Final answer:
The solute in the .1M aqueous solution is likely HBr (hydrobromic acid) because it is a strong acid that conducts electricity, turns blue litmus red, and reacts with zinc to produce hydrogen gas bubbles.
Step-by-step explanation:
The student is testing a .1M aqueous solution and observed that it conducts electricity, turns blue litmus red (indicating that the solution is acidic), and reacts with zinc to produce bubbles (which typically indicates hydrogen gas production characteristic of acid-metal reactions). Given these observations, the likely compound in the solution is an acid.
Option 1, CH3OH (methanol), is not acidic enough to exhibit the observed behaviours. Option 2, LiBr, is a salt and would not turn litmus paper red. Option 4, LiOH, is a strong base and would turn red litmus paper blue, not blue litmus paper red. Therefore, option 3, HBr (hydrobromic acid), is the best answer because it is a strong acid and will conduct electricity effectively, turn blue litmus paper red, and react with zinc to release hydrogen gas bubbles.
An aqueous solution of HBr conducts electricity well due to the presence of mobile ions, which is consistent with it being a strong electrolyte. The fact that it turns blue litmus to red confirms its acidic nature. Lastly, the reaction with zinc is characteristic of acids, which produce hydrogen gas when reacting with active metals. Therefore, HBr satisfies all the given observations and is the correct answer to the question.