Iron (III) hydroxide is soluble in acid:
Fe(OH)3(s)3H^+(aq)-->Fe^3^+(aq)+3H2O(l)
a. How many milliliters of 1.00 M HCl are needed to dissolve 1.00 g of iron (III) hydroxide?
b. If you added enough HCl to dissolve the 1.00 g of iron (III) hydroxide and then diluted the solution to 50.0 mL, what would the concentration (molarity) of iron be in the solution?
c. Haw many grams of iron (III) hydroxide can be dissolved in 10.0 mL of 12.0 M HCl?
a. Convert 1.00 g Fe(OH)3 to mols. mols = grams/molar mass.
Use the coefficients in the balanced equation to convert mols Fe(OH)3 to mols H^+.
mols HCl = M x L. You know mols HCl and M HCl, solve for L and convert to mL.
b. M Fe^3+ = mols/L soln
You know mols from part a, L you get from L added from part a + 50 mL(0.050 L).l
c. mols HCl = M x L = 12.0 x 0.01 L = ?
Convert mols HCl to mols Fe(OH)3 and convert that to grams Fe(OH)3
a. To calculate the amount of HCl needed to dissolve 1.00 g of iron (III) hydroxide, we need to use the molar mass of Fe(OH)3.
Molar mass of Fe(OH)3 = (55.85 g/mol) + 3×(1.01 g/mol + 16.00 g/mol) = 106.84 g/mol
First, convert the mass of Fe(OH)3 to moles:
moles of Fe(OH)3 = mass / molar mass = 1.00 g / 106.84 g/mol = 0.00936 mol
Since the balanced equation shows that 1 mole of Fe(OH)3 reacts with 3 moles of HCl, we can set up a mole ratio:
0.00936 mol Fe(OH)3 × (3 mol HCl / 1 mol Fe(OH)3) = 0.0281 mol HCl
Now, we can calculate the volume of 1.00 M HCl needed using the molarity equation:
Molarity = moles / volume
1.00 M = 0.0281 mol / volume
Volume = 0.0281 mol / 1.00 M = 0.0281 L = 28.1 mL
Therefore, you would need approximately 28.1 mL of 1.00 M HCl to dissolve 1.00 g of iron (III) hydroxide.
b. After dissolving 1.00 g of iron (III) hydroxide in enough HCl and diluting the solution to 50.0 mL, we need to calculate the concentration (molarity) of iron (Fe^3+) in the solution.
Since 1 mole of Fe(OH)3 produces 1 mole of Fe^3+, the moles of Fe^3+ in the solution are equal to the moles of Fe(OH)3 dissolved:
moles of Fe^3+ = 0.00936 mol
Now, calculate the final molarity of Fe^3+ using the diluted volume:
Molarity = moles / volume
Molarity = 0.00936 mol / 0.050 L = 0.187 M
Therefore, the concentration (molarity) of iron (Fe^3+) in the solution is 0.187 M.
c. To determine the amount of iron (III) hydroxide that can be dissolved in 10.0 mL of 12.0 M HCl, we can use the same approach as in part a.
First, calculate the moles of HCl:
moles of HCl = Molarity × volume = 12.0 M × 0.010 L = 0.12 mol
Since the balanced equation indicates that 3 moles of HCl react with 1 mole of Fe(OH)3:
moles of Fe(OH)3 = 0.12 mol / (3 mol HCl / 1 mol Fe(OH)3) = 0.04 mol
Now, calculate the mass of Fe(OH)3 using the molar mass:
mass = moles × molar mass = 0.04 mol × 106.84 g/mol = 4.27 g
Therefore, approximately 4.27 grams of iron (III) hydroxide can be dissolved in 10.0 mL of 12.0 M HCl.
To solve these problems, we need to use stoichiometry and the concentration formula. Let's go step by step to find the answers.
a. How many milliliters of 1.00 M HCl are needed to dissolve 1.00 g of iron (III) hydroxide?
To solve this, we need to find the number of moles of iron (III) hydroxide, and then determine the volume of 1.00 M HCl needed to react with that amount.
First, let's calculate the moles of iron (III) hydroxide:
1. Convert the mass of iron (III) hydroxide to moles using its molar mass.
The molar mass of iron (III) hydroxide (Fe(OH)3) can be calculated by adding the atomic masses of its elements:
Fe: 55.845 g/mol
O: 15.999 g/mol (There are three oxygen atoms)
H: 1.00784 g/mol (There are three hydrogen atoms)
Therefore, the molar mass of Fe(OH)3 = mass of Fe + (3 x mass of O) + (3 x mass of H).
2. Calculate the moles of Fe(OH)3 using the formula: moles = mass/molar mass.
Now that we have the moles of Fe(OH)3, we can use stoichiometry to determine the volume of 1.00 M HCl required to react with it.
From the balanced equation you provided: Fe(OH)3(s) + 3H^+(aq) --> Fe^3+(aq) + 3H2O(l), we see that one mole of Fe(OH)3 reacts with three moles of H^+ (HCl). Therefore, the volume of 1.00 M HCl required can be calculated using the formula:
volume = moles of HCl / concentration of HCl.
b. If you added enough HCl to dissolve the 1.00 g of iron (III) hydroxide and then diluted the solution to 50.0 mL, what would the concentration (molarity) of iron be in the solution?
To find the concentration of iron (Fe^3+) in the final solution, we need to calculate the number of moles of iron and divide it by the final volume of the solution.
First, calculate the moles of iron (Fe^3+) produced. From the balanced equation, we know that one mole of Fe(OH)3 reacts to form one mole of Fe^3+. Use the moles of Fe(OH)3 calculated in part a to determine the number of moles of Fe^3+.
Finally, divide the moles of Fe^3+ by the final volume of the solution (given as 50.0 mL). Make sure to convert the volume to liters.
c. How many grams of iron (III) hydroxide can be dissolved in 10.0 mL of 12.0 M HCl?
To solve this problem, we will use stoichiometry and the concentration formula again.
First, we need to calculate the moles of HCl present in 10.0 mL of the solution. Use the formula: moles = concentration x volume (in liters).
From the balanced equation, we know that the molar ratio between Fe(OH)3 and HCl is 1:3. Therefore, one mole of Fe(OH)3 reacts with three moles of HCl.
Convert the moles of HCl to the moles of Fe(OH)3 using this ratio.
Lastly, calculate the mass of Fe(OH)3 in grams using the formula: mass = moles x molar mass.
Remember to always check your units and perform the appropriate conversions.
If you follow these steps, you should be able to find the answers to all three questions.