Determine the hydronium ion concentration
in a solution that is 0.00027 M HCl.
Answer in units of M.
Determine the hydroxide ion concentration in
a solution that is 0.00027 M HCl.
Answer in units of M.
This is a two part question and I have tried multiple times and every time I try a new answer it's wrong. Can someone help me please! Thanks in advance!
To determine the hydronium ion (H3O+) concentration in a solution, you need to know the initial concentration of the acid and the stoichiometry of the acid's dissociation reaction. In the case of hydrochloric acid (HCl), it is a strong acid that dissociates completely in water.
The balanced chemical equation for the dissociation of HCl is:
HCl(aq) → H+(aq) + Cl-(aq)
From this equation, you can see that one mole of HCl yields one mole of H3O+ ions. Therefore, for a 0.00027 M HCl solution, the concentration of H3O+ ions will be the same as the concentration of HCl.
So, the hydronium ion concentration in a 0.00027 M HCl solution is 0.00027 M.
Now, let's move on to the second part of the question. To determine the hydroxide ion (OH-) concentration in a solution, you need to consider the fact that HCl is a strong acid and does not contribute significantly to the hydroxide ion concentration.
In other words, the hydroxide ion concentration in a HCl solution will be very low or negligible. Therefore, the hydroxide ion concentration in a 0.00027 M HCl solution can be considered as essentially 0 M.
In summary:
Hydronium ion concentration in a 0.00027 M HCl solution = 0.00027 M
Hydroxide ion concentration in a 0.00027 M HCl solution ≈ 0 M
If you had posted your work I wouldn't have to guess what you did.
M HCl = 2.7E-4
pH = -log(HCl) since HCl is a strong acid and ionizes 100%.
Then (H^+)(OH^-) = Kw = 1E-14