Q4/A liquid mixture is prepared by combining N different liquids with densities pi; pz: ...PN. The volume of component i added to the mixture is V, and the mass fraction of thiscomponent in the mixture is x. The components are completely miscible. The following twoformulas provide estimates of the density of the liquid mixture, , if the volume of themixture equals the sum of the pure-component volumes. Only one of the formulas is correct,however.(i) p(ii)Determine whether (i) or (i) is the correct formula (show your proof), and then use thecorrect formula to estimate the density (g/cm) of a liquid mixture containing 60.0 wt%acetone, 25.0 wt% acetic acid, and 15.0 wt% carbon tetrachloride.

The mass fraction wi is defined as the fraction of one substance with mass mi to the mass of the…

Q4/ A liquid mixture is prepared by combining N different liquids with densities pi; p2: ... PN. The volume of component i added to the mixture is V, and the mass fraction of this component in the mixture is x. The components are completely miscible. The following two formulas provide estimates of the density of the liquid mixture, p, if the volume of the mixture equals the sum of the pure-component volumes. Only one of the formulas is correct, however. (i) p: (ii) Determine whether (1) or (ii) is the correct formula (show your proof), and then use the correct formula to estimate the density (g/cm') of a liquid mixture containing 60.0 wt% acetone, 25.0 wt% acetic acid, and 15.0 wt% carbon tetrachloride.

Q4/ A liquid mixture is prepared by combining N different liquids with densities pi; p2: ... PN. The volume of component i added to the mixture is V, and the mass fraction of this component in the mixture is x. The components are completely miscible. The following two formulas provide estimates of the density of the liquid mixture, p, if the volume of the mixture equals the sum of the pure-component volumes. Only one of the formulas is correct, however. (i) p: (ii) Determine whether (1) or (ii) is the correct formula (show your proof), and then use the correct formula to estimate the density (g/cm') of a liquid mixture containing 60.0 wt% acetone, 25.0 wt% acetic acid, and 15.0 wt% carbon tetrachloride.

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

Similar questions

A gas mixture for use in some lasers contains 4.65 %%by weight HClHCl, 2.35 %% H2H2, and 93 %% NeNe. Part A: What is the mole fraction of HClHCl in this mixture? Part B: What is the mole fraction of HClHCl in this mixture? Part C: What is the mole fraction of NeNe in this mixture?
A chemist attempts to prepare some very pure crystals of borax by dissolving 100g of Na2B4O7 in 200 grams of boiling water. He then cools the solution slowly until some borax crystallizes out. Calculate the grams of borax recovered in the crystals per 100 grams of initial solution (Na2B4O7 plus water), if the residual solution at 550C after the crystals are removed contains 12.4% Na2B4O7.What is the percent yield or percent recovery of Na2B4O7.
Boiling Point Elevation/Freezing Point Depression T = m K where, for freezing point depression: T = T(pure solvent) - T(solution) and for boiling point elevation: T = 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. Solvent Formula Kb(°C / m) Kf(°C / m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02
- 2022.pdf - Adobe Acrobat Pro DC (32-bit) ndow Help oter 14 - Soluti. x 2 / 3 100% 9) An aqueous solution has a normal boiling point of 103.0°C. What is the freezing point of this solution? For water Kb = 0.51°C/m and Kf=1.86°C/m. 9) A) -0.82°C B) -3.0°С С) -3.6°C D) -11°C 10) A solution of an 22.4 g of an unknown protein dissolved in enough water to make 0.150 L of solution has an osmotic pressure of 658 torr at 25°C. Based on these data, what is the molar mass of the protein? 10) search hp
The graph given below plots the (approximate) partial molar volumes of ethanol (black line) and water (red line) in units of ml/mole at 25°C in a mixture as a function of the mole fraction of ethanol. Use the information in this graph (note the different y axes for water and ethanol) and the densities at 25°C to calculate the resulting total volume of the g following two mixtures.(pethanol = 0.789 ml & PH20 = 0.998 ) ml a. 150 ml ethanol + 100 ml H2O b. 200 ml ethanol + 40 ml H2O H20 VELOH Vet o*HA -V ELOH V H2O T 0.8 1.0 0.2 0.4 0.6 0.0 XELOH 53 54 55 57 15 18
The experimental data in the table was collected during a freezing point depression study where BHT (butylated hydroxytoluene) was the solvent. Mass Mass of BHT of unknown 8.526 g 1.316 g Use this data to calculate the molar mass of the unknown solute. molar mass= 16962 Incorrect psy HW 3.pdf Freezing point of pure BHT 74.60 °C APA Title Page -....doc Freezing point of BHT and unknown solution 71.69 °C PSY Final Project....pdf A K₁ for BHT 6.83 °C/m g/mol SH
A chemist attempts to prepare some very pure crystals of borax by dissolving100g of Na2B4O7 in 200 grams of boiling water. He then cools the solution slowly until some borax crystallizes out. Calculate the grams of borax recovered in the crystals per 100 grams of initial solution (Na2B4O7 plus water), if the residual solution at 55oC after the crystals are removed contains 12.4% Na2B4O7.What is the percent yield or percent recovery of Na2B4O7. Show process diagram and solution.
Calculate freezing temperature Tf and the boiling temperature Tb of a solution formed by mixing 15.6g of magnesium chloride, strong electrolyte with 155g of acetic acid, freezing point in 17.0 Celsius and boiling point of 118 Celsius. the Kf and Kb for the solvent are 3.90 Celsius/m and 3.07 Clesius/m respectively Explain in a paragraph your reasoning of your answer
. Throat spray is used in relieving pain and imritation caused by sore throat, sore mouth, or canker sores. It is composed of a diluted solution of Phenol in water. The mass percent of the usual throat spray is 1.40% C6H5OH in water. The density of the Phenol solution and Water are known to be 0.9956 g/ml and 1.00 g/ml respectively. Calculate the Molarity of the solution.
Determine the appropriate quantity (in terms of volume) of 50 wt.% NaOH solution (Specific gravity: 1.52) that is required to prepare 1 liter 0.1 M NaOH standard solution.
Given these values, find the initial mole fraction and initial mass % of the solute (NaCl) Solvent (water) weight: 200g Solute (NaCl) weight: 39g Solute (NaCl) Molar mass=58.44 moles of solute (NaCl) = .667
In the determination of molar mass of an unknown substance by ebullioscopic constant, 30 mL of acetone (C3H6O) was placed in a test tube with thermometer and glass tubing and subjected to water bath. Upon boiling, the temperature reads 56 degC. For the boiling point of unknown-acetone solution, you prepared the solution by mixing 1.60 g of unknown solute in the 30 mL acetone and subjected it again to water bath. The boiling temperature of the solution is 56.68 degC. The density of acetone = 0.9849 g/mL and the Kb of acetone = 1.67 degC/kg Questions: 1. What is the molal concentration of the solution? 2. What is the value for delta Tb or the change in boiling temperature (in degrees Celsius)? 3. How many moles of solute are present in the solution?