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!

c- cold periods in earth's history during which glaciers covered much of the surface.

explanation:

space exploration has led to the development and technological improvement of many everyday items. (if this answer is wrong i will find the right answer) : )