Ould you please offer me some insight to this,

Calculate the hydrogen ion concentration (H+) for the aqueous solution in which (OH-) is1×10-15 mol/L. Is this solution acidic, basic or neutral?
Thanks in advance

(H^+)(OH^-) = Kw = 1E-14

You know OH, solve for H^+.
If H = OH neutral
If H > OH acid
If H < OH basic

To calculate the hydrogen ion concentration (H+) in the given solution, we can utilize the concept of the pH scale. The pH scale is a logarithmic scale used to measure the acidity or alkalinity (basicity) of a solution. The pH scale ranges from 0 to 14, where a pH of 7 is considered neutral, a pH lower than 7 is acidic, and a pH higher than 7 is basic or alkaline.

In this case, we are given the hydroxide ion concentration (OH-) of the aqueous solution, which is 1×10^-15 mol/L. To calculate the hydrogen ion concentration (H+), we need to use the concept of the Kw constant, which represents the equilibrium constant for water.

Kw = [H+][OH-]

At 25°C, Kw has a value of 1.0 × 10^-14 mol^2/L^2. Since we are given the hydroxide ion concentration (OH-), we can rearrange the equation and solve for the hydrogen ion concentration (H+).

[H+] = Kw / [OH-]
[H+] = (1.0 × 10^-14 mol^2/L^2) / (1×10^-15 mol/L)
[H+] = 1.0 × 10^-14 mol/L / 1×10^-15 mol/L
[H+] = 10

Therefore, the hydrogen ion concentration (H+) in the solution is 10 mol/L.

Now, to determine whether the solution is acidic, basic, or neutral, we can use the pH scale. As mentioned earlier, a pH less than 7 indicates acidity, a pH greater than 7 indicates alkalinity, and a pH of 7 indicates neutrality.

To find the pH, we can use the formula:

pH = -log[H+]

pH = -log(10)
pH ≈ -1

Since the calculated pH is less than 7, this solution can be considered acidic.