Calculate the pH of a 7. 75x10^-12 M Hydrobromic acid solution.


pH= __________ (round to 4 sig figs)


This solution is _________(acidic/basic).


(30 points)

Answers

Answer 1

To calculate the pH of a 7.75x10^-12 M Hydrobromic acid (HBr) solution, we need to first write the dissociation equation for HBr in water:

HBr + H2O → H3O+ + Br-

The equilibrium constant expression for this reaction is:

Ka = [H3O+][Br-]/[HBr]

Since we know the concentration of HBr, we can use the value of Ka to calculate the concentration of H3O+ in the solution, which will then give us the pH. The value of Ka for HBr is 8.7x10^-9.

Let x be the concentration of H3O+ in the solution. Then, we can write:

8.7x10^-9 = x^2/7.75x10^-12

Solving for x, we get:

x = 2.6x10^-6 M

Therefore, the pH of the solution is:

pH = -log[H3O+] = -log(2.6x10^-6) = 5.59

Since the pH is less than 7, the solution is acidic.

Therefore, the pH of the 7.75x10^-12 M Hydrobromic acid solution is 5.59 and the solution is acidic.

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