Let's walk through the process of determining the moles of [tex]\( \text{BaCl}_2 \)[/tex] present in 200 mL of 0.10 M [tex]\( \text{BaCl}_2 \)[/tex].
1. Volume Conversion:
- First, convert the volume from milliliters (mL) to liters (L) since molarity is given in terms of moles per liter (M).
- 200 mL [tex]\( \times \frac{1 \text{ L}}{1000 \text{ mL}} = 0.2 \text{ L} \)[/tex]
2. Calculate the Moles of [tex]\( \text{BaCl}_2 \)[/tex]:
- Use the molarity (0.10 M) to find the moles of [tex]\( \text{BaCl}_2 \)[/tex] in the 0.2 liters of solution.
- Molarity (M) is defined as moles of solute per liter of solution.
- Therefore, moles of [tex]\( \text{BaCl}_2 \)[/tex] = Molarity [tex]\( \times \)[/tex] Volume (in liters)
- [tex]\( \text{moles of BaCl}_2 = 0.10 \text{ M} \times 0.2 \text{ L} = 0.020 \text{ mol} \)[/tex]
Thus, there are [tex]\( 0.020 \)[/tex] moles of [tex]\( \text{BaCl}_2 \)[/tex] present in 200 mL of 0.10 M [tex]\( \text{BaCl}_2 \)[/tex].
