The freezing point of pure water is 0°C and its molal freezing point depression constant (Kf) is 1.86°C/m. a. What is the change in the freezing point (∆Tf) of a solution that contains 53 grams of sucrose (MW= 342.3 g/mol) dissolved in 1000 grams of water.

The freezing point of pure water is 0°C and its molal freezing point depression constant (Kf) is 1.86°C/m. a. What is the change in the freezing point (∆Tf) of a solution that contains 53 grams of sucrose (MW= 342.3 g/mol) dissolved in 1000 grams of water.

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: When 14.0 g of a certain molecular compound X are dissolved in 85. g of benzene (CH), the freezing…

Q: Using this equation, find the new freezing point for each of the following solutions. For water, .…

A: a. 3.85 mol NaCl in 4.50 kg of water b. 2.00 g K3PO4 in 1.00 kg of water c. 150.0 g of sugar (molar…

Q: A certain liquid X has a normal freezing point of -3.00 °C and a freezing point depression constant…

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

Q: For a general chemistry 2 lab, an aqueous solution of a soluble compound (a nonelectrolyte) is…

A: 34.7 g of a compound is dissolved in sufficient water to form 0.267 L of solution. The solution…

Q: Calculate the freezing point of a solution containing 0.135 mol of a nonionic solute in 2.50 kg of…

A: When a non volatile solute is added to pure solvent then its freezing point decreases If Tf° is…

Q: A solution made by dissolving 150.0 g of an unknown compound in 330.0 mL of benzene to make a…

A: The properties of solution that depend only on the concentration of the solute and is independent of…

Q: When 0.279 g of a molecular compound, benzoic acid, was dissolved in 43.0 g of benzene, the freezing…

A: Depression in freezing point :- When a nonvolatile solute is added to pure solvent then its…

Q: 10 A 3.40-g sample of a mixture of naphthalene (C, H.) and pyrene (CH) is dissolved in 35.0 g…

A: Given: The mass of the mixture of naphthalene and pyrene = 3.40 g The mass of benzene (solvent) =…

Q: 1. The solubility of L-glutamic acid (an amino acid) in water has been determined to be as follows…

A: Solubility: When the maximum amount of solute is dissolve in the solvent is called solubility. On…

Q: Chemistry When 248. mg of a certain molecular compound X are dissolved in 65.0 g of benzene (CH),…

Q: solution

A: We will calculate Tf

Q: When 541. mg of a certain molecular compound X are dissolved in 75. g of dibenzyl ether…

A: Here we are required to find the molar mass

Q: When you open a bottle of a carbonated beverage, bubbles of carbon dioxide gas escape from the…

A: Henry’s Law:Henry's Law explains the solubility of gas in a liquid solution. It states that the…

Q: please calculate only freezing point

Q: 7. Camphor (C10H160) freezes at 179.8°C, and it has a particularly large freezing point depression…

A: The expression for freezing point depression is given by, Tf-Ti=Kf.m where Kf is the freezing point…

Q: 100 90 NaNO 80 70 60 CaCl 50 Pb(NO)2 40 NaCl KCI 30 20 KCIO, 10 Ce,(SO 10 20 30 40 50 60 70 80 90…

A: When the amount of solute is dissolved in a solvent to make a homogenous mixture are known as…

Q: A certain substance X has a normal freezing point of 0.5 °C and a molal freezing point depression…

A: mass of urea = 21.87 gmolar mass of (NH2)2CO = 60.06 g/molKf = 4.05oC kg/molT(solvent) = 0.5oCi = 1…

Q: The boiling point of benzene, CaHe, is 80.10 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that…

Q: - 1 The molal freezing point depression constant K₁=2.02 °C-kg-mol for a certain substance X. When…

Q: When 0.357 g of an unknown compound was dissolved in 60.0 g of benzene (MM: 78.11g/mol), the…

Q: A student made a solution by mixing 28.20 g of an unknown substance with 500.0 g of benzene (C6H63,…

A: Depression in freezing point (∆Tf) solvent will calculated as:-∆Tf= kf×W2W1×M2Where∆Tf=Depression in…

Q: 3. In a dilute aqueous solution of an unknown solute, MC1× (the anion is Cl¯, but the cation is…

Q: 15. What is the freezing point for an aqueous solution of KBr that was made from dissolving 25.0…

Q: Select the solute that will cause the largest freezing-point depression when dissolved in water. a.…

A: The depression in the freezing point is caused when a non-volatile solute is added to the solution.…

Q: [References] If we add 178 g of ethylene glycol, C,H,O2, per 1000. g of water to a car radiator,…

A: Depression in freezing point is a colligative property

Q: A certain liquid X has a normal freezing point of -4.00 °C and a freezing point depression constant…

Q: A 3.40-g sample of a mixture of naphthalene (C₁₀H₈) and pyrene (C₁₆H₁₀) is dissolved in 35.0 g…

A: Assuming mass of naphthalene in the mixture is y. Hence mass of pyrene = mass of mixture - mass of…

Q: When 225. g of alanine (C,H,NO₂) a are dissolved in 1100. g of a certain mystery liquid X, the…

A: Answer: When a non-volatile solute is dissolved in a solvent then its freezing point decreases which…

Q: When 571. mg of a certain molecular compound X are dissolved in 60.0 g of benzene (CH), the freezing…

Q: A student dissolves 14. g of stilbene (CH12) in 450. mL of a solvent with a density of 1.09 g/mL.…

A: Molarity: The mole of the solute dissolved in one liter of the solution is known as the molarity of…

Q: When 361. g of urea (CH₂N₂O) are dissolved in 1350. g of a certain mystery liquid X, the freezing…

A: According to Raoult's law, the depression in the freezing point of a solution:Here, i = van't Hoff…

Q: 1. A 0.735 g of a covalent organic compound is dissolved in 15.00 g cyclohexane (freezing point =…

A: The depression in freezing point is given by, ΔTf = mKf…

Q: After the addition of 24 g of ethanol (CH;OH) to 1 kg of water, the freezing point of the solution…

A: ∆Tf = Kf .m Where ∆Tf = (T° - Ts) Where T° =freezing point of pure water = 273 K Ts =freezing…

Q: Calculate the van't Hoff factor for iron(III) chloride

A: Since, nitrobenzene C2H5NO2 is non electrolyte it will be having vantoff factor 1 Now Since mass…

Q: What is the freezing point of this solution? (The freezing point of 1 kg of water is lowered 1.86…

A: Colligative properties are dependent on the number of moles of solute in the solution. There are…

Q: 1-A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C.…

Q: Which of the following phenomena is best described by Henry’s Law? a. Increasing temperature favors…

A: Henry's law is exclusively for gases, it is used to study the solubility of gasesIt states that at…

Q: 16. Determine the cahnge in boiling point for 397.7 g of carbon disulfide (Kb= 2.34 degrees Celsius…

A: We have to calculate the change in boiling point.

Q: A solution is made by dissolving 7.80 grams of MgCl2 in 420.0 mL of water. What is the freezing…

A: Given: The mass of solute, (MgCl2)= 7.80 g The molar mass of MgCl2=95.2 g/mol The volume of the…

Q: When 225. g of urea (CH,N,0) are dissolved in 1200. g of a certain mystery liquid x, the freezing…

Q: You make a solution composed of 156.8 g of acetic acid and 18.7 g of a mystery solute. If the…

Q: The solubility of PbCrO4 in water at 25 °C is measured to be 1.7 × 10° Round your answer to 2…

A: Given, solubility = 1.7 x 10-4 g/LTo calculate the solubility product we need to calculate the molar…

Q: A pharmacist mixes together 20g of crystals of compound A and 10g of crystals of compound B. The…

A: The prominent size of crystals is 0.1-0.4 mm. To dissolve the crystals, the solution must be heated…

Q: The normal freezing point of a certain liquid X is 0.60°C, but when 0.14 kg of barium hydroxide…

A: Given : Mass of barium hydroxide, Ba(OH)2 i.e solute = 0.14 Kg = 140 g (since 1 Kg = 1000 g)…

Q: The dispersed phase of a certain colloidal dispersion consistes of spheres of diameter 1.0 x 102 nm.…

A: The diameter of colloidal sphere (d) = 1.0 ×102 nm.…

Q: Use the solubility curve below to determine how much NANO3 can dissolve in 300 g of water at 10…

A: The given graph is plotted between solubility and temperature. This shows the dependence of…

Q: What is the molar mass (in g/mol) of the unknown compound?

Q: A 2.50 g sample of naphthalene, C₁0H8, was dissolved in 100 g of benzene. What is the freezing point…

Q: 0 When 4.18 g of a certain molecular compound X are dissolved in 45.0 g of benzene (C6H6), the…

Question

100%

The freezing point of pure water is 0°C and its molal freezing point depression constant (Kf) is 1.86°C/m.

a. What is the change in the freezing point (∆Tf) of a solution that contains 53 grams of sucrose (MW= 342.3 g/mol) dissolved in 1000 grams of water.

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 3

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

What is the freezing point of a solution made by dissolving 45.0 g of glucose (C2H12O6) in 500. g of water? The freezing point depression constant, Kf, of water is 1.86 °C/m and the molar mass of glucose is 180.0 g/mol. ΔTf = Kf m i a. -0.465°C b. -0.620°C c. -1.86°C d. -0.930°C
The molal boiling point elevation constant K = 1.15 °C·kg⋅mol the solution boils at 145.4 °C. Calculate the boiling point of pure X. Be sure your answer has the correct number of significant digits. °C x10 1 for a certain substance X. When 14.4 g of urea Ś ((NH,),CO) (NH₂) CO) are dissolved in 150. g of X,
3. 2 g of NacI is dissolved in 500 g of water at 35°C. Determine the ff: PNacI • 2.16 cm a. Boiling point elevation b. Freezing point depression C. Vapor pressure of the solution d. Osmotic pre ssure
When 605. mg of a certain molecular compound X are dissolved in 100. g of cyclohexane (CH₁₂), the freezing point of the solution is measured to be 6.4 °C. Calculate the molar mass of X. If you need any additional information on cyclohexane, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and t is rounded to I significant digit. 0 8 0.8 D-D X 4 G
Calculating molality.
A student dissolves 20. g of benzoic acid (C,H,O,) in 125. mL of a solvent with a density of 1.07 g/mL. The student notices that the volume of the solvent does not change when the benzoic acid dissolves in it. Calculate the molarity and molality of the student's solution. Be sure each of your answer entries has the correct number of significant digits. molarity Ox10 molality %D
Use the graph to estimate the solubility of NANO3 in water at 40 °C. * Effect of temperature on solubility 160 KNO, 140 NANO, 120 100 KBr- 80 NH,CI 60 Na,So, 40 NaCI 20 10 20 30 40 50 60 70 80 90 Temperature (°C) 68 g/100 g H20 O 77 g/100 g H20 96 g/100 g H20 O no solubility Concentration (g/100 g H;0)
Please help with the following:
A certain organic compound O has a solubility in acetonitrile of 13.8 at 25. °C. Calculate the mass of O that's dissolved in L 650. mL of a saturated solution of O in acetonitrile at this temperature. Be sure your answer has the correct unit symbol and 3 significant digits. x10
Ethylene glycol (EG), CH₂(OH)CH₂(OH), is a common automobile antifreeze. It is water soluble and fairly nonvolatile (b.p. 197 °C). Calculate the freezing point of a solution containing 651 g of this substance in 2505 g of water. Would you keep this substance in your car radiator during the summer? The molar mass of ethylene glycol is 62.01 g.
1. Suppose that you add 27.5 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 oC/m. With the added solute, you find that there is a freezing point depression of 3.58 oC compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound? 2. What is the freezing point (in degrees Celcius) of 3.70 kg of water if it contains 187.4 g of CaBr2? The freezing point depression constant for water is 1.86 oC/m and the molar mass of CaBr2 is 199.89 g/mol. 3. What mass, in grams, of NaCl needs to be added to 1.6 kg of water in order to create a solution with a freezing point of -5.6 °C? The freezing point depression constant of water is 1.86 ºC/m.
When 911. mg of a certain molecular compound X are dissolved in 35.0 g of benzene (C,H6), the freezing point of the solution is measured to be 2.5 °C. Calculate the molar mass of X. If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. Ox10 미□