7.25 Why is K K a a 2 1 ? for H₂SO₄ in water? 

7.25

H₂SO₄ is dibasic acid (two replacable H⁺ ions) . In aqueous solution it dissociates in two steps as follows:

H2SO4 + H2O H3O+ + HSO4	(Ka1 = very large)
HSO4 + H2O H3O+ + SO42	(Ka2 = 1.2 x 10–2)

The formula for dissociation constants are:

The neutral H₂SO₄ molecule has more tendency to lose a proton (H⁺) than the Lowry-Bronsted base (which can donate electron i.e. accept a proton H⁺) HSO ^-.

This is because a neutral has a much higher tendency to lose a proton than the negatively charged. Thus, the former is a much stronger acid than the latter.

<p><strong>7.25 </strong></p><p>H₂SO₄ is dibasic acid (two replacable H⁺ ions) . In aqueous solution it dissociates in two steps as follows:</p><table><tbody><tr><td width="287"><p>H₂SO₄ + H₂O H₃O⁺ + HSO₄</p></td><td width="186"><p> (K_a1 = very large)</p></td></tr><tr><td width="287"><p>HSO₄ + H₂O H₃O⁺ + SO₄²</p></td><td width="186"><p> (K_a2 = 1.2 x 10^–2)</p></td></tr></tbody></table><p>The formula for dissociation constants are:</p><div><div><picture><source srcset="https://images.shiksha.com/mediadata/images/articles/1688024577phpo736pf_480x360.jpeg" media=" (max-width: 500px)"><img src="https://images.shiksha.com/mediadata/images/articles/1688024577phpo736pf.jpeg" alt="" width="225" height="127"></picture></div></div><p>The neutral H₂SO₄ molecule has more tendency to lose a proton (H⁺) than the Lowry-Bronsted base (which can donate electron i.e. accept a proton H⁺) HSO ^-.</p><p>This is because a neutral has a much higher tendency to lose a proton than the negatively charged. Thus, the former is a much stronger acid than the latter.</p>

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