Question

A 500 mL solution of 0.002 M NaOH would contain how many moles of OH-?

Answer 1

Answer on Question #43708 - Chemistry - Physical Chemistry

Question:

A 500 mL solution of 0.002 M NaOH would contain how many moles of OH⁻?

Answer:

$$\text{molarity} = \frac{\text{moles of solute}}{\text{liter of solution}}$$

From this equation we calculate moles of solute of NaOH in 500 mL of 0.002 M.

$$\text{moles of solute} = \text{molarity} \times \text{liter of solution} = 0.002 \mathrm{M} \times 0.5 \mathrm{L} = 0.001 \text{ moles}$$

When dissolved in water, the strong base sodium hydroxide ionizes into hydroxide and sodium ions:

$$\mathrm{NaOH} \rightarrow \mathrm{Na}^{+} + \mathrm{OH}^{-}$$

As you see from the chemical equation from 1 mole of NaOH we can get 1 mole of OH⁻. That's why from 0.001 moles of NaOH we can get 0.001 moles of OH⁻.

Answer: 0.001 moles of OH⁻

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