HF dissociates slightly in water. It is?

Question

HF dissociates slightly in water. It is?
1. a strong electrolyte
2. a weak electrolyte
3. a nonelectrolyte
4. an unknown kind of electrolyte

Answer 1

2 weak electrolyte

Answer 2

Compounds that form ions in water (dissociate) cause the water to conduct electricity (then they are called electrolytes).

How well the water conducts electricity depends on how much the compound dissociates (comes apart into ions). Compounds where all or almost all of the compound dissociates are called strong electroyles because the water will conduct a lot.

Compounds that only dissociate just a little bit (but do dissociate) are called weak electrolytes because the water conducts just a little.

Compounds that don't dissociate at all are called nonelectrolytes.

That makes the HF a weak electrolyte since it dissociates a little.

Answer 3

because of its low tendency to dissociate to ions in water, therefore, HF is a weak electrolyte in aqueous solution. ...

First, we recognize HF as an acid; it can donate H+. It is not one of the six 'strong acids' (do you remember those by name and formula?); therefore, HF is a weak electrolyte in aqueous solution. It ionizes only partially, so that HF is in equilibrium with H+(aq) and F-(aq) ions.

Answer 4

It is a weak electrolyte.

Answer 5

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