How many cations are there in 10.0 g of sodium phosphate?

Question

Quizplus · Accepted Answer

First, we need to find the molar mass of sodium phosphate ($Na_3PO_4$). The molar mass is calculated as follows: $3 \times 22.99$ (sodium) + $30.97$ (phosphorus) + $4 \times 16.00$ (oxygen) = $163.94 \, g/mol$. Then, we calculate the number of moles in 10.0 g of sodium phosphate: $10.0 \, g \div 163.94 \, g/mol = 0.061 \, mol$. Since each formula unit of sodium phosphate contains 3 sodium ions ($Na^+$), the total number of cations is $0.061 \, mol \times 3 \times 6.022 \times 10^{23} \, mol^{-1} = 1.10 \times 10^{23}$ cations.

How Many Cations Are There in 10