1,2,3,5,6 please! Are all ionic substances aqueous electrolytes? Are all aqueous
ID: 481945 • Letter: 1
Question
1,2,3,5,6 please!
Are all ionic substances aqueous electrolytes? Are all aqueous electrolytes ionic compounds? What is the effect of the solvent on conductivity? Use your results to classify each substance as strong electrolyte, weak electrolyte, or nonelectrolyte in each solvent tested. Classify each substance as metallic, ionic, or covalent. Classify each substance as acid, base, salt, or other (acid = H^+ anion; base often = cation +OH-; salt = cation other than H^+ + anion other than OH-). Is it possible for a covalent substance to be an electrolyte (strong or weak)? Explain, and give examples. Is it possible for an ionic substance to be a nonelectrolyte? Explain, and give examples.Explanation / Answer
1. Yes all of them are electrolytes, because they mostly break up into ions as they dissolve in water.
2. No, all aqueous electrolytes are not ionic compounds. Acids and a few other molecular compounds such as ammonia, NH3, react with water to form ions and are consequently electrolytes. For example, when HCl(g) dissolves in water to form hydrochloric acid, HCl(aq), it ionizes or breaks apart into H+(aq) and Cl–(aq) ions in solution.
3.The conductivity will depend upon the type of solvent being used.
When electrolytes are dissolved in water (or other polar solvents) they ionize into positive (cation) and negative (anion) ions. Nonpolar substances possess relatively low dielectric constants — chloroform, ether, carbon. Thus, the nonpolar solvents are poor solvents for electrolytes, and hence for conductivity.
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