If the pH of a solution of NaCN(aq) is 8.710, then the equilibrium concentration of CN^-(aq) expressed in scientific notation
To find the equilibrium concentration of CN^-(aq), we need to convert the given pH to the concentration of H^+(aq), and then use the ionization constant of water to find the concentration of OH^-(aq). Since CN^-(aq) is the conjugate base of HCN(aq), we can use the relationship:
pH + pOH = 14
We are given that the pH is 8.710, so we can calculate the pOH:
pOH = 14 - pH
= 14 - 8.710
= 5.290
Now, we can convert pOH to the concentration of OH^-(aq) using the formula:
pOH = -log[OH^-]
-[OH^-] = 10^(-pOH)
= 10^(-5.290)
Since the solution is aqueous and not saturated, we can assume that [OH^-] = [CN^-]. Therefore, the equilibrium concentration of CN^-(aq) is:
[CN^-] = 10^(-5.290)