pH = 3.89
calculate concentration of hydronium ion and hydroxide ion in solution.
pH = -log(H3O^+); solve for H3O^+.
Then (H3O^+)(OH^-) = Kw = 1E-14. You know Kw and H3O^+, solve for OH^-
Calculate the PH of 0.025moldm3 trioxonitrate(v) solution.
To calculate the concentration of hydronium ion (H3O+) and hydroxide ion (OH-) in a solution given the pH, we can use the following equations:
pH = -log[H3O+]
pOH = -log[OH-]
pH + pOH = 14
1. Calculate the concentration of hydronium ion (H3O+):
pH = -log[H3O+]
Rearranging the formula:
[H3O+] = 10^(-pH)
[H3O+] = 10^(-3.89)
[H3O+] = 1.31 x 10^(-4) M (mol/L)
2. Calculate the concentration of hydroxide ion (OH-):
pOH = 14 - pH
pOH = 14 - 3.89
pOH = 10.11
[OH-] = 10^(-pOH)
[OH-] = 10^(-10.11)
[OH-] = 7.08 x 10^(-11) M (mol/L)
Therefore, the concentration of hydronium ion (H3O+) is 1.31 x 10^(-4) M and the concentration of hydroxide ion (OH-) is 7.08 x 10^(-11) M in the given solution.
To calculate the concentrations of hydronium ion (H3O+) and hydroxide ion (OH-) in a solution based on its pH, you can use the concept of the pH scale and the autoionization of water.
The pH scale is a measure of the acidity or alkalinity of a solution and ranges from 0 to 14. A pH of 7 is considered neutral, pH less than 7 indicates acidity, and pH greater than 7 indicates alkalinity. In a neutral solution, the concentration of hydronium ions (H3O+) is equal to the concentration of hydroxide ions (OH-).
The pH of the solution you provided is 3.89, which indicates acidity. Therefore, the concentration of hydronium ions will be higher than the concentration of hydroxide ions.
To determine the concentrations of H3O+ and OH- from pH, you can use the following equations:
pH = -log[H3O+]
pOH = -log[OH-]
By rearranging these equations, you can solve for the concentrations [H3O+] and [OH-]:
[H3O+] = 10^(-pH)
[OH-] = 10^(14 - pH - pOH)
In a neutral solution, the pH and pOH would be equal, and both would have a value of 7.
Let's calculate the concentrations of H3O+ and OH- using the given pH value of 3.89:
[H3O+] = 10^(-pH) = 10^(-3.89) = 1.26 x 10^(-4) M (rounded to four significant figures)
[OH-] = 10^(14 - pH - pOH)
Since we know the pH (3.89), and in a neutral solution, pH = pOH, we can substitute these values into the equation:
[OH-] = 10^(14 - 3.89 - 3.89) = 5.31 x 10^(-11) M (rounded to four significant figures)
Therefore, the concentration of hydronium ions ([H3O+]) in the solution is approximately 1.26 x 10^(-4) M, and the concentration of hydroxide ions ([OH-]) is approximately 5.31 x 10^(-11) M.