a container holds 2.0 l of 2.0 m na₂co₃ solution. how many moles of na⁺ ions are in the solution?\n\nna₂co₃…

a container holds 2.0 l of 2.0 m na₂co₃ solution. how many moles of na⁺ ions are in the solution?\n\nna₂co₃ → 2na⁺ + co₃²⁻\n\n2.0 moles na⁺\n8.0 moles na⁺\n4.0 moles na⁺

a container holds 2.0 l of 2.0 m na₂co₃ solution. how many moles of na⁺ ions are in the solution?\n\nna₂co₃ → 2na⁺ + co₃²⁻\n\n2.0 moles na⁺\n8.0 moles na⁺\n4.0 moles na⁺

Answer

Explanation:

Step1: Calculate moles of $\text{Na}_2\text{CO}_3$

Moles = Molarity × Volume = $2.0\ \text{M} \times 2.0\ \text{L} = 4.0\ \text{mol}$

Step2: Relate to $\text{Na}^+$ moles

1 $\text{Na}_2\text{CO}_3$ gives 2 $\text{Na}^+$, so: Moles of $\text{Na}^+ = 4.0\ \text{mol} \times 2 = 8.0\ \text{mol}$

Answer:

8.0 moles Na⁺