Find the ph of the following solution. 1.2 l of a solution containing 5.0x10^-4 grams of hydrobromic acid.

The HBr is a strong acid, that is, it is fully consumed in the reaction

molar mass HBr = 80.91 g/mol

number of moles = 5.0 x 10⁻⁴ / 80.91 = 6.17 x 10⁻⁶ moles

molarity = 6.17 x 10⁻⁶ / 1.2 = 5.14 x 10⁻⁶ M

HBr  H₃O⁺   +           Br ⁻
↓                                 ↓                     ↓
  5.14 x 10⁻⁶                0                     0
- 5.14 x 10⁻⁶             5.14 x 10⁻⁶   5.14 x 10⁻⁶ 

0                             5.14 x 10⁻⁶ M         5.14 x 10⁻⁶ M

PH = - log [ H₃O⁺ ]

PH = - log [ 5.14 x 10⁻⁶ ]

PH = 5.82