1. Part ASolution temperature =24 °CConductivity of instrument grade water = 1.043 uScm!Conductivity of deionised water = 1.74 µScm!Conductivity of tap water =330 μScmlOn the basis of data above comment on conditions of the different water grades.2. The experimental data for electrolytes in Part B are given below:Electrolytec (M)K (ms.cm')HC10.015.06KCI0.011.415NaCl0.011.236CaCl20.012.30КОН0.012.29CH3OH0.010.003K2SO40.012.65Calculate molar conductivity A of each electrolyte solution in Sm/mol above. Correct for theconductivity of deionized water.

Answered: Image /qna-images/answer/f9cd7737-d0d7-4a0f-9842-bec5d3d59750.jpg

Answered: 1. Part A Solution temperature = 24 °C…

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 CHM 126 student performed the "Determination of Molar Mass by Freezing Point Depression" experiment. He started the experiment by measuring the mass and freezing point of the pure solvent with minimal error. Instead of quickly finishing the experiment, he took a lunch break. After returning from lunch, he noted that the solvent had absorbed some impurities from the atmosphere. He went ahead and performed the rest of the experiment anyway. Assuming a negligible (very minor) change in the mass of the solvent after absorbing impurities, which of the following choices contains only correct statements: because of the experimental error, the measured ATwill increase, the measured molality will increase, and the measured molar mass will contain no additional error because of the experimental error, the measured ATwill decrease, the measured molality will decrease, and the measured molar mass will decrease because of the experimental error, the measured ATwill decrease, the measured molality…
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Q 7 please

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