Question

Determine the mass percent of anhydrous sodium carbonate \(\left(\mathrm{Na}_{2} \mathrm{CO}_{3}\right)\) and water in sodium carbonate decahydrate \(\left(\mathrm{Na}_{2} \mathrm{CO}_{3} \cdot 10 \mathrm{H}_{2} \mathrm{O}\right)\)

Short answer

In sodium carbonate decahydrate \(\left(\mathrm{Na}_{2} \mathrm{CO}_{3} \cdot 10 \mathrm{H}_{2} \mathrm{O}\right)\), the mass percent of anhydrous sodium carbonate \(\left(\mathrm{Na}_{2} \mathrm{CO}_{3}\right)\) is 37.03%, while the mass percent of water (H2O) is 62.97%.

Step-by-step solution

Determine the molar mass of anhydrous sodium carbonate (Na2CO3)

To find the molar mass, sum up the molar masses of the individual elements in the compound. For Na2CO3: Molar Mass of Na = 22.99 g/mol Molar Mass of C = 12.01 g/mol Molar Mass of O = 16.00 g/mol Molar mass of Na2CO3 = (2 × 22.99) + 12.01 + (3 × 16.00) = 105.99 g/mol

Determine the molar mass of sodium carbonate decahydrate (Na2CO3·10H2O)

We will determine the molar mass of Na2CO3·10H2O by adding the molar mass of Na2CO3 and 10 times the molar mass of H2O. Molar Mass of H2O = (2 × 1.01) + 16.00 = 18.02 g/mol Molar mass of Na2CO3·10H2O = 105.99 + (10 × 18.02) = 105.99 + 180.20 = 286.19 g/mol

Calculate the mass percentage of anhydrous sodium carbonate (Na2CO3) in sodium carbonate decahydrate

To find the mass percentage of Na2CO3 in Na2CO3·10H2O, divide the molar mass of Na2CO3 by the molar mass of Na2CO3·10H2O and multiply by 100: Mass percentage of Na2CO3 = (Molar mass of Na2CO3 / Molar mass of Na2CO3·10H2O) × 100 = (105.99 / 286.19) × 100 = 37.03%

Calculate the mass percentage of water (H2O) in sodium carbonate decahydrate

To find the mass percentage of H2O in Na2CO3·10H2O, divide the total molar mass of H2O by the molar mass of Na2CO3·10H2O and multiply by 100: Mass percentage of H2O = (Total molar mass of H2O / Molar mass of Na2CO3·10H2O) × 100 = (180.20 / 286.19) × 100 = 62.97% So, the mass percent of anhydrous sodium carbonate (Na2CO3) in sodium carbonate decahydrate is 37.03%, and the mass percent of water (H2O) in sodium carbonate decahydrate is 62.97%.

Key concepts

Molar Mass Calculation

Molar mass is a crucial concept in chemistry, representing the mass of one mole of a substance. It is measured in grams per mole (g/mol).
Calculating the molar mass of a compound involves summing the molar masses of all the atoms that constitute the molecular formula of the compound.

• The atomic masses of elements are usually found on the periodic table.
• Each element's molar mass is multiplied by the number of times the element appears in the formula.

For example, in the compound \(\mathrm{Na}_{2} \mathrm{CO}_{3}\), sodium (Na) appears twice, carbon (C) once, and oxygen (O) three times. By multiplying the atomic masses by these frequencies and adding them together, we can determine that the molar mass for \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) is 105.99 g/mol.
This technique helps determine other values needed to find the mass percent composition in more complex problems.

Sodium Carbonate Decahydrate

Sodium carbonate decahydrate, represented as \(\mathrm{Na}_{2} \mathrm{CO}_{3} \cdot 10 \mathrm{H}_{2} \mathrm{O}\), is a hydrated form of sodium carbonate.
"Deca" refers to the ten water (H₂O) molecules attached to each \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) unit.

• This compound is often referred to as "washing soda" and has applications in domestic and industrial cleaning.
• The presence of water causes it to have a different molar mass than anhydrous sodium carbonate.

To find the molar mass of sodium carbonate decahydrate, we combine the molar mass of sodium carbonate with that of the ten water molecules. Calculating as done earlier, the molar mass of \(\mathrm{Na}_{2} \mathrm{CO}_{3} \cdot 10 \mathrm{H}_{2} \mathrm{O}\) totals 286.19 g/mol.
This hydrated version changes some physical properties, like solubility and crystalline structure.

Anhydrous Sodium Carbonate

Anhydrous sodium carbonate, commonly referred to as \(\mathrm{Na}_{2} \mathrm{CO}_{3}\), is the base form of sodium carbonate without any water molecules attached. "Anhydrous" effectively means "without water".

• This compound appears as a white, powdery solid and is known for its applications in glass manufacturing and detergent formulations.
• Without attached water, it maintains the simple molecular weight calculated from its constituent elements.

In industrial and chemical contexts, the absence of water in anhydrous sodium carbonate allows for reactions without moisture-related side effects. Knowing its molar mass of 105.99 g/mol provides a basis for calculating compositions of more complex hydrated forms, like sodium carbonate decahydrate.
Its comparative simplicity makes it invaluable for stoichiometry-based calculations and mass percent composition tasks.

Molecular Formula

A molecular formula represents the number and type of atoms present in a molecule of a compound. Unlike empirical formulas, which provide a simplified ratio, molecular formulas give the exact composition.

• This formula is crucial for understanding the precise weight of the molecule because it tells us each element's contribution to the mass.
• By using the molecular formula, chemists can easily identify and quantify the possible interactions and compounds in a reaction.

For example, the molecular formula \(\mathrm{Na}_{2} \mathrm{CO}_{3} \cdot 10 \mathrm{H}_{2} \mathrm{O}\) indicates the full composition and structure, including ten water molecules.
When performing calculations like determining molar mass or percentage compositions, knowing the molecular formula ensures that all components are correctly accounted for.
This guards against error and ensures precise formulation in laboratory and industrial settings.