Given that the vapor pressure of water is 17.54 Torr at 20 °C, calculate the vapor-pressure lowering, AP, of an aqueoussolution that is 2.30 m in sucrose (C1,H2011).AP =0.6978TorrCalculate the vapor-pressure lowering, AP, of an aqueous solution that is 2.30 m in aluminum chloride. Assume 100%dissociation for electrolytes.ΔΡ-Torr- TOOLSx10

Given that: Vapor pressure of water = 17.54 Torr Molality of sucrose = 2.30 m Molality of…

Given that the vapor pressure of water is 17.54 Torr at 20 °C, calculate the vapor-pressure lowering, AP, of an aqueous solution that is 2.30 m in sucrose (C,H„O1). AP = | 0.6978 Torr Calculate the vapor-pressure lowering, AP, of an aqueous solution that is 2.30 m in aluminum chloride. Assume 100% dissociation for electrolytes. AP = Torr - TOOLS x10

Given that the vapor pressure of water is 17.54 Torr at 20 °C, calculate the vapor-pressure lowering, AP, of an aqueous solution that is 2.30 m in sucrose (C,H„O1). AP = | 0.6978 Torr Calculate the vapor-pressure lowering, AP, of an aqueous solution that is 2.30 m in aluminum chloride. Assume 100% dissociation for electrolytes. AP = Torr - TOOLS x10

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter10: Effect Of Electrolytes On Chemical Equilibria

Section: Chapter Questions

Problem 10.8QAP

See similar textbooks

Similar questions

Assume that the solubility of carbon dioxide gas in pop at 5oC is 0.586 g/100 mL and at 20oC its solubility is 0.169 g/100 mL. What mass of carbon dioxide gas will escape from a 355-mL can of Coke that has been taken out of the fridge and has been sitting open at 20oC?
What is the activity of liquid water of a multicomponent solution in which the vapor pressure of water is 748.2 mmHg at 100.0 0C?
The henry constant for the dissolution of CO2 in water is 3.4 x 10^-2 atm/M at 25°C. Assuming ideal behavior, calculate the pressure of CO2 gas required to reach 0.0018 mole fraction of CO2 in the prepared carbonated water. density of carbonated water=1gcm^-3
The molar mass of phenolphthalein, an acid-base indicator, was determined by osmotic pressure measurements. A student obtained an osmotif pressure of 14.6mm Hg at 25C for a 2.00-L solution containing 500.0 mg of phenolphthalein. What is the molar mass of phenolphthalein?
Given that the value of Kf for water is 1.86°C/m, what is the freezing point of an aqueous solution of NaCl (58.45 g/mol) prepared by mixing 427.0 g solute with 1.000 kg of water?
The partial pressure of O₂(g), referred to as P(O₂(g)), in the lungs is 0.210 atm. The Keq of oxygen dissolving at 310.0 K is 6.32 x 10⁻⁴. Calculate molar concentration of O₂(aq) dissolved in blood at 310.0 K (body temperature) that is in equilibrium with O₂(g).
Phenol (C6H5OH) is partially dimerized in the solvent bromoform. When 2.58 g of phenol is dissolved in 100 g of bromoform, the bromoform freezing point is lowered by 2.37°C. Pure bromoform freezes at 8.3°C and has kf = 14.1°C kg/mol. Calculate the equilibrium constant Km for the dimerization reaction of phenol in bromoform at 6°C, assuming an ideally dilute solution.
2. What is the total equilibrium vapor pressure of a benzene toluene solution if the mole fraction of benzene is 0.249? (The equilibrium vapor pressure is 95.1 mmHg for pure benzoic and it is 28.4 mmHg for pure toluene.)
What is the freezing point (°C) of a solution prepared by dissolving 31.1 g of Ca(OH)2 in 185 g of water? The molal freezing point depression constant for water is 1.86 °C/m (assume complete dissociation of the salt?)
Given that the value of kf for water is 1.86°C/m, what is the freezing point of an aqueous solution of NaCl prepared by mixing 427.0 g solute with 1.000 kg of water? Show your work for full credits (just explain step by step and put the answer at the end)
Calculate the vapor pressure of salt solution containing 20g salt (NaCl) in 1.5 kg of water at 25C
Calculate the osmotic pressure at 25°C across a semipermeable membrane separating seawater (1.14 M total particles) from a 0.436 M solution of aqueous NaCl.