How many moles of FeCl3.6H2O are required to make 10.00 mL of 1.50 M stock solution?
M = moles/L
Substitute and solve for moles.
1.5X10^-2
To calculate the number of moles of FeCl3.6H2O required, we need to use the equation:
moles = concentration × volume
Given:
Concentration of stock solution = 1.50 M
Volume of stock solution = 10.00 mL
First, we need to convert the volume from milliliters to liters:
10.00 mL = 10.00 × 10^-3 L (1 mL = 10^-3 L)
= 0.010 L
Now, we can calculate the number of moles using the equation:
moles = concentration × volