What is the approximate pH of a solution labeled 6 x 10^-5 M HBr?

4.2 thank you so much do u have time for another one?

4.2

pH = -log(6 x 10^-5) = ??

Oh, now that's a tough one! Let me think... Hmmm... Ah, got it! The pH of the HBr solution is approximately "acidic". Just kidding! The approximate pH of a solution labeled 6 x 10^-5 M HBr is around 4.22. Hope that helps, and remember, laughter is the best pH-adjuster!

To determine the approximate pH of a solution labeled as 6 x 10^-5 M HBr, we need to use the fact that HBr is a strong acid and it fully dissociates in water. HBr dissociates into H+ (hydrogen ions) and Br- (bromide ions). The concentration of H+ ions will determine the pH of the solution.

The concentration of HBr is given as 6 x 10^-5 M. Since HBr fully dissociates, the concentration of H+ ions is also 6 x 10^-5 M.

pH is a measure of the acidity or alkalinity of an aqueous solution. It is defined as the negative logarithm (base 10) of the concentration of H+ ions.

To calculate the pH, we can take the negative logarithm of the H+ concentration:
pH = -log[H+]

Therefore, pH = -log(6 x 10^-5)
Using logarithm properties, we can rearrange this equation to simplify the calculation:
pH = -log6 -log(10^-5)

The logarithm of 10^-5 is -5, so the equation becomes:
pH = -log6 + 5

Now we can calculate the pH using a calculator or logarithm table:
pH ≈ -0.778 + 5
pH ≈ 4.222

Therefore, the approximate pH of the solution labeled 6 x 10^-5 M HBr is approximately 4.222.

9.8 or 9.9

9.8