what is the value of [OH-] in a 0.730 M solution of Sr(OH)2?
Nevermind. I figured it out.
To determine the value of [OH-], we need to consider the stoichiometry of the compound Sr(OH)2. For each mole of Sr(OH)2, we have two moles of OH-.
First, let's calculate the molar concentration of Sr(OH)2:
Given the concentration of Sr(OH)2 solution as 0.730 M, this means that there are 0.730 moles of Sr(OH)2 in one liter of solution.
Since Sr(OH)2 dissociates into Sr2+ ions and two OH- ions, we have twice the concentration of OH- compared to Sr(OH)2.
Thus, the concentration of OH- in the solution will be 2 times the concentration of Sr(OH)2:
[OH-] = 2 * 0.730 M
= 1.460 M
Therefore, the value of [OH-] in a 0.730 M solution of Sr(OH)2 is 1.460 M.