Ethanol, CH_3CH_2OH, is a nonelectrolyte; acetic acid, HC_2H_3O_2, is a weak ele

Question

Ethanol, CH_3CH_2OH, is a nonelectrolyte; acetic acid, HC_2H_3O_2, is a weak electrolyte; and aluminum chloride, AlCl_3, is a strong electrolyte. What are the solute particles present in aqueous solutions of each compound? (Select all that apply.) ethanol O^2- OH^- CH_3CH_3OH_2^+ CH_3CH_2OH H^+ acetic acid O^2+ H^+ HC_2H_3O^2+ C_2H_3O_2^- HC_2H_3O_2 OH^- aluminum chloride AlCl_3 Al^3+ Cl^3- HAlCl_3^+ Al^+ Cl^- If 0.1 mol of each compound is dissolved in solution, which one contains about 0.4 mol of solute particles, which contains 0.1 mol of solute particles, and which contains somewhere between 0.1 and 0.2 mol of solute particles?

Explanation / Answer

In the first part, the best way is to put the reaction so we can see the disolution:

For ethanol:
CH3CH2OH(l) ---------> CH3CH2OH(aq)

For AlCl3:
AlCl3 ---------> Al3+ + 3Cl-

For acetic acid:
CH3COOH ---------> CH3COO- + H+

This would answer your first question of the particles in solution.

For your second question, and basing on the previous reactions, we can say that AlCl3 would have 0.4 mol (3*0.1 + 0.1 = 0.4)
Ethanol would be 0.1 particles.
Acetic acid will have between 0.1 and 0.2 mol particles.

Hope this helps

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