Explain why the dissociation of a weak acid can be ignored when calculating the pH of a solution that contains both a weak acid and a strong acid. The ion from the strong acid is a common ion in the dissociation reaction of the weak acid. Consequently, it shifts the equilibrium back toward the which the dissociation of the to the point where the amount of ion that it produces is negligible

The answer is in the explanation.

Explanation:

The dissociation of a weak acid consist in the following equilibrium:

HX ⇄ H⁺ + X⁻

Where Ka is defined as:

Ka =  [H⁺] [X⁻] / [HX]

A strong acid (HY) dissociates completely in water, thus:

HY → H⁺ + Y⁻

As the strong acid produces H⁺, in the equilibrium, the reaction shifts to the left -The undissociated form-, reducing the production of H⁺, allowing ignore the dissociation of the weak acid when calculating the pH.

Higher, this is because Hydrogen is inheretly positive and as a cation produces very high polarity in the molecule. This only works for molecules with hydrogen + any of the following elements:
Oxygen,
Nitrogen,
Flourine