What is the concentration of hydronium ions in a solution that is 0.12 M HBrO(aq) and 0.160 M NaBrO(aq)?
To determine the concentration of hydronium ions in the solution, we need to consider the dissociation of HBrO.
The balanced equation for the dissociation of HBrO is:
HBrO(aq) ⇌ H+(aq) + BrO-(aq)
From the stoichiometry of the equation, we can see that for every 1 mole of HBrO that dissociates, 1 mole of H+ (hydronium ions) is produced. Therefore, the concentration of H+ (hydronium ions) is equal to the concentration of HBrO.
Given that [HBrO] = 0.12 M, the concentration of hydronium ions in the solution is also 0.12 M.
To find the concentration of hydronium ions in the solution, we need to consider the dissociation of the acid, HBrO.
The balanced equation for the dissociation of HBrO in water is as follows:
HBrO(aq) ⇌ H+(aq) + BrO-(aq)
From the balanced equation, we can see that one HBrO molecule dissociates to produce one hydronium ion (H+) and one hypobromite ion (BrO-).
Now, we'll calculate the concentration of hydronium ions:
Given:
[HBrO] = 0.12 M (concentration of HBrO)
[NaBrO] = 0.160 M (concentration of NaBrO)
Since HBrO dissociates to form H+ and BrO-, the initial concentration of H+ ions is equal to the concentration of HBrO. Therefore, [H+] = 0.12 M.
Hence, the concentration of hydronium ions in the solution is 0.12 M.