A KCI solution is prepared by dissolving 60.0 g KCI in 250.0 g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 ?mmHg mmHg 22.5O mmHg 21.3O mmHg 25.5O

A KCI solution is prepared by dissolving 60.0 g KCI in 250.0 g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 ?mmHg mmHg 22.5O mmHg 21.3O mmHg 25.5O

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 60QAP: An aqueous solution of M2O is prepared by dissolving 10.91 g of the electrolyte in 435 mL of...

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: A solution is prepared from 2.00 x 10 2 g of sucrose (342g/mol) and 3.5 x 10 2 g water (18 g/mol).…

A: Given values- Weight of Sucrose = 200 gm Weight of water = 350 gm Vapour pressure of water = 17.5…

Q: Calculate the vapor pressure at 50°C of a coolant solution that is 51.0:49.0 ethylene…

A: Raoult’s law: Raoult’s law states that partial pressure of the substance above a solution is equal…

Q: A solution was prepared by mixing 24.6 grams of camphor (C10H16O), an FDA-approved topical analgesic…

A: Ans Moles of the camphor = 24.6 grams152.23g/mol = 0.16159 mol Moles of the Benzene = given density…

Q: The vapor pressure of chloroform is 173.11 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that…

A: Raoult's law :- According to this law " The relative lowering vapour pressure ( RLVP ) of a…

Q: The vapor pressure of diethyl ether (ether) is 463.6 mm Hg at 25 °C. How many grams of chlorophyll ,…

A: We have to determine the mass of a non-volatile, non-electrolyte solute chlorophyll solute that is…

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

Q: 20 g of compound A (Mwt=46), with vapor pressure 400 mmHg at 70°C, mixed with 15g of compound B…

A: This question is related to finding out the total vapor pressure. The method is correct undoubtedly.…

Q: Glycerin (C3H8O3) is a nonvolatile nonelectrolyte with a density of 1.26 g/mL at 25 °C. Calculate…

A: Since volume of water = 500 mL => mass of water = volume X density = 500 X 1 = 500 g Hence moles…

Q: 20 g of compound A (Mwt=46), with vapor pressure 420 mmHg at 60°C, mixed with 15g of compound B…

Q: solution in a sealed flask contains 15 g of sodium chloride in 150 mL water. Given the vapor…

A: Given mass of sodium chloride = 15 g Molar mass of sodium chloride = 58.5 g/mol Number of moles of…

Q: Ethanol (C₂H₅OH) has a vapor pressure of 93.0 torr and a density of 0.785 g/mL. Pentane (C₅H₁₂) has…

A: Given Vapour pressure of ethanol (P1°) = 93 torr Vapour pressure of pentane (P2°) = 435 torr…

Q: Calculate the vapor pressure in millimeters of mercury for a 3.52 M KCI aqueous solution at 50°C.…

Q: A solution contains a mixture of two volatile substances A and B. The mole fraction of substance A…

Q: The vapor pressure of benzene is 100.0 mmHg at 26.1°C. Calculate the vapor pressure of a solution…

Q: A 2.0 L aqueous solution contains 0.25 mole of CaCO3. What is the concentration (molality) of the…

Q: 80.0 g of non-volatile maltose (molar mass = 342.34 g/mol) is added to 152 g of water (molar mass =…

A: The expression that can be used to determine the vapor pressure of the resulting solution is the…

Q: 5.152g of Na2CO3(s) is added to 75.0mL of water at 21.20°C. When the dissolution is complete, the…

A: Please find the solution attached here as handwritten note.

Q: The vapor pressure of ethanol is 54.68 mm Hg at 25°C. How many grams of saccharin, C7H5NO3S, a…

A: Vapor pressure of pure ethanol = 54.68 mm Hg Vapor pressure of solution = 53.52 mm Hg The relative…

Q: The liquid used in automobile cooling systems is prepared by dissolving ethylene glycol (HOCH2CH2OH)…

A: For an ideal solution the Raoult's Law states that partial vapor pressure of a component in a…

Q: 9. A solution is prepared by dissolving 248 g of sucrose (C12H2½O11; MM = 342.0 g/mol) in 155 g…

A: Moles of sucrose are, Moles = mass ÷ molar mass Moles = 248 g ÷ 342.0 g/mol Moles = 0.73 mol Moles…

Q: The liquid used in automobile cooling systems is prepared by dissolving ethylene glycol (HOCH2CH2OH)…

A: Number of moles of ethylene glycol and water is calculated,If the total volume of coolant is assumed…

