Calculate the amount concentration of the ammonium ion in 100.0 ml of a solution containing 14.4 g of ammonium carbonate.
To calculate the amount concentration of the ammonium ion (NH4+) in the given solution, we need to know the molar mass of ammonium carbonate and use it to find the number of moles of NH4+.
The molar mass of ammonium carbonate (NH4)2CO3 is calculated by adding the molar masses of the individual elements:
Molar mass of nitrogen (N) = 14.01 g/mol
Molar mass of hydrogen (H) = 1.01 g/mol x 4 = 4.04 g/mol
Molar mass of carbon (C) = 12.01 g/mol
Molar mass of oxygen (O) = 16.00 g/mol x 3 = 48.00 g/mol
Molar mass of (NH4)2CO3 = (14.01 g/mol x 2) + (1.01 g/mol x 4) + 12.01 g/mol + (16.00 g/mol x 3) = 96.09 g/mol
Next, we can use the given mass of ammonium carbonate (14.4 g) and its molar mass (96.09 g/mol) to calculate the number of moles using the formula:
Number of moles = mass / molar mass
Number of moles of (NH4)2CO3 = 14.4 g / 96.09 g/mol = 0.1493 mol
Since each mole of ammonium carbonate contains two moles of ammonium ions (NH4+), the number of moles of NH4+ will be twice as much:
Number of moles of NH4+ = 0.1493 mol x 2 = 0.2986 mol
Finally, we can calculate the amount concentration (C) of NH4+ by dividing the number of moles by the volume (V) of the solution in liters:
Amount concentration (C) = Number of moles / Volume
Volume = 100.0 ml = 100.0 ml / 1000 ml/L = 0.100 L
Amount concentration of NH4+ = 0.2986 mol / 0.100 L = 2.986 mol/L
Therefore, the amount concentration of the ammonium ion in the given solution is 2.986 mol/L.
To calculate the amount concentration of the ammonium ion, we first need to determine the moles of ammonium ion present in the solution.
Step 1: Find the molar mass of ammonium carbonate.
Ammonium carbonate consists of one ammonium ion (NH4+) and one carbonate ion (CO3^2-).
The molar mass of ammonium carbonate can be calculated by adding the molar masses of its constituents:
Molar mass of NH4+ = (1 x 14.01 g/mol) + (4 x 1.01 g/mol) = 18.05 g/mol
Molar mass of CO3^2- = (1 x 12.01 g/mol) + (3 x 16.00 g/mol) = 60.01 g/mol
The molar mass of ammonium carbonate is:
Molar mass of (NH4)2CO3 = (2 x 18.05 g/mol) + 60.01 g/mol = 96.09 g/mol
Step 2: Calculate the number of moles of ammonium carbonate.
We are given 14.4 g of ammonium carbonate.
Using the formula: moles = mass/molar mass
moles of (NH4)2CO3 = 14.4 g / 96.09 g/mol = 0.1499 mol (rounded to four decimal places)
Step 3: Determine the stoichiometry between ammonium carbonate and ammonium ion.
From the formula (NH4)2CO3, we can see that there are 2 ammonium ions (NH4+) for every 1 ammonium carbonate [(NH4)2CO3].
Therefore, for every mole of (NH4)2CO3, there are 2 moles of NH4+.
Step 4: Calculate the moles of ammonium ion.
moles of NH4+ = 2 x moles of (NH4)2CO3
moles of NH4+ = 2 x 0.1499 mol = 0.2998 mol (rounded to four decimal places)
Step 5: Calculate the amount concentration of the ammonium ion.
Amount concentration, also known as molarity, is defined as the moles of solute (NH4+) divided by the volume of the solution in liters.
Amount concentration (C) = moles of solute (NH4+) / volume of solution (in liters)
We are given the volume of the solution as 100.0 ml, which is equivalent to 0.1000 liters.
Amount concentration of NH4+ = 0.2998 mol / 0.1000 L = 2.998 M (rounded to three decimal places)
Therefore, the amount concentration of the ammonium ion in the solution is 2.998 M.
3.00 mol/L
In what? mols/L, M, g/L, etc. I'll assume M or moles/L.
moles (NH4)2CO3 = grams/molar mass = ?
Then mols NH4^+ = 2 x mols (NH4)2CO3.
M = mols NH4^+/L = ?