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.