Question

Which shows weak ionization in water?

• A. $H_2{SO}_4$
• B. ${HNO}_3$
• C. $NaCl$
• D. $HCl$

Answer 1

Answer: (A)

$H_{2}S{O}_4$ has weaker Ionisation in water because dissociation takes place in two steps wherein second step there is no 100% ionisation because $HS{O}_4^{-}$ is weak acid ion:

$1)H_{2}S{O}_4+H_{2}O\to H_3{O}^{+}+HS{O}_4^{-}$

$2)HS{O}_4^{-}+H_{2}O\to H_3{O}^{+}+S{O}_4^{2-}$

NaCl dissociates in one steps :

$NaCl\to N{a}^{+}+C{l}^{-}$

$HN{O}_3\to H^{+}+N{O}_3^{-}$

So, A is correct option