Given that the pOH of a solution is 6.0, we can use the relationship between pH, pOH, and the ion product of water (Kw) in aqueous solutions:
\[pH + pOH = 14\]
Here, pH is the negative logarithm of the hydrogen ion concentration ([H+]) and pOH is the negative logarithm of the hydroxide ion concentration ([OH^-]). Since we are given the pOH as 6.0, we can substitute this value into the equation:
\[pH + 6.0 = 14\]
Now, let's solve for pH:
\[pH = 14 - 6.0\]
\[pH = 8.0\]
So, the correct statement is:
\[pH + pOH = 14\]
\[8.0 + 6.0 = 14\]
Therefore, the correct statement is "pH plus pOH equals 14."
