Calculate the vapor pressure of a solution made by dissolving 11.1 g Ca(OH)2 in 1 102 g of water at 25 °C. Vapor pressure of pure water is 23.76 mm Hg at 25 °C. View Available Hint(s) O21.4 mmHg O23.1 mmHg 22.0 mmHg O25.5 mmHg

Calculate the vapor pressure of a solution made by dissolving 11.1 g Ca(OH)2 in 1 102 g of water at 25 °C. Vapor pressure of pure water is 23.76 mm Hg at 25 °C. View Available Hint(s) O21.4 mmHg O23.1 mmHg 22.0 mmHg O25.5 mmHg

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: At 25 °C, the vapor pressure of ethanol is 60.0 mmHg and the vapor pressure of methanol is 127.0…

A: Given, Vapor pressure of ethanol = 60.0 mmHg Vapor pressure of methanol = 127.0 mmHg Molar ratio of…

Q: What would be the theoretical freezing point of a solution made by dissolving 10.48 g of NaCl in…

A: Freezing point of solution is less then freezing point of pure solvent

Q: A solution is prepared by mixing 45.68 g of carbon disulfide (CS2, 76.13 g/mol) with 16.42 g of…

A: We know that, the partial pressure of solute in vapor phase is equal to the mole fraction of solute…

Q: 1.What will be the new vapor pressure of the water in a 250 mL solution of 0.3774M solution of…

A: We will use colligative property i.e. relative lowering in vapour pressure to calculate vapor…

Q: The vapor pressure of pure water at 25 °C is 23.8 torr. What is the vapor pressure (torr) of water…

Q: A solution made by dissolving 0.502 g of an unknown electrolyte in 25.00 g of CCI4. The solution…

A: In the given question, molar mass of unknown electrolyte is to be found. The formula used is :-∆Tb =…

Q: What will be the vapor pressure of a solution, at 30°C, made by dissolving 50.0 g of a glucose…

Q: Calculate the vapor pressure above a solution prepared by dissolving 2.50 g of aspirin (C9H8O4) in…

Q: What is the solubility of xenon (in units of grams per liter) in water at 25 °C, when the Xe gas…

Q: A 132 g sample of a nonvolatile compound was dissolved in 4.30 mol of cyclohexane (P° = 100.0 mmHg).…

A: Given data: The mass of the sample (solute)=132 g. The moles of cyclohexane (solvent) n2=4.30 mol.…

Q: Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (CeH1206) in…

Q: Which aqueous solution has the LOWEST freezing point? 2 MC12H22O11 2 M Na2SO4 2 M KCl O2 M MgSO4

A: The objective of the question is to determine which among the given aqueous solutions has the lowest…

Q: A solution is prepared by dissolving 30.7 g ethylene glycol (M 62.0) in 500.0 mL H2 O. What is the…

A: I am providing you an Image that has solution of the desired problem

Q: Mg(s) + 2 HCI(aq) → MgCl₂(aq) + H₂(9) The total pressure of gas collected over water is 710.0 mmHg…

Q: Calculate the change in vapor pressure (DP) of a solution prepared by dissolving 25.5 g of…

Q: A solution was prepared by dissolving 12.0 g of glucose (180 g/mol) in 150. mL solution. What is the…

Q: A 1.00 % by mass solution of lactose (C12H22011, 342.30 g/mol) in water has a density of 1.0602 g/mL…

A: Given, density of Solution = 1.0602 g/mL Mass % lactose = 1.00 % Molar mass of lactose = 342.30…

Q: AKCI solution is prepared by dissolving 25.0 g KCI in 250.0 g of water at 25°C. What is the vapor…

A: From Rault's law we can calculate the change of vapor pressure of a solution from the vapor…

Q: Calculate the molality of a solution prepared by dissolving 12.1 g of CH3OH in 475 g of water O 2.40…

A: Mass of CH3OH = 12.1 g Mass of water = 475 g Molality of the solution = ?

Q: The vapor pressure of pure water is 23.80 torr at 25.00°C. Determine the vapor pressure of an…

A: We will first find mole fraction of each component. Then find vapor pressure of solution using…

Q: Calculate the boiling point (oC) at P = 1 atm of a solution of 15.0 g of acetone (MM = 58.080 g/mol)…

A: Given; The given mass of acetone, (Wb) = 15 g. The given mass of camphor, (Wa) = 50 g=0.05 Kg. The…

Q: the density of a 3.539 M HNO3 aqueous solution is 1.150 g x mL-1 at 20 Degrees C. What is the molar…

A: Given Molarity = 3.539 M Density = 1.15 g/ml

Q: Which of the following solutions will be expected to have the highest vapor pressure? O 0.10 m…

A: The colligative properties are those properties of solutions that depend on the number of solute…

Q: The solubility of solid X is given below. What is the maximum percent recovery if a student wanted…

A: NOTE: Assuming that the initial temperature is 100 oC and the final temperature is 0 oC as per the…

Q: What is the molality of ethanol (C₂H5OH) in an aqueous solution that is 39.8% ethanol by mass? O…

Q: The enthalpy of solution of KCI is 40 kJ/mol. The hydration energies of K* and Cl are -315 kJ/mol…

A: Lattice energy is the amount of energy released when one mole of crystalline ionic compound formed…

Q: A sample of aqueous Ethylene Glycol (C₂H602) is prepared by adding some Ethylene Glycol to 700 grams…

A: i = 1 as the solute is non-electrolyteT(solvent) = 0.0oCT(solution) = -2.85oCKf = 1.9oC/m

Q: Solutions & Colligative Properties 1. The vapor pressure of water at 20°C is 17.5 torr. What is the…

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

Q: A solution is prepared by adding 15.00 g of lactose (milk sugar) to 110.0 g of water at 55°C. The…

A: GIVEN: Given mass of lactose=15 gGiven mass of water=110 gVapor pressure of pure water at 55 degree…

Q: calculate the molality of ethylene glycol required to decrease the freezing point of water by 6.2 °C…

Q: A 1.09 g sample of substance X is dissolved in 26.8 g of benzene. The freezing point of the solution…

A: The ratio of moles of solute to the mass of the solvent in kg is known as molality.

Q: The concentration in molality of HCI in a solution that is prepared by dissolving 5.5 g of HCI in…

A: The concentration of HCl solution can be calculated as

Q: Consider a solution made by dissolving 331 g of sucrose in 116 ml of water at 45˚C. The vapor…

A: Given data are, given mass of sucrose = 331 g given volume of water = 116 mL density of water =…

Q: Determine the boiling point of a solution that contains 70.6 g of naphthalene (molar mass 128.16…

A: Molality of solution can be calculated as follows:

Q: Choose the aqueous solution below with thelowest freezing temperature. 0.200 m NaCI 0.200 m…

A: To identify: Solution with lowest freezing temperature.

Q: Which of the following aqueous solutions should have the lowest freezing point? 1.0 m NaCl 1.0…

A: When non volatile solute is added to solution , the freezing point of solution decreases. This is…

Q: The vapor pressure of pure water is lower than the vapor pressure of a 3.20 m solution. O True O…

A: Colligative property is the property which depends only on the number of solute particles in the…

Q: Choose the aqueous solution below with the lowest freezing point. All solutions are made of…

A: Given, Depression in freezing point is a colligative property which depends upon the amount of…

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

Calculate the vapor pressure of a solution made by dissolving 11.1 g Ca(OH)2 in 1 102 g of water at 25 °C. Vapor pressure of pure water is 23.76 mm Hg at 25 °C.
▸ View Available Hint(s)
O21.4 mmHg
O23.1 mmHg
22.0 mmHg
25.5 mmHg

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: Given data

VIEW

Step 2: Calculation of moles of calcium hydroxide and water

VIEW

Step 3: Calculation of total moles and mole fraction of water

VIEW

Step 4: Calculation of vapor pressure of a solution

VIEW

Step 5: Explanation for incorrect options

VIEW

Solution

VIEW

Step by step

Solved in 6 steps with 8 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

By how much will the vapor pressure of water decrease if a solution at 40.0°C is produced by dissolving 17.1555 g of Co(NO3)3 (formula mass = 244.93 g/mol) with 29.3720 g of water. The vapor pressure of pure water at this temperature is 55.30 mmHg. If the solute is ionic, assume that it is completely ionic!
The vapor pressure of water at 45.0 °C is 71.93 mmHg. Calculate the vapor pressure of a solution of 1.25m Al(ClO3)3 at this temperature (assume 100% dissociation). Hint - the moles of solvent is 55.5 moles and the moles of solute is 5.0 moles. Group of answer choices 360. mmHg 89.9 mmHg 71.9 mmHg 70.4 mmHg 66.0 mmHg
A sample of an ionic solid is dissolved in 1.00 kg of water. The freezing point of the water is -0.01 °C. If three times the mass of ionic solid is dissolved in 1.00 kg of water and the resulting freezing point of the solution is -0.09 °C, which of the following would be possible formulas for the solid: MX, MX2, or MX3, where M represents a metal cation and X an anion with a 1- charge? Explain your reasoning.
A solution contains 45.0 g of glucose, C6H12O6, dissolved in 175.0 g of water at 22C. Calculate the vapor pressure of this solution in the atmosphere. The vapor pressure of pure water is 19.8 mm Hg at 22C.
What would be the theoretical freezing point of a solution made by dissolving 10.43 g of NiCl 2 in 365.0 g of water? The freezing point constant of water is 1.86 °C/molal. The molar mass of NiCl 2 is 129.5994 g/mol. 1.230 °C 1.506 °C 0.8128 °C -1.230 °C 1.022 °C
The freezing point of CCI4 is -22.3°C and the freezing point depression constant is 29.8 °C/m. If a solution of C5H12 in CCI4 freezes at -37.6°C, what is the molality of this solution? O 0.513 0.722 O 2.01 O 5.01 O 1.26
What would be the theoretical freezing point of a solution made by dissolving 5.444 g of CaSO 4 in 140.0 g of water? The freezing point constant of water is 1.86 °C/molal. The molar mass of CaSO 4 is 136.14 g/mol. -0.8291 °C -0.6091 °C 1.063 °C 0.9412 °C -1.063 °C
A solution is made by dissolving 41.3 g urea (CH4N20), a nonelectrolyte, in 275 g water. Calculate the vapor pressure of this solution at 25°C and 45°C. vapor pressure of water 25°C 23.8 torr 45°C 71.9 torr vapor pressure at 25°C = torr vapor pressure at 45°C = torr
Choose the aqueous solution below with the lowest freezing point. All solutions are made of nonvolatile solutes. 0.200 m C6H12O6 0.200 m Al2(SO4)3 0.200 m K3PO4 0.200 m Ca(ClO4)2 These all have the same freezing point
What is the freezing point of a solution prepared by dissolving 5.84 g Na2SO4 in 250.0 g H2O?
Choose the aqueous solution that has the lowest melting point. There are all solutions of nonvolatile solutes. A) 0.150 m CaCl2 B) 0.200 m C6H12O6 C) 0.125 m NaCl D) 0.100 m AlCl3 E) They all have the same melting point.
Vapor pressure of water is 31.8 torr at 30°C. If 17.9 g AlCl3 is dissolved in 100. g of water, calculate the vapor pressure of the solution. O 29.0 torr 28.2 torr O26.5 torr O 31.0 torr