Which of the following statement/s is/are TRUE? I. The Arrhenius Theory cannot be applied to account for the behavior of the molar conductivity of strong electrolytes, since these solutes are completely dissociated, at least in dilute solutions. II. Debye=Huckel Theory of interionic attraction satisfactorily explains the variation of the molecular conductivity of strong electrolytes with concentration. II. The ions interact with the solvent molecules through dipole-dipole interaction. IV. When an electric potential is applied across the solution, the ions migrate and the ionic atmosphere around these ions is modified. O , II, II O I, II, IV O I,I O , II O ,1I, IV

Which of the following statement/s is/are TRUE? I. The Arrhenius Theory cannot be applied to account for the behavior of the molar conductivity of strong electrolytes, since these solutes are completely dissociated, at least in dilute solutions. II. Debye=Huckel Theory of interionic attraction satisfactorily explains the variation of the molecular conductivity of strong electrolytes with concentration. II. The ions interact with the solvent molecules through dipole-dipole interaction. IV. When an electric potential is applied across the solution, the ions migrate and the ionic atmosphere around these ions is modified. O , II, II O I, II, IV O I,I O , II O ,1I, IV

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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Which of the following statement/s is/are TRUE? The Arrhenius Theory cannot be applied to account for the behavior of the molar conductivity of strong electrolytes, since these solutes are completely dissociated, at least in dilute solutions. Debye=Huckel Theory of interionic attraction satisfactorily explains the variation of the molecular conductivity of strong electrolytes with concentration. The ions interact with the solvent molecules through dipole-dipole interaction. When an electric potential is applied across the solution, the ions migrate and the ionic atmosphere around these ions is modified. I, II, IV I, III II, III, IV I, II I, II, III
Which of the following statement/s is/are TRUE? The Arrhenius Theory cannot be applied to account for the behavior of the molar conductivity of strong electrolytes, since these solutes are completely dissociated, at least in dilute solutions. Debye=Huckel Theory of interionic attraction satisfactorily explains the variation of the molecular conductivity of strong electrolytes with concentration. The ions interact with the solvent molecules through dipole-dipole interaction. When an electric potential is applied across the solution, the ions migrate and the ionic atmosphere around these ions is modified.
what is molar conductivity? what are its units?
The molar conductivities of 0.01 M solution of sodium chloride, potassium chloride and potassium sulfate are 126.5, 149.9 and 153.3 Scm² mol⁻¹ respectively. The molar conductivity for sodium sulfate is
Asample of 2.05 g of polystyrene of uniform polymer chain length was dissolved in enough toluene to form 0.100 Lofsolution. The osmotic pressure of this solution was found to be 1.21 kPa at 25°C. Calculate the molar mass of thepolystyrene.a) 2.35 x 104 g/molb) 4.20x 105 g/molc) 3.05 105 g/mold) 4.20x 103 g/mole) 4.20 x 104 g/mol
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Two liquids, A and B, show partial miscibility below 52.4 °C. The critical concentration at the upper critical temperature is x = 0.459, where x is the mole fraction of A. At 40.0 °C the two solutions in equilibrium havex = 0.22 and x = 0.60, respectively, and at 42.5 °C the mole fractions are 0.24 and 0.48. Sketch the phase diagram. Describe the phase changes that occur when B is added to a fixed amount of A at (i) 48 °C, (ii) 52.4 °C.
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True or False For strong electrolytes, such as hydrochloric acid, the molar conductivity decreases slightly as the concentration is increased.
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