help i. Write the equation for the reaction that forms the few (but important) i

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i. Write the equation for the reaction that forms the few (but important) ions in pure water ii. Why is tap water more conductive than distilled water? ii Is there any evidence that methanol forms ions either in the pure state or when dissolved in water? Would you classify methanol as a strong electrolyte, weak electrolyte, or nonelec- trolyte? Compare your measurements for CHOH(aq), CH,COOH(aq), and HCI(aq). would you classify aqueous acetic acid as a strong electrolyte, weak electrolyte, or nonelectrolyte What species are present in aqueous acetic acid? In glacial acetic acid iv. Species Present CH,COOH(aq) CH,COOH(0) Does sucrose behave like a strong electrolyte, weak electrolyte, or nonelectrolyte when it is dissolved in water? What species are present in C,H,,O(aq) v. vi. The models of solid NaCl describe it as consisting of Na cations and Cl anions. If this is the case, why is NaCI(s) not an electrolyte?

Explanation / Answer

Ans. I. Balanced Reaction: H2O(aq) + H2O(aq) <--------------> H3O+(aq) + OH-(aq)

Autoprotolysis of water produces H3O+ and OH- ions in pure water.

In pure water, [H3O+] = [OH-] = 10-7

#II. Tap water generally consists of various ions like Ca2+, Fe2+, Cl-, SO42- Mg2+ dissolved in it. Moreover, dissolution of atmospheric CO2 in it produces small amount of carbonic acid which further dissociates into bicarbonate ion and proton. That is, the tap water consists of several ions whereas distilled water does not (at least, theoretically). Greater is the number of ions in water, greater is its conductivity because ions conduct charge.

Therefore, presence of relatively larger amount of ions in tap water makes it more conductive that distilled water.

#III. Methanol forms ions when dissolved in water.

Conductivity of pure methanol is extremely lower than its aqueous solution. Higher conductivity (higher than both pure water and pure methanol) of methanol solution in water indicates that methanol undergoes dissociation to form ions in water.

Methanol acts as weak acid. So, the pH of methanol solution must be acidic whereas that of pure water or methanol neutral.

#IV. HCl – HCl is a strong electrolyte because it undergoes complete dissociation when dissolved in water.

CH3COOH (aq) is a weak electrolyte because it undergoes small dissociation when dissolved in water.

CH3COOH(l) or pure acetic acid is nonelectrolyte because it does not undergo significant dissociation in pure form.

#V. When dissolved in water, sucrose acts as nonelectrolyte because it does not dissociates into ions.

The aqueous solution consists of C12H22O11 only but no ions.

#VI. In solid form, the Na+ and Cl- ions remains attached to each other in its lattice structure. There is no free Na+ and Cl- ions in solid form. Therefore, solid NaCl is NOT an electrolyte.

When dissolved in water, the solid NaCl dissolves to form free hydrated Na+(aq) and Cl-(aq) ions.

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