Calculate the pH in a solution prepared by continuously bubbling SO2 at a pressure of 0.500 atm into pure water.

The pH in a solution prepared by continuously bubbling SO₂ is 1.03.

Explanation:

Searching in google the reaction is:

SO₂(g) + H₂O(l) ⇄ H₂SO₃(ac)    K = 1.33

The constant is:

Having that K = 1.33 and P(SO₂) = 0.500 atm, the concentration of H₂SO₃ is:

Now, we have the following dissociation of H₂SO₃ in water:

H₂SO₃(ac) + H₂O(l) ⇄ HSO₃⁻(ac) + H₃O⁺(ac)   Ka₁ = 1.5x10⁻²

0.665-x                         x                    x

Solving the above equation for x we have:

x = 0.093 = [H₃O⁺] = [HSO₃⁻]

Also, the HSO₃⁻ dissociates in water as follows:

HSO₃⁻(c) +  H₂O(l) ⇄ SO₃²⁻(ac) + H₃O⁺(ac)  Ka₂ = 6.3x10⁻⁸

0.093-y                        y                0.093+y  

Solving the above equation for y we have:

y = 6.3x10⁻⁸

So, the concentration of H₃O⁺ is:

Finally, the pH is:

Therefore, the pH in a solution prepared by continuously bubbling SO₂ is 1.03.

I hope it helps you!

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i