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arsen [322]
3 years ago
15

The acid-dissociation constants of sulfurous acid (h2so3) are kal = 1.7 × 10-2 and ka2 = 6.4 × 10-8 at 25.0°c. calculate the ph

of a 0.163 m aqueous solution of sulfurous acid.
Chemistry
2 answers:
stira [4]3 years ago
7 0

Constructing the ICE table for acid-dissociation  of sulfurous acid

 H₂SO₃ --> H⁺ + HSO₃⁻

I    0.163 M      0        0

C     - x           + x       + x

E   0.163 - x    + x       + x

Writing the acid dissociation expression  of sulfurous acid,

Kₐ = [H⁺ ][ HSO₃⁻]/ [H₂SO₃]

Plugging in the values we get,

\frac{x²}{(0.163 - x)} = 1.7 x 10⁻²

Since 1.7 x 10⁻² is small we can ignore x in the denominator,

\frac{x²}{0.163}  = 1.7 x 10⁻²

x = 0.052640 M  

pH = 1.28  

Thus the pH of a 0.163 M aqueous solution of sulfurous acid is 1.28.

nignag [31]3 years ago
3 0

<span>Given:

acid-dissociation constants of sulfurous acid</span>:

Ka1 = 1.7 * 10^(-2)

Ka2 = 6.4 * 10^(-8) at 25.0 °C. 

aqueous solution of sulfurous acid = 0.163 M

 

x² / (0.163 - x) = 1.7 * 10^(-2) 

You simplify it to:

<span>x² / (0.163) = 1.7  *10^(-2) </span>

x = 0.052640 M 

pH = 1.28 

<span>
So, the pH of a 0.163 M aqueous solution of sulfurous acid is 1.28.</span>

 

To add, aqueous solutions of sulfur dioxide purpose are as disinfectants and reductant, as are solutions of sulfite<span> salts and </span>bisulfite. By accepting another oxygen<span> atom, they are </span>oxidised to sulfuric acid or sulfate.

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