To determine the equilibrium concentration of CN^- in a solution of NaCN, we need to use the pH value and the dissociation constant of NaCN.
The pH of a solution is a measure of the concentration of H+ ions in the solution. In this case, we know that the pH of the solution is 8.710.
To find the equilibrium concentration of CN^-, we can use the pOH value, which is the negative logarithm of the concentration of OH- ions in the solution. Since water is the only source of OH- ions in this case, we can find the pOH value using the following equation:
pOH = 14 - pH
pOH = 14 - 8.710 = 5.29
To find the equilibrium concentration of CN^-, we can use the dissociation constant of NaCN. The dissociation constant (Ka) is a value that indicates the extent to which a compound dissociates in a solution. In this case, the dissociation constant (Ka) of NaCN is not provided, so we cannot calculate the equilibrium concentration of CN^- without this information.
However, if we assume that NaCN completely dissociates in water, we can say that the equilibrium concentration of CN^- is equal to the concentration of NaCN. Since we do not have the concentration of NaCN, we cannot determine the equilibrium concentration of CN^- in this specific scenario.
If the pH of a solution NaCN is 8.710 the equilibrium concentration of CN^- is
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