The pH of 6.0 M KOH is 13.78. What is the hydrogen ion concentration of this solution
pH = -log(H+). Solve for (H^+).
To find the hydrogen ion concentration (H+) of a solution, we can use the equation:
pH = -log10[H+]
In this case, the pH of the solution is 13.78. So let's rearrange the equation to solve for [H+]:
[H+] = 10^(-pH)
[H+] = 10^(-13.78)
Using a calculator, we find that [H+] is approximately 1.58 x 10^(-14) M.
Therefore, the hydrogen ion concentration of the 6.0 M KOH solution is approximately 1.58 x 10^(-14) M.
To find the hydrogen ion concentration of a solution, you can use the formula for pH, which is defined as the negative logarithm of the hydrogen ion concentration:
pH = -log[H+]
Given that the pH of a 6.0 M KOH solution is 13.78, we can use this information to calculate the hydrogen ion concentration.
First, subtract the pH from 14 (since the sum of the pH and pOH of a solution is always 14) to find the pOH:
pOH = 14 - pH
pOH = 14 - 13.78
pOH = 0.22
Next, convert the pOH to OH- concentration using the formula:
pOH = -log[OH-]
OH- concentration = 10^(-pOH)
Substituting the value of pOH into the equation:
OH- concentration = 10^(-0.22)
OH- concentration ≈ 0.6309 M
Since KOH completely dissociates in water to produce OH-, the OH- concentration is also the concentration of the hydroxide ions (OH-) in the solution.
Now, since the hydroxide ion and hydrogen ion (H+) concentrations are equal in a basic solution like KOH, the concentration of H+ can be considered the same as OH-:
H+ concentration ≈ 0.6309 M
Therefore, the hydrogen ion concentration of the given 6.0 M KOH solution is approximately 0.6309 M.