Final answer:
To calculate the moles of solute particles in 100.0 ml of 2.50 M (NH₄)₃PO₄, you convert the volume to liters, multiply by the molarity to find the moles of (NH₄)₃PO₄, then account for dissociation, which leads to 1.25 moles of solute particles.
Step-by-step explanation:
To find out how many moles of solute particles are present in 100.0 ml of 2.50 M (NH₄)₃PO₄, we need to understand a couple of concepts. First, 'M' stands for molarity, which is the number of moles of solute per liter of solution. We also need to know that (NH₄)₃PO₄ dissociates into 4NH₄⁺ and 1PO₄³⁻, resulting in a total of 4 + 1 = 5 moles of particles per mole of (NH₄)₃PO₄.
To calculate the moles of solute particles, we can perform the following steps:
- Convert the volume of the solution from milliliters to liters: 100.0 ml = 0.100 L.
- Multiply the molarity of the solution by the volume in liters to get the moles of(NH₄)₃PO₄:
2.50 M * 0.100 L = 0.250 moles of (NH4)3PO4. - Since each mole of (NH₄)₃PO₄. produces 5 moles of particles upon dissociation, multiply 0.250 moles of (NH₄)₃PO₄. by 5:
0.250 moles * 5 = 1.25 moles of solute particles.
Therefore, there are 1.25 moles of solute particles in 100.0 ml of 2.50 M (NH₄)₃PO₄.