Final answer:
The initial pH of the 37.0 ml sample of 0.170 M HBr, which is a strong acid, is calculated to be approximately 0.77 by using the formula pH = -log[H+].
Step-by-step explanation:
The student asks to determine the initial pH in the titration of a 37.0 ml sample of 0.170 M HBr with 0.200 M KOH. Since HBr is a strong acid, we can assume it completely dissociates in water. Hence, the initial concentration of H+ ions is equal to the initial concentration of HBr.
The initial pH of the solution can be calculated using the formula pH = -log[H+], where [H+] represents the concentration of hydrogen ions. Plugging the initial concentration of HBr into the formula gives us:
pH = -log(0.170 M) = 0.77
Therefore, the initial pH of the 37.0 ml sample of 0.170 M HBr is approximately 0.77.