A mixture contains only NaCl and Fe(NO3)3. A .456 gram sample of the mixture is dissolved in water and an excess of NaOH is added, producing a precipitate of Fe(OH)3. The precipitate is dried and filtered, and its mass is determined to be .107 g.
The mass of iron in the sample?
The mass of Fe(NO3)3 in the sample?
the mass percent of Fe(NO3)3 in the sample?
hjh
Oh, the chemistry of mixtures! Let's solve this problem step by step, shall we?
Firstly, we need to figure out the mass of iron (Fe) in the sample. Since the only source of iron in the mixture is Fe(NO3)3, we can assume that all of the iron comes from this compound.
Given that the mass of Fe(OH)3 precipitate is 0.107 g, we can calculate the moles of Fe(OH)3 by dividing its mass by its molar mass. Then, we use the balanced chemical equation to determine the moles of Fe(NO3)3, which is 1:1 with Fe(OH)3. Finally, we multiply the moles of Fe(NO3)3 by its molar mass to find the mass of Fe(NO3)3 in the sample.
As for the mass percent of Fe(NO3)3 in the sample, we divide the mass of Fe(NO3)3 by the mass of the sample, then multiply by 100 to get the mass percent.
Let's crunch some numbers and find out the answers!
Inserting numbers into the equation... *beep boop beep*... calculating... 42%... humorous drumroll, please...
The mass of iron in the sample is 0.107 grams, and let's call it "The Iron King"!
The mass of Fe(NO3)3 in the sample is the same as "The Iron King" because it's the only source of iron, so it's 0.107 grams as well.
Finally, the mass percent of Fe(NO3)3 in the sample is approximately 23.39% (calculated by dividing the mass of Fe(NO3)3 by the mass of the sample and multiplying by 100). Let's call it "The Nitrate Dancer"!
So, to summarize:
- The mass of iron in the sample is 0.107 grams, The Iron King!
- The mass of Fe(NO3)3 in the sample is also 0.107 grams, still The Iron King, showing off its dual identity!
- The mass percent of Fe(NO3)3 in the sample is approximately 23.39%, The Nitrate Dancer!
I hope those calculations brought a smile to your face, just like a dancing nitrate! If you have any more questions or need further amusement, I'm here to assist!
To find the mass of iron in the sample, we need to calculate the difference in mass before and after the formation of Fe(OH)3.
1. Calculate the mass of Fe(OH)3 precipitated:
Mass of Fe(OH)3 = 0.107 g
2. Convert the mass of Fe(OH)3 to the mass of iron.
Fe(OH)3 has an atomic weight of 106.867 g/mol, and it contains one iron atom. Therefore,
Mass of iron in Fe(OH)3 = 1 * (55.845 g/mol / 106.867 g/mol) * 0.107 g = 0.056 g
So, the mass of iron in the sample is 0.056 grams.
To find the mass of Fe(NO3)3 in the sample, we need to use stoichiometry.
3. Calculate the molar ratio between Fe(OH)3 and Fe(NO3)3:
From the balanced equation: Fe(NO3)3 + 3NaOH -> Fe(OH)3 + 3NaNO3
The molar ratio between Fe(NO3)3 and Fe(OH)3 is 1:1.
4. Convert the mass of Fe(OH)3 to the mass of Fe(NO3)3.
The molar mass of Fe(NO3)3 is 241.859 g/mol. Therefore,
Mass of Fe(NO3)3 = (241.859 g/mol / 106.867 g/mol) * 0.107 g = 0.243 g
So, the mass of Fe(NO3)3 in the sample is 0.243 grams.
To find the mass percent of Fe(NO3)3 in the sample, we need to express the mass of Fe(NO3)3 as a percentage of the total mass of the mixture.
5. Calculate the total mass of the mixture.
The total mass of the mixture is given as 0.456 grams.
6. Calculate the mass percent of Fe(NO3)3.
Mass percent of Fe(NO3)3 = (mass of Fe(NO3)3 / total mass of mixture) * 100
Mass percent of Fe(NO3)3 = (0.243 g / 0.456 g) * 100 = 53.29%
Therefore, the mass percent of Fe(NO3)3 in the sample is 53.29%.
mass Fe = 0.107 x (1 mol Fe(OH)3/molar mass Fe(OH)3) x (1 mol Fe/1 mol Fe(OH)3) x (molar mass Fe/1 mol Fe) = ??
mass Fe(NO3)3 = mass Fe(OH)3 x (molar mass Fe(NO3)3/molar mass Fe(OH)3 = xx
%Fe(NO3)3 = (mass Fe(NO3)3/mass sample)*100 = xx