Final answer:
To find the number of Na+ ions in 1.50 grams of sodium, you first convert the mass to moles using the molar mass of sodium, then convert the moles to ions using Avogadro's number, resulting in approximately 3.91 × 10²22 Na+ ions.
Step-by-step explanation:
To calculate how many ions of Na+ are in 1.50 grams of sodium, we need to use the molar mass of sodium and Avogadro's number.
Step 1: Convert Grams to Moles
First, we convert the mass of sodium to moles using the molar mass of sodium (Na), which is approximately 22.99 g/mol:
1.50 g Na * (1 mol Na / 22.99 g Na) = 0.065 mol Na
Step 2: Convert Moles to Ions
Next, we use Avogadro's number (6.022 × 1023 ions/mol) to convert moles to ions:
0.065 mol Na * (6.022 × 1023 ions/mol Na) = 3.91 × 1022 Na+ ions
Therefore, there are approximately 3.91 × 1022 Na+ ions in 1.50 grams of sodium.