Answer:
HCOOH (formic acid) weak acid
HClO₄ strong acid
HI strong acid
NH₃ weak base
NaOH strong base
HNO₂ weak acid
CH₃COOH (acetic acid) weak acid
(CH₃)₂NH weak base
HNO₃ strong acid
Ca(OH)₂ strong base
HCl strong acid
KOH strong base
HCN weak acid
HF weak acid
CH₃NH₂ weak base
CsOH strong base
HBr strong acid
LiOH strong base
Ba(OH)₂ strong base
H₂SO₄ strong acid
Explanation:
Strong electrolytes are those that <em>completely</em> dissociate in water, so they exist mostly in the ionic form.
AB(aq) ⇒ A⁺(aq) + B⁻(aq)
On the other hand, weak electrolytes dissociate <em>only partially</em> in water, so that at equilibrium there is a mixture of the molecular form and the ionic form.
AB(aq) ⇄ A⁺(aq) + B⁻(aq)
Electrolytes can be acid or basic.
There are 7 strong acids: HCl, HBr, HI, HClO₃, HClO₄, HNO₃ and H₂SO₄. The rest of the acids are weak.
Strong bases are those hydroxides that contain cation from Groups 1 and 2 of the Periodic Table (e.g. NaOH, Ca(OH)₂). The rest of the bases are weak.
NH₃
, (CH₃)₂NH, and CH₃NH₂ are bases, despite not having OH⁻ groups, because they can accept H⁺, according to Bronsted-Lowry acid-base definition.
NH₃ + H₂O ⇄ NH₄⁺ + OH⁻
(CH₃)₂NH + H₂O ⇄ (CH₃)₂NH₂⁺ + OH⁻
CH₃NH₂ + H₂O ⇄ CH₃NH₃⁺ + OH⁻
With this information, we can classify the compounds from the list as a strong acid, strong base, weak acid, or weak base.
