If the pH of a solution NaCN is 8.710 what would the equilibrium concentration of CN^- is
To determine the equilibrium concentration of CN^- in the solution, we need to calculate the concentration of H+ ions first.
Since the pH of the solution is given, we can calculate the concentration of H+ ions using the formula:
pH = -log[H+]
Rearranging the equation, we have:
[H+] = 10^(-pH)
Substituting the given pH value:
[H+] = 10^(-8.710)
Calculating this, we find:
[H+] ≈ 1.32 x 10^(-9) M
Now, since NaCN is a strong electrolyte, it will completely dissociate into its ions Na+ and CN^-.
Therefore, the concentration of CN^- ions will be equal to the concentration of NaCN, as it is a 1:1 ratio.
Thus, the equilibrium concentration of CN^- ions in the solution is approximately 1.32 x 10^(-9) M.