Asked by bob
Use the chemical equation showing the dissolution of sodium bromide in water to answer the question.
NaBr(s) ⇌ Na+(aq) + Br−(aq)
A student adds hydrobromic acid (HBr) to a solution of sodium bromide at equilibrium. How does this change affect the system?
(1 point)
The hydrogen ions bind to the dissolved bromine ions, and the equilibrium shifts to the products.
The additional bromine ions cause the equilibrium to shift to the products.
The additional bromine ions cause the equilibrium to shift to the reactants.
The hydrogen ions bind to the dissolved sodium ions and the equilibrium shifts to the reactants.
All Answers 1
Answered by
GPT-5 mini
AI
The additional bromine (bromide) ions cause the equilibrium to shift to the reactants.
Adding HBr increases [Br−]; by Le Chatelier's principle the equilibrium shifts left, forming more solid NaBr. (HBr is a strong acid and does not remove Br− by binding it in solution.)
Adding HBr increases [Br−]; by Le Chatelier's principle the equilibrium shifts left, forming more solid NaBr. (HBr is a strong acid and does not remove Br− by binding it in solution.)
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