A dilute solution of acetic acid produced by fermentation and oxidation of natural carbohydrates is called vinegar. If 44.4 g of acetic acid, CH3COOH, are dissolved in 67.1 g of water, what is the mole fraction of acetic acid?Atomic Mass:C=12.01 ; H=1.008 ;O = 16.0Express your answer in three decimal places. Do not write the unit.

Mole fraction can be calculated by using the formula: Mole fraction of X = Number of moles of XTotal…

Answered: A dilute solution of acetic acid…

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...

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A sample of Al metal was reacted with 10.0 mL of HCl solution to produce 150.0 mL of H2 gas at 25 °C and 0.975 atm Calculate the molarity of the HCl solution. 2 Al + 6 HC1 – →2 AlCl3 +3 H2 Express the answer to 3 sig. figs.
CHEMY 101 SEC SEM 12 2020-21 2 Enter your answer in the provided box. How many grams of sucrose (C1,H01) must be added to 499 g of water to give a solution with a vapor pressure 0.287 mmHg less than that of pure water at 20°C? (The vapor pressure of water at 20°C is 17.5 mmHg.) X 01:40:30
A 365 µM solution of a dye molecule, Rhodamine 6G, dissolved in methanol is allowed to sit open to the air such that the volume of the solution is reduced to 43% of its original volume due to evaporation of methanol. Assuming that no dye molecules are lost during the evaporation process, what is the concentration of the dye in the remaining ethanol after evaporation?
Boiling Point Elevation/Freezing Point Depression AT = m K where, for freezing point depression: AT = T(pure solvent) - T(solution) and for boiling point elevation: AT = T(solution) - T(pure solvent) m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Formula H₂O Kb(°C/ m) Kf(°C / m) 0.512 1.86 1.22 1.99 3.67 Benzene 2.53 Diethyl ether CH3CH₂OCH2CH3 2.02 Solvent Water Ethanol Chloroform CHCl3 C6H6 CH3CH₂OH 5.12
4- 30- [14] How many liters of the antifreeze ethylene glycol (HOCH₂CH₂OH, 54.09 g/mol) would you add to a car-radiator containing 6.50 L of water to keep it from freezing if the coldest winter temperature in your area is -20°C? Calculate the boiling point of this water-ethylene glycol mixture. (The density of ethylene glycol is 1.11 g/mL, the molal freezing and boiling point constants are respectively kf = 1.86°/m and kb= 0.52 °/m). & Page 5
What is the osmotic pressure (N) of a solution containing 0.125 mol of a nonelectrolyte in 0.500 L of solution at 25°C? R = 0.0821 L·atm/mol·K. Give your answer for atm and mmHg. Follow the 3 significant figures. No need to include the units in your answer. For scientific notation express your answer by using E as x10. For example for 2.23x103 --> 2.23E3
The diving atmosphere used by the U.S. Navy in its undersea Sea-Lab experiments consisted of 0.036 mole fraction O2 and 0.056 mole fraction N2, with helium (He) making up the remainder. What are the masses of nitrogen, oxygen, and helium in a 8.47 g sample of this atmosphere? Mass of oxygen = Mass of nitrogen = Mass of helium =
17
A dilute solution of acetic acid produced by fermentation and oxidation of natural carbohydrates is called vinegar. If 48.7 g of acetic acid, CH3COOH , are dissolved in 68.1 g of water, what is the mole fraction of acetic acid? Atomic Mass: C=12.01 ; H=1.008 ; O = 16.0 Express your answer in three decimal places. Do not write the unit.
(please type answer).
At 25.0 °C the Henry's Law constant for nitrogen monoxide (NO) gas in water is 0.0019 M/atm. Calculate the mass in grams of NO gas that can be dissolved in 425. mL of water at 25.0 °C and a NO partial pressure of 4.98 atm. Round your answer to 2 significant digits. Submit 0 x10 X S
H law

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