The reaction between barium hydroxide and hydrobromic acid produces
a a molecular compound and a weak electrolyte
b two strong electrolytes
c two molecular compounds
d two weak electrolytes
e a molecular compound and a strong electrolyte
The correct answer and explanation is :
The correct answer is:
(e) a molecular compound and a strong electrolyte
Explanation:
When barium hydroxide (\text{Ba(OH)}_2) reacts with hydrobromic acid (\text{HBr}), the reaction follows a classic acid-base neutralization pattern:
[
\text{Ba(OH)}_2 + 2\text{HBr} \rightarrow \text{BaBr}_2 + 2\text{H}_2\text{O}
]
Breaking it down:
- Reactants:
- Barium hydroxide ((\text{Ba(OH)}_2)) is a strong base because it completely dissociates in water into (\text{Ba}^{2+}) and (\text{OH}^-) ions.
- Hydrobromic acid ((\text{HBr})) is a strong acid, meaning it fully ionizes in water into (\text{H}^+) and (\text{Br}^-) ions.
- Products:
- Barium bromide ((\text{BaBr}_2)) is a strong electrolyte because it is an ionic compound that dissolves completely in water, releasing (\text{Ba}^{2+}) and (\text{Br}^-) ions.
- Water ((\text{H}_2\text{O})) is a molecular compound, meaning it consists of covalently bonded atoms and does not ionize significantly in solution.
Thus, the reaction results in a molecular compound (water) and a strong electrolyte (barium bromide).
Why Other Options Are Incorrect:
- (a) A molecular compound and a weak electrolyte → Incorrect because (\text{BaBr}_2) is a strong electrolyte, not a weak one.
- (b) Two strong electrolytes → Incorrect because water is not an electrolyte; it is a neutral molecular compound.
- (c) Two molecular compounds → Incorrect because (\text{BaBr}_2) is an ionic compound, not a molecular one.
- (d) Two weak electrolytes → Incorrect because both (\text{HBr}) and (\text{Ba(OH)}_2) are strong electrolytes.
Hence, option (e) is the correct answer.