what is the hydronium ion concentration in a 0.55 M HNO3 solution ? what is the pH of this solution?
Thank You!!!
To determine the hydronium ion concentration in the 0.55 M HNO3 solution, we need to consider that HNO3 is a strong acid that completely ionizes in water. The balanced chemical equation for this reaction is:
HNO3 + H2O → H3O+ + NO3-
Since HNO3 completely ionizes, the concentration of H3O+ will be equal to the concentration of the HNO3 solution. Therefore, the hydronium ion concentration in a 0.55 M HNO3 solution is 0.55 M.
To determine the pH of this solution, we can use the formula:
pH = -log10 [H3O+]
Using the hydronium ion concentration we just found (0.55 M), we can plug it into the formula:
pH = -log10 (0.55)
Calculating this using a calculator, we find:
pH ≈ 0.26
Therefore, the pH of the 0.55 M HNO3 solution is approximately 0.26.
To find the hydronium ion (H3O+) concentration in a 0.55 M HNO3 (nitric acid) solution, you can start by considering the dissociation reaction of nitric acid in water:
HNO3 + H2O -> H3O+ + NO3-
From the equation, you can see that for every 1 mole of HNO3, 1 mole of H3O+ is formed. This means that the concentration of H3O+ ions is the same as the concentration of the HNO3 solution, which in this case is 0.55 M.
Therefore, the hydronium ion concentration in the 0.55 M HNO3 solution is 0.55 M.
Now, to find the pH of the solution, you can use the equation:
pH = -log[H3O+]
Substituting the H3O+ concentration (0.55 M) into the equation:
pH = -log(0.55)
Calculating this using a calculator, we find that the pH of the 0.55 M HNO3 solution is approximately 0.26.
So, the hydronium ion concentration is 0.55 M and the pH is 0.26.