The scatter plot below shows the density of ethylene glycol solutions vs. the mass % of those solutions. Density (g/mL) 1.04+ 1.03 1.02 1.01 0.99- 0.98- 12 14 16 % Mass% Q The equation for the line of best fit shown on the scatter plot is y= 0.001683 +0.9959. Use the equation of the trendline to determine the mass percent of an ethylene glycol solution with a densit- of 1.015 g/mL.

The scatter plot below shows the density of ethylene glycol solutions vs. the mass % of those solutions. Density (g/mL) 1.04+ 1.03 1.02 1.01 0.99- 0.98- 12 14 16 % Mass% Q The equation for the line of best fit shown on the scatter plot is y= 0.001683 +0.9959. Use the equation of the trendline to determine the mass percent of an ethylene glycol solution with a densit- of 1.015 g/mL.

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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The molal freezing point depression constant K,=2.88 °C•kg•mol 'for a certain substance X. When 4.138 g of urea (NH),CO) are dissolved in 100. g of X, the solution freezes at 1.1 °C. Calculate the freezing point of pure X. Round your answer to 2 significant digits. Check Explanation C2022 McGraw Hill LLC. All Rights Reserved Terms of Use Pmvacy Center Accessibility tv
Boiling Point Elevation/Freezing Point DepressionT = m KWhere: 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 note that ΔT as defined above will be a negative number for freezing point depression. Therefore, Kf must also be given as a negative number.
To 500 g of K2Cr207 solution with a mass fraction K2Cr20, 5% added 300g of water. Determine the mass fraction of K2Cr207 in the resulting solution а. 32,5 % b. 10.91 % с. 8.76 % d. 1.107 % е. 3.125 %
TRUE or FALSE. Extraction is attained when the solute is completely dissolved and the concentration of the solution so formed is uniform. The concentration of the liquid retained by the solid leaving any stage is the same as that of the liquid overflow from the same stage.
120=233k×5 Find the value of k.
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
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Quinine is a natural product extracted from the bark of the cinchona tree, which is native to South America. Quinine is used as an antimalarial agent. When 1.90 g of quinine is dissolved in 25.0 g of cyclohexane, the freezing point of the solution is lowered by 4.88 °C. Look up the freezing point and Kf constant for cyclohexane in the Colligative Constants table. Calculate the molar mass of quinine. molar mass: g/mol
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