ChemistryOld MathJax webviewWhich one of the following is correct forthe sparingly soluble salts?1. The cation plus its negativeatmosphere has less positive charge thanthe cation alone.II. Increasing ionic strength reducesthe attraction between any particularion and promotes dissociation into ions.III. For the average anion, there will bemore cations than anions near it becausecations are attracted to the anion, butanions are repelled.lonic atmospheresSelect one:Cationa. I, II and IIIb. II and IIIc. I and IIId. I and IIe. Only Id+Anion With explainations please am not in hurry (6)Which one of the following is correct forthe sparingly soluble salt solutioncontaining inert soluble salts?1. The cation plus its negativeatmosphere has less positive charge thanthe cation alone.II. Increasing ionic strength reducesthe attraction between any particularion and promotes dissociation into ions.III. For the average anion, there will bemore cations than anions near it becausecations are attracted to the anion, butanions are repelled.lonic atmospheresSelect one:Cationa. I, II and IIIb. II and IIIc. I and IIId. I and IIe. Only ISolve this question please8+Anion

Which one of the following is correct for the sparingly soluble salts? 1. The cation plus its negative atmosphere has less positive charge than the cation alone. II. Increasing ionic strength reduces the attraction between any particular ion and promotes dissociation into ions. III. For the average anion, there will be more cations than anions near it because cations are attracted to the anion, but anions are repelled.

Which one of the following is correct for the sparingly soluble salts? 1. The cation plus its negative atmosphere has less positive charge than the cation alone. II. Increasing ionic strength reduces the attraction between any particular ion and promotes dissociation into ions. III. For the average anion, there will be more cations than anions near it because cations are attracted to the anion, but anions are repelled.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 4P: Figure 16.3 shows the solubility of AgNO3 in water inunits of moles of AgNO3 per kilogram of H2O. If...

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