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Oxyacids of Phosphorus

The base of ...

Question

The _____ base of $H S O_{4}^{⊝}$ in aqueous solution is $S O_{4}^{2 -}$ .

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Solution

Reaction involve-
$H S O_{4}^{⊝} + H_{2} O ⟶ S O_{4}^{2 -} + H_{3} O^{+}$
$A c i d$ $C o n j u g a t e b a s e$

Therefore, the $c o n j u g a t e$ base of $H S O_{4}^{⊝}$ in aqueous solution is $S O_{4}^{2 -}$

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H_{2} S O_{4} ⟶ H^{+} + H S O_{4}^{-}

(100% ionisation)

H S O_{4}^{-} ⟶ H^{+} + S O_{4}^{2 -}

(10% ionisation)

The given reaction takes place when sulphuric acid dissolves in water.

If we start with

0.2 M

aqueous solution of

H_{2} S O_{4}

[S O_{4}^{2 -}]

in the above case will be:

Q. The conjugate base of

H S O_{4}^{-}

in an aqueous solution is:

When sulphuric acid dissolves in water, the following reactions take place:

H_{2} S O_{4} ⟶ H^{+} + H S O_{4}^{-}

100 %

H_{2} S O_{4}^{-} ⟶ H^{+} + S O_{4}^{2 -}

10 %

0.2 M

aqueous solution of

H_{2} S O_{4}

[H_{3} O^{+}]

in aqueous solution is:

When sulphuric acid dissolves in water, the following reactions take place:

H_{2} S O_{4} ⟶ H^{+} + H S O_{4}^{-}

100 %

H_{2} S O_{4}^{-} ⟶ H^{+} + S O_{4}^{2 -}

10 %

0.2 M

aqueous solution of

H_{2} S O_{4}

The species that has the maximum concentration is :

Q. The boiling point of a 0.5 molal aqueous solution of

N a H S O_{4}

100.64^{\circ} C

. What is the dissociation constant for the following reaction?

[K_{b} of H_{2} O = 0.512 K k g m o l^{- 1}]

H S O_{4}^{-} ⇌ H^{+} + S O_{4}^{2 -}

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