Q: The vapor pressure of benzene is 73.03 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves…

A: Raoult's Law :- The relative lowering vapor pressure of a dilute solution containing non volatile…

Q: a. Is -8.0C°. What is the molal concentration of the solution? (K; =-1 a-1.86 b-4.3 C-4.5 d-14.8…

A: Given, Freezing point of the solution = Tf = - 8.0 0C What is the molal concentration or molality…

Q: The vapor pressure of ethanol is 54.68 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves…

A: Since you have posted multiple question, we will solve only first question for you. To get rest of…

Q: The vapor pressure of chloroform is 173.11 mm Hg at 25°C. How many grams of testosterone, C19H2802,…

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: The freezing point of an aqueous solution of MgBr, was found to be -5.7 °C. Calculate the boiling…

A: The given information is: Tf(solvent) = -5.7°C Tf(solution) = 0°C Calculating the depression in the…

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: Calculate the vapor pressure lowering when 15.0 g of glucose (Mv= 180.18 g/mol) is dissolved in 100…

A: Lowering in vapor pressure is one of the colligative property which depend only on the number of…

Q: Calculate the vapor pressure in mmHg of aqueous solution containing 60 g of urea (m.m 60 g/mole) in…

Q: A solution is prepared by mixing 75 g of methanol (CH3OH, 32.04 g/mol) with 25 g of ethanol…

Q: liquid. What is the vapor pressure of solution made by adding 150. 9 of glycer torr and its density…

A: Given -> Weight of glycerine= 150 gm Volume of H2O = 325 ml = 0.325 L (1L = 1000ml) Temperature…

Q: A solution is prepared by dissolving 413 g of sucrose (C12H22O11) in 614 g of water. What is the…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: What would be the theoretical freezing point of a solution made by dissolving 15.56 g of CrSO 4 in…

Q: A solution is prepared by dissolving 62.0 g of glucose, C,H, O, in 125.0 g of water. At 30.0 °C 12…

A: Vapour pressure of a solution can be calculated by using Following formula - P = X P0 Here , P is…

Q: en the solute and the solvent have the same intermolecular forces . true or false ? 2. If the mass…

A: Answer (1) true because "like dissolve like" principle when solute and solvent have same kind of…

Q: A solution is prepared by dissolving 70 g of sucrose in 250 g of water at 25 degrees Celsius. What…

A: According to Raoult’s law, for solutions that contain non-volatile solutes, the vapor pressure of…

Q: The vapor pressure of chloroform is 173.11 mm Hg at 25 C. A nonvolatile, nonelectrolyte that…

A: This numerical is related to relative lowering of vapour pressure. The formula used is: Po is the…

Q: Safrole is used as a topical antiseptic. Calculate the vapor pressure of a solution prepared by…

Q: A solution was prepared by mixing 24.6 grams of camphor (C10H16O), an FDA-approved topical analgesic…

A: According to the Raoults law, the vapour pressure of the solution is - Ps = Po X Here - Ps = vapour…

Q: Consider a solution made by dissolving 339 g of sucrose in 123 ml of water at 45˚C. The vapor…

Q: The vapor pressure of benzene is 100.0 mmHg at 26.1°C. Calculate the vapor pressure of a solution…

Q: An aqueous solution containing glucose has a vapor pressure of 19.4 torr at 25°C. What would be the…

A: Given data:

Q: The vapor pressure of chloroform is 173.11 mm Hg at 25°C.How many grams of cholesterol, C27H46O, a…

A: Relative lowering of vapor pressure is equal to the mole fraction of solute.

Q: Calculate the mass of urea that should be dissolved in 197 g of water at 35 ° C to produce a…

A: The dissolution of a specific mass of a solute in a specific volume of the solvent produces a…

Q: A solution is made by dissolving 37.1 g urea (CHAN20), a nonelectrolyte, in 275 g water. Calculate…

A: Answer: On dissolving a non-volatile solute in a solvent, vapor pressure of the solution according…

Q: Use the References to dle The vapor pressure of ethanol is 54.68 mm Hg at 25 °C. A nonvolatile,…

Q: What is the molality of p-dichlorobenzene (C6H4Cl2, 147 g/mol) when 2.65 g is dissolved in 50.0 mL…

Question

I need the answer as soon as possible

A KCI solution is prepared by
dissolving 60.0 g KCI in
250.0 g of water at 25°C.
What is the vapor pressure
of the solution
if the vapor pressure of
water at 25°C is 23.76
?mmHg
mmHg 22.5O
mmHg 21.3O
mmHg 25.5O
mmHg 20.5O

