(a) What is the mass, in grams, of 2.50⨉10⁻³ mol of ammonium phosphate?

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Determine the molar mass of ammonium phosphate, (NH_4)_3PO_4.

Calculate the molar mass by adding the atomic masses of all atoms in the formula: 3 nitrogen (N), 12 hydrogen (H), 1 phosphorus (P), and 4 oxygen (O) atoms.

Use the formula: mass (g) = moles × molar mass (g/mol) to find the mass.

Substitute the given moles (2.50 \(\times\) 10^{-3} mol) and the calculated molar mass into the formula.

Perform the multiplication to find the mass in grams.

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Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in a molecule. For ammonium phosphate (NH4)3PO4, the molar mass can be determined by adding the masses of nitrogen, hydrogen, phosphorus, and oxygen in the compound.

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Molar Mass Concept

Stoichiometry

Stoichiometry is the area of chemistry that involves the calculation of reactants and products in chemical reactions. It allows chemists to predict the quantities of substances consumed and produced in a given reaction based on the balanced chemical equation. In this case, stoichiometry helps relate the number of moles of ammonium phosphate to its mass.

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Conversion of Moles to Grams

To convert moles of a substance to grams, one multiplies the number of moles by the molar mass of the substance. This conversion is essential in quantitative chemistry, as it allows for the practical application of mole calculations in laboratory settings. For the given question, multiplying 2.50×10⁻³ mol of ammonium phosphate by its molar mass will yield the mass in grams.

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