To find the pH of a 0.0660 M solution of LiOH, we need to first consider the chemical reaction that occurs when LiOH dissolves in water:
LiOH → Li+ + OH-
LiOH dissociates completely in water to produce Li+ ions and OH- ions. Since LiOH is a strong base, it will generate a high concentration of OH- ions in solution.
We can use the concentration of OH- ions to calculate the pH of the solution, using the following equation:
pH = 14 - pOH
where pOH is the negative logarithm of the hydroxide ion concentration [OH-]. To find the pOH of the solution, we first need to calculate the concentration of OH- ions using the concentration of LiOH:
[OH-] = 0.0660 M
Now we can calculate the pOH:
pOH = -log[OH-] pOH = -log(0.0660) pOH = 1.18
Finally, we can calculate the pH using the equation above:
pH = 14 - pOH pH = 14 - 1.18 pH = 12.82
Therefore, the pH of a 0.0660 M solution of LiOH is 12.82.
