: To make a solution, 40 g of a nonelectrolyte is dissolved into 300 g of water. The freezing point…

A: The depression in freezing point of solution is given as, ΔTf = Kf m Where,m is the molality of…

Q: The solvent carbon disulfide has a melting point of -111.5 deg C, and a freezing point depression…

A: Given: The melting (freezing point) point of carbon disulfide = -111.5 deg C. The freezing point…

Q: A nonvolatile solute is dissolved in benzene so that it has a mole fraction of 0.147. What is the…

Q: A 0.5 M NaOH solution has a density of 1.0295 g/mL. Calculate the w% and the molality of the 0.5 M…

A: 0.5M NaOH solution means 0.5 moles NaOH is present in 1000mL solution weight of solute NaOH =…

Q: What is the mole fraction, X, of solute and the molality, m (or b), for an aqueous solution th 17.0%…

A: The mole fraction of a component in the mixture is defined by the ratio of moles of that substance…

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

From the information given below, determine the molality and the molecular weight of the
solute;
Freezing Point
Depression (*C)
5.81
Molality=
3.21
Molecular Weight =
3.21
Van't Hoff
Factor
1.00
m
X g/mole
Solvent
Water
Mass of
Solvent (kg)
0.100
Mass of
Solute (g)
10.0

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: Introduction to given problem

VIEW

Step 2: Calculation of molality

VIEW

Step 3: Calculation of molecular mass

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 3 images

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

Boiling Point ElevationThe boiling point of a solution INCREASES with the number of dissolved solute particles. This is summarized by the expression: Tb = m i KbWhere: Tb is the increase in the boiling point = Tb(solution) - Tb(pure solvent) m is the molality of the solution = (# moles solute / kg solvent) i is the "van't Hoff" factor = (# moles of solute particles / mole of solute) For nonelectrolytes: i = 1 For strong electrolytes: i = number of (cations + anions) For weak electrolytes: 1 < i < number of (cations + anions) Kb is the boiling point elevation constant. It depends only on the SOLVENT. Example:Na2SO4 is a soluble salt. It breaks into two Na+ cations and one SO42- anion in solution.i = 2 + 1 = 3 CH3COOH is a weak acid. It breaks into a few CH3COO - anions and a few H+ cations. 1 < i < 2.
Calculate the molality of the solution given that the boiling point of the solution is 25℃, the normal boiling point of the solvent is 40℃, the Kb is 2.53℃/ m and the solute is KNO3.
please put complete solution
Aqueous ethanol solutions are prepared by mixing measured weights of assayed ethanol and organic-free water. What is the molality of an aqueous solution that is 22.2 % ethanol, C2H5OH , by mass? Atomic Mass: C=12.01 ; H=1.008 ; O = 16.0
We have a 1.000 M aqueous solution of C3H8O(aq) (C3H8O is the only solute). Thedensity of this solution is 0.988 g/mL. Calculate the molality, the percent mass, and themole fraction of C3H8O in this aqueous solution. The molar masses of C, O, and H are12.01, 16.00, and 1.01 g/mol
Complete the freezing point depression table below: Mass / Volume added Added reagent Molecular Weight van't Hoff Factor molality Freezing Point 20.0 g NaCl 25.0 g Li2SO4 10.0 mL 0.150 M ethanol Kf (°C/m) of water: 1.86 Freezing Point of Water, °C: 0.0 SOLVENT: 100 g water
6. What volume of conc. HCl (density 1.19g/cm3, 38% HCl by weight) is required to make up 18L of 0.50N HCl. 7. Sulfuric acid, H2SO4 has a density of 1.198g/cm3 containing 27.0% by weight. Calculate the molar and molal concentration
Aqueous ethanol solutions are prepared by mixing measured weights of assayed ethanol and organic-free water. What is the molality of an aqueous solution that is 45.1 % ethanol, C2H5OH , by mass? Atomic Mass: C=12.01 ; H=1.008 ; O= 16.0 Express your answer in two decimal places. Do not write the unit.
A compound is found to have a molar mass of 598 g mol-¹. If 36.1 mg of the compound is dissolved in enough water to make 174 mL of solution at 25 °C, what is the osmotic pressure of the resulting solution (in units of mbar). Report your answer to 1 decimal place. (R = 0.08314 bar L mol-¹ K-¹)
True or False1.) The phase diagram of a pure solvent shows a lower freezing point compared to solutions2.) The process of freezing only lowers the kinetic energy of solute particles in a solution3.) Ionic solutes have higher van't hoff factor compared to non ionic solutes4.) The formation of intermolecular forces of attraction requires complete dissolution
Osmotic pressure data for a solution containing an unknown sugar are given below. Determine the molar mass of the sugar. T (atm) 2.59 5.06 7.61 12.75 18.13 23.72 density (g/L) 33.5 65.7 96.5 155 209 259
5-please see attached