Calculate the volume and mass required to make 100 mL of 0.10 M solutions of your assigned acid and conjugate base.
Assigned acid and conjugate base:
Ammonium chloride- 53.49 g/mol
Ammonia- 1.0 M
ammonium chloride:
mass=.1*.100*53.49 grams. Add water to make up 100ml
ammonia:
you are diluting it 10 times, 1 part ammonia, 9 parts water.
1 part=100ml/10=10ml
9 parts:90ml
To calculate the volume and mass required to make a 0.10 M solution of ammonium chloride and ammonia, we need to use the formula:
Molarity (M) = moles of solute / volume of solution in liters
First, let's calculate the moles of solute needed using the formula:
moles = Molarity * volume (in liters)
Given:
Molarity (M) = 0.10 M
Volume = 100 mL = 0.1 L
For Ammonium Chloride:
Molar mass of Ammonium Chloride = 53.49 g/mol
Using the formula for moles:
moles of Ammonium Chloride = Molarity * volume
moles of Ammonium Chloride = 0.10 M * 0.1 L = 0.01 moles
Now, we can calculate the mass of Ammonium Chloride needed using the formula:
mass = moles * molar mass
mass of Ammonium Chloride = 0.01 moles * 53.49 g/mol = 0.5349 g
Therefore, to make 100 mL of a 0.10 M Ammonium Chloride solution, you would need to measure 0.5349 grams of Ammonium Chloride.
Similarly, for Ammonia:
Molarity (M) = 1.0 M
Volume = 100 mL = 0.1 L
For Ammonia:
Molar mass of Ammonia = 17.03 g/mol
Using the formula for moles:
moles of Ammonia = Molarity * volume
moles of Ammonia = 1.0 M * 0.1 L = 0.1 moles
Now, we can calculate the mass of Ammonia needed using the formula:
mass = moles * molar mass
mass of Ammonia = 0.1 moles * 17.03 g/mol = 1.703 g
Therefore, to make 100 mL of a 0.10 M Ammonia solution, you would need to measure 1.703 grams of Ammonia.
To calculate the volume and mass required to make 100 mL of a 0.10 M solution of ammonium chloride (NH4Cl) and ammonia (NH3), we need to use the formula:
Molarity (M) = moles / volume (L)
First, let's calculate the moles of NH4Cl required for a 0.10 M solution:
Molarity (M) = moles / volume (L)
0.10 M = moles / 0.100 L
moles of NH4Cl = 0.10 M x 0.100 L
moles of NH4Cl = 0.010 mol
Next, let's calculate the mass of NH4Cl required:
molar mass of NH4Cl = 53.49 g/mol
mass of NH4Cl = moles x molar mass
mass of NH4Cl = 0.010 mol x 53.49 g/mol
mass of NH4Cl = 0.5349 g
So, to make 100 mL of a 0.10 M NH4Cl solution, you will need 0.5349 grams of NH4Cl.
Now, let's calculate the moles of ammonia (NH3) required for a 0.10 M solution:
Molarity (M) = moles / volume (L)
0.10 M = moles / 0.100 L
moles of NH3 = 0.10 M x 0.100 L
moles of NH3 = 0.010 mol
Since the molarity of ammonia is already given as 1.0 M, we don't need to calculate the mass as it is already at the desired concentration.
So, to make 100 mL of a 0.10 M NH3 solution, you will need 0 grams of NH3.