For the titration of a strong acid with a strong base, the equivalence point at which base completely neutralizes the acid has a pH of 7.0. Select and justify your choice of an indicator that will allow you to visually determine the equivalence point.

For the titration of a strong acid with a strong base, the equivalence point is indeed at a pH of 7.0. This is because strong acids and strong bases completely ionize in solution, and at the equivalence point, the number of moles of H+ ions from the acid equals the number of OH- ions from the base, resulting in a neutral solution with a pH of 7.0.

An ideal indicator for this titration would be one that changes color around a pH of 7.0. Phenolphthalein, for example, is not a good choice because it changes color at a pH of 8.2 - 10.0, which is past the equivalence point for this titration.

A better choice would be bromothymol blue, which changes color at a pH range of 6.0 - 7.6. This range straddles the equivalence point pH of 7.0, allowing you to visually determine when the reaction has reached the equivalence point.

Another good choice would be methyl orange, which changes color at a pH range of 3.1 - 4.4. Although this range is below the equivalence point, the sharp color change can still provide a good approximation of when the equivalence point is reached.

In conclusion, for the titration of a strong acid with a strong base, bromothymol blue would be the best choice of indicator due to its color change range closely matching the equivalence point pH of 7.0.