Calculate the hydrogen-ion concentration [H+] for an aqueous solution in which [OH-] is 1 x 10^-11 mol/L. Is this solution acidic, basic, or neutral?
To calculate the hydrogen-ion concentration [H+], you can use the equation for the ion product of water.
The ion product of water (Kw) is defined as the product of the hydrogen-ion concentration [H+] and the hydroxide-ion concentration [OH-] in an aqueous solution at a given temperature. At 25°C, Kw is approximately 1 x 10^-14.
The equation for the ion product of water is as follows:
Kw = [H+] x [OH-]
Since you have been given the hydroxide-ion concentration [OH-] as 1 x 10^-11 mol/L, and you know that Kw = 1 x 10^-14, you can rearrange the equation to solve for the hydrogen-ion concentration [H+].
[H+] = Kw / [OH-]
[H+] = (1 x 10^-14) / (1 x 10^-11)
[H+] = 1 x 10^-14 / 1 x 10^-11
[H+] = 1 x 10^-14 x 1 x 10^11
[H+] = 1 x 10^-3
So, the hydrogen-ion concentration [H+] is 1 x 10^-3 mol/L.
Since the hydrogen-ion concentration is greater than 1 x 10^-7 mol/L (which is the concentration of a neutral solution), this solution is acidic.
Therefore, the solution is acidic based on the given hydrogen-ion concentration.
To calculate the hydrogen-ion concentration ([H+]) for the given aqueous solution, we can use the relationship between the concentrations of hydrogen ions and hydroxide ions in water:
[H+] × [OH-] = 1 x 10^-14 mol^2/L^2
Given that [OH-] = 1 x 10^-11 mol/L, we can substitute this value into the equation and rearrange it to solve for [H+]:
[H+] × 1 x 10^-11 = 1 x 10^-14
[H+] = (1 x 10^-14) / (1 x 10^-11)
[H+] = 1 x 10^-14 / 1 x 10^-11
[H+] = 1 x 10^-3 mol/L
Therefore, the hydrogen-ion concentration ([H+]) is 1 x 10^-3 mol/L.
To determine if the solution is acidic, basic, or neutral, we'll compare the [H+] with the reference pH scale:
- If [H+] is greater than 1 x 10^-7 mol/L, the solution is acidic.
- If [H+] is less than 1 x 10^-7 mol/L, the solution is basic.
- If [H+] is exactly 1 x 10^-7 mol/L, the solution is neutral.
In this case, since [H+] is 1 x 10^-3 mol/L, which is greater than 1 x 10^-7 mol/L, the solution is acidic.
(H^+)(OH^-) = Kw = 1 x 10^-14
(H^+) >1 x 10^-7 = acid
(H^+) = 1 x 10^-7 = neutral
(H^+) < 1 x 1-^-7 = basic