Chemistry
Hey guys, i have a question about how to figure out how much mass of a compound i need to find 130ppm here is the question.
What mass of Fe(NH4)2(SO4)2*6H2O is required to prepare 2.25 L of a 130 ppm iron solution?
Now i know that ppm is (mg of desired compound)/(kg of solvent used) But in this case im not quite sure what the solvent would be?
Would the solvent be the previously explained Fe..... compound just minus the Fe? or would the compound just bethe 6H2O? im confused, if anyone could help that would be great.
To solve this problem, we need to determine the mass of Fe(NH4)2(SO4)2·6H2O required to prepare the 2.25 L solution with a concentration of 130 ppm.
First, let's understand the meaning of ppm. ppm stands for "parts per million," and it represents the ratio of the mass of the solute (in this case, Fe(NH4)2(SO4)2·6H2O) to the mass of the solution (solvent + solute), multiplied by one million.
In this context, the solvent refers to the liquid component of the solution, which does not react with the solute. In this case, the solvent is indeed the water (H2O). The Fe(NH4)2(SO4)2 compound and the associated 6H2O molecules are considered solute.
To find the mass of Fe(NH4)2(SO4)2·6H2O needed, we'll follow these steps:
Step 1: Convert ppm to a decimal fraction
130 ppm means 130 parts per million, so we can rewrite this as 130/1,000,000, which simplifies to 0.00013 (since we are multiplying by one million).
Step 2: Calculate the mass of the solvent (water)
To determine the mass of the solution, we need to find the density of water. The density of water at room temperature is approximately 1 g/mL or 1 kg/L.
Therefore, the mass of the solvent (water) in the 2.25 L solution is 2.25 kg (2.25 L x 1 kg/L).
Step 3: Calculate the mass of the solute (Fe(NH4)2(SO4)2·6H2O)
Now we can use the ppm value to find the mass of the solute.
Mass of solute = ppm x mass of solvent
Mass of solute = 0.00013 x 2.25 kg
Step 4: Calculate the molar mass of Fe(NH4)2(SO4)2·6H2O
To determine the mass of a compound, we need to know its molar mass. The molar mass of Fe(NH4)2(SO4)2·6H2O can be calculated by summing up the atomic masses of all the elements in the compound.
Fe(NH4)2(SO4)2·6H2O contains:
- 1 Fe atom (55.85 g/mol)
- 2 Ammonium (NH4) ions (2 x 18.03 g/mol)
- 2 Sulfate (SO4) ions (2 x 96.06 g/mol)
- 12 water (H2O) molecules (12 x 18.02 g/mol)
Calculate the total molar mass by summing up these values.
Step 5: Convert the mass of the solute to the required mass of Fe(NH4)2(SO4)2·6H2O
Using the molar mass calculated in step 4, divide the mass of the solute obtained in step 3 by the molar mass to find the mass of Fe(NH4)2(SO4)2·6H2O required.
Now you have the mass of the Fe(NH4)2(SO4)2·6H2O compound needed to prepare the 2.25 L iron solution with a concentration of 130 ppm.
To determine the mass of Fe(NH4)2(SO4)2*6H2O needed to prepare a 130 ppm iron solution, you need to consider the total volume of solution and the amount of iron required.
1. Identify the solvent:
In this case, the solvent is the solution you will be preparing, which is the 2.25 L of the iron solution.
2. Calculate the mass of Fe required:
To determine the mass of Fe (iron) required, you need to convert the ppm concentration to a mass concentration.
ppm = (mass of solute / mass of solution) * 10^6
Since you want to determine the mass of solute (Fe), rearrange the formula:
mass of solute = (ppm * mass of solution) / 10^6
Given:
ppm = 130
mass of solution = 2.25 L
mass of solute = (130 ppm * 2.25 L) / 10^6
3. Convert the volume of solution to mass of solution:
To convert the volume of solution (2.25 L) to mass, you need to know the density of the solution. Assuming the density is 1 g/mL (since most aqueous solutions have similar densities to water), you can use the following conversion:
mass of solution = volume of solution * density
mass of solution = 2.25 L * 1 g/mL
4. Calculate the mass of Fe(NH4)2(SO4)2*6H2O:
To determine the mass of Fe(NH4)2(SO4)2*6H2O, you need to find the molar mass and the stoichiometric ratio of Fe in the compound.
The molar mass of Fe(NH4)2(SO4)2*6H2O is calculated as follows:
Fe: 1 atom * molar mass of Fe
(NH4)2(SO4)2: 1 molecule * molar mass of (NH4)2(SO4)2
6H2O: 6 molecules * molar mass of H2O
Add up all the calculated masses to get the molar mass of Fe(NH4)2(SO4)2*6H2O.
5. Use stoichiometry to relate Fe to Fe(NH4)2(SO4)2*6H2O:
Now, determine the stoichiometric ratio of Fe in Fe(NH4)2(SO4)2*6H2O. This can be determined by looking at the balanced chemical equation for the compound.
For example, if the equation is 2 Fe(NH4)2(SO4)2*6H2O -> 2 Fe + ... (rest of the equation),
then the stoichiometric ratio of Fe to Fe(NH4)2(SO4)2*6H2O is 2:2 or 1:1.
6. Calculate the required mass of Fe(NH4)2(SO4)2*6H2O:
Multiply the mass of Fe calculated in step 3 by the stoichiometric ratio determined in step 5 to find the mass of Fe(NH4)2(SO4)2*6H2O required.
Remember to use the molar mass of Fe(NH4)2(SO4)2*6H2O calculated in step 4 to get accurate results.
I hope this step-by-step explanation helps you calculate the mass of Fe(NH4)2(SO4)2*6H2O required for the iron solution!