Find the concentration of H+ if pOH of a solution is 11.7.
Well, if the pOH is 11.7, then the concentration of OH- ions must be quite high. So high in fact, that it's the life of the party. But let's not forget about its counterpart, the H+ ion. Since water is neutral, we know that the concentration of H+ ions must be equal to the concentration of OH- ions. So, in this case, the concentration of H+ ions would also be quite high, making it the center of attention just like its party buddy OH-.
To find the concentration of H+, we can use the equation:
pH + pOH = 14
Given that the pOH of the solution is 11.7, we can calculate the pH by subtracting the pOH from 14:
pH = 14 - 11.7
pH = 2.3
The concentration of H+ is related to the pH using the equation:
[H+] = 10^(-pH)
Therefore, the concentration of H+ can be calculated as follows:
[H+] = 10^(-2.3)
To find the concentration of H+ ions, you first need to calculate the concentration of OH- ions in the solution using the pOH value provided.
Step 1: Calculate the concentration of OH- ions using the formula:
OH- concentration = 10^(-pOH)
In this case, the pOH is 11.7, so the OH- concentration can be calculated as follows:
OH- concentration = 10^(-11.7)
Step 2: Calculate the concentration of H+ ions using the equation:
H+ concentration x OH- concentration = 1 x 10^(-14) (for water at 25 degrees Celsius)
Since the concentration of OH- ions has been calculated in Step 1, you can substitute this value into the equation and solve for H+ concentration:
H+ concentration x (10^(-11.7)) = 1 x 10^(-14)
H+ concentration = (1 x 10^(-14)) / (10^(-11.7))
H+ concentration ≈ 2.83 x 10^(-4) M
Therefore, the concentration of H+ ions in the solution is approximately 2.83 x 10^(-4) M.
pH + pOH = 14
You know pOH, solve for pH.
Then pH =-log(H^+). Plug and chug.