What is the H+ concentration for an aqueous solution with pOH = 4.13 at 25 ?
pH + pOH = pKw = 14
To find the H+ concentration (also known as the concentration of hydronium ions) for an aqueous solution with a given pOH, you can use the following equation:
pOH = -log[OH-]
Since pOH and OH- are related, you can also use this equation to find the concentration of OH-:
[OH-] = 10^(-pOH)
At 25°C, the equation relating the concentrations of H+ and OH- is:
Kw = [H+][OH-] = 1.0 x 10^-14
where Kw is the ion product of water.
To find the H+ concentration, you can rearrange this equation as follows:
[H+] = Kw / [OH-]
Given pOH = 4.13, we can calculate the OH- concentration:
[OH-] = 10^(-pOH)
= 10^(-4.13)
Using a scientific calculator, we can find that [OH-] is approximately 7.52 x 10^(-5) M.
Now, we can substitute the value of [OH-] into the equation for [H+] to find the H+ concentration:
[H+] = Kw / [OH-]
= (1.0 x 10^-14) / (7.52 x 10^(-5))
≈ 1.33 x 10^(-10) M
Therefore, the H+ concentration for the aqueous solution with a pOH of 4.13 is approximately 1.33 x 10^(-10) M at 25°C.
To find the H+ concentration for an aqueous solution, we need to use the relationship between the pH, pOH, and H+ concentration. The pH and pOH are related to each other by the equation: pH + pOH = 14.
Given that the pOH is 4.13, we can find the pH by subtracting the pOH from 14: pH = 14 - pOH = 14 - 4.13 = 9.87.
The pH is measured on a logarithmic scale, which means that the H+ concentration is given by 10 raised to the power of the negative pH: [H+] = 10^(-pH).
Therefore, the H+ concentration for the given aqueous solution is [H+] = 10^(-9.87). To calculate this value, you can use a scientific calculator or the calculator function on your phone or computer.