Recall that molarity is given by:

$\overline{){\mathbf{Molarity}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{moles}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solute}}{\mathbf{Liters}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solution}}}$

We are going to do the following steps to solve this problem:

Step 1: Determine moles of solute

Step 2: Determine Liters of solution

Step 3: Determine the molarity of the solution

Step 4: Determine the molarity of each ions

Calcium hydroxide is a strong base. Compute [Ca^{2+}] and [OH^{−}] for a solution that is prepared by dissolving 0.60 g of Ca(OH)_{2} in enough water to make a 1500 mL of solution. [Atomic weights: Ca=40, O=16, H=1]

a. 5.4x10^{-3}, 9.1x10^{-3}

b. 5.4x10^{-3}, 1.08x10^{-2}

c. 5.4x10^{-3}, 5.4x10^{-3}

d. 1.8x10^{-2}, 1.8x10^{-2}

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