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

A sucrose (C12H22O11) solution that is 45.0% sucrose by mass has a density of 1.203 g/mL at 25C. Calculate its (a) molarity. (b) molality. (c) vapor pressure(vpH2Oat25C=23.76mmHg). (d) normal boiling point.
Consider two hypothetical pure substances, AB(s) and XY(s). When equal molar amounts of these substances are placed in separate 500-mL samples of water, they undergo the following reactions: AB(s)A+(aq)+B(aq)XY(s)XY(aq) a Which solution would you expect to have the lower boiling point? Why? b Would you expect the vapor pressures of the two solutions to be equal? If not, which one would you expect to have the higher vapor pressure? c Describe a procedure that would make the two solutions have the same boiling point. d If you took 250 mL of the AB(aq) solution prepared above, would it have the same boiling point as the original solution? Be sure to explain your answer. e The container of XY(aq) is left out on the bench top for several days, which allows some of the water to evaporate from the solution. How would the melting point of this solution compare to the melting point of the original solution?
An aqueous solution of M2O is prepared by dissolving 10.91 g of the electrolyte in 435 mL of H2O(d=1.00g/mL). The solution freezes at -4.68C. What is M+? (Assume complete dissociation of M2O to M+ and O2-.)
In some regions of the southwest United States, the water is very hard. For example, in Las Cruces, New Mexico, the tap water contains about 560 g of dissolved solids per milliliter. Reverse osmosis units are marketed in this area to soften water. A typical unit exerts a pressure of 8.0 atm and can produce 45 L water per day. a. Assuming all of the dissolved solids are MgCO3 and assuming a temperature of 27C, what total volume of water must be processed to produce 45 L pure water? b. Would the same system work for purifying seawater? (Assume seawater is 0.60 M NaCl.)
Carbon tetrachloride (CCl4) boils at 76.8C and has a density of 1.59 g/mL. (a) A solution prepared by dissolving 0.287 mol of a nonelectrolyte in 255 mL of CCl4 boils at 80.3C. What is the boiling point constant (kb) for CCl4? (b) Another solution is prepared by dissolving 37.1 g of an electrolyte (MM=167g/mol) in 244 mL of CCl4. The resulting solution boils at 85.2C. What is i for the electrolyte?
An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25 C. (a) What is the average molar mass of starch? (The result is an average because not all starch molecules are identical.) (b) What is the freezing point of the solution? Would it be easy to determine the molecular weight of starch by measuring the freezing point depression? (Assume that the molarity and molality are the same for this solution.)
Silver ion has an average concentration of 28 ppb (parts per billion) in U.S. water supplies. (a) What is the molality of the silver ion? (b) If you wanted 1.0 102 g of silver and could recover it chemically from water supplies, what volume of water in liters would you have to treat? (Assume the density of water is 1.0g/cm3.)
An organic compound contains carbon (71.17%), hydrogen (5.12%) with the remainder nitrogen. Dissolving 0.177 g of the compound in 10.0 g of benzene gives a solution with a vapor pressure of 94.16 mm Hg at 25 C. (The vapor pressure of pure benzene at this temperature is 95.26 mm Hg.) What is the molecular formula for the compound?
A sample of HgCI2 weighing 9.41 g is dissolved in 32.75 g of ethanol, C2H5OH ( Kb=1.20 C/m). The boiling point elevation of the solution is 1.27 C. Is HgCI2 an electrolyte in ethanol? Show your calculations.
Glycerin, C3H8O3, is a nonvolatile liquid. What is the vapor pressure of a solution made by adding 164 g glycerin to 338 mL H2O at 39.8C? The vapor pressure of pure water at 39.8C is 54.74 torr and its density is 0.992 g/cm3.
An aqueous solution contains 0.180 g of an unknown, nonionic solute in 50.0 g of water. The solution freezes at 0.040 C. What is the molar mass of the solute?
A carbonated beverage is made by saturating water with carbon dioxide at 0C and a pressure of 3.0 atm. The bottle is then opened at room temperature (25C), and comes to equilibrium with air in the room containing CO2(PCO2=1.0103M/atm). The Henry's law constant for the solubility of CO2 in water is 0.0769 M/atm at 0C and 0.0313 M/atm at 25C. (a) What is the concentration of carbon dioxide in the bottle before it is opened? (b) What is the concentration of carbon dioxide in the bottle after it has been opened and come to equilibrium with the air?