A glass cup of juice is found to have poH of 11.40.Calculate the concentration of the hydrogen ions in the juice
To calculate the concentration of hydrogen ions (H+), we need to determine the concentration of hydroxide ions (OH-) first, as they are involved in the pH calculation.
The pOH is given as 11.40. We can convert this to [OH-] concentration using the formula: pOH = -log[OH-]
Therefore, we have: 11.40 = -log[OH-]
To find [OH-], we can use the inverse logarithm (antilog) of the pOH value: [OH-] = 10^(-pOH)
Substituting the value, we get: [OH-] = 10^(-11.40)
Calculating this using a calculator, we find that [OH-] is approximately 3.98 x 10^(-12) mol/L.
Since water is neutral, the concentration of hydrogen ions (H+) is equal to the concentration of hydroxide ions (OH-) in pure water, which is 1 x 10^(-7) mol/L.
Now, we can use the relation between [H+] and [OH-] to calculate the concentration of hydrogen ions.
[H+] x [OH-] = 1 x 10^(-14) mol^2/L^2 (at 25 degrees Celsius)
Substituting the values, we get: [H+] x (3.98 x 10^(-12) mol/L) = 1 x 10^(-14) mol^2/L^2
Solving for [H+], we find: [H+] = (1 x 10^(-14) mol^2/L^2) / (3.98 x 10^(-12) mol/L)
Simplifying this expression, we get: [H+] ≈ 2.51 x 10^(-3) mol/L
Therefore, the concentration of hydrogen ions (H+) in the juice is approximately 2.51 x 10^(-3) mol/L.
To calculate the concentration of hydrogen ions (H+) in a solution, we can use the formula:
[H+] = 10^(-pH)
Given that the poH of the juice is 11.40, we can use the formula to calculate the concentration of hydrogen ions.
[H+] = 10^(-11.40)
To solve this equation, simply take 10 raised to the power of -11.40:
[H+] = 0.00000000004
Therefore, the concentration of hydrogen ions in the juice is 0.00000000004 M (moles per liter).
Convert pOH to pH.
pH + pOH = pKw = 14
pH = 14 - 11.40 = ?
Then pH = - log (H^+)
(H^+) = ?