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?
The hydrogen ions bind to the dissolved sodium ions and the equilibrium shifts to the reactants.
The additional bromine ions cause the equilibrium to shift to the reactants.
The additional bromine ions cause the equilibrium to shift to the products.
The hydrogen ions bind to the dissolved bromine ions, and the equilibrium shifts to the products.
For Honers,
1. A system is at equilibrium. Which statement is correct?
->The rate of the forward reaction equals the rate of the reverse reaction.
2. H2O(l) + heat ⇄ H2O(g) A sample of water is at equilibrium at 100°C. Which statement best describes what will happen if liquid water is added to the system?
->More liquid water molecules will change to water vapor until a new equilibrium is reached.
3. Co(H2O)62+ + 4Cl– + heat ⇄ CoCl42– + 6H2O Cobalt ions form complex ions with water and chloride. The Co(H2O)62+ ions are pink, and the CoCl42– ions are blue. A scientist creates a solution that is purple at equilibrium. How can the scientist make the solution more pink?
->By adding water (H2O)
4. It is the above question, which is correct
5. A copper complex reacts with ammonia according to the following reaction, where the left side of the reaction is a pale sky-blue color and the right side is dark blue.
Cu(H2O)42+(aq) + 4NH3(aq) ⇄ Cu(NH3)42+(aq) + 4H2O(aq)
Which change to a solution at equilibrium will make the solution darker?
->Removing water (H2O)
The answer is "The additional bromine ions cause the equilibrium to shift to the reactants."
Anonymous is correct thank you!
To answer the question, we need to understand how the addition of hydrobromic acid (HBr) affects the equilibrium system of sodium bromide dissolution in water.
The chemical equation provided shows the dissolution of sodium bromide (NaBr) in water, resulting in the formation of sodium ions (Na+) and bromide ions (Br-). This implies that sodium bromide is in equilibrium with its ions in the solution.
When hydrobromic acid (HBr) is added, it dissociates in water, releasing hydrogen ions (H+) and bromide ions (Br-). These additional bromide ions can affect the equilibrium by changing the concentration of bromide ions in the solution.
In this case, the additional bromine ions cause the equilibrium to shift to the products. This means that more sodium ions and bromide ions will be produced, favoring the right side of the equation. The reason for this shift is the Le Chatelier's principle, which states that if a system at equilibrium is subjected to a stress (in this case, the addition of bromide ions), it will adjust to counteract the effect of the stress.
Therefore, the correct answer is: The additional bromine ions cause the equilibrium to shift to the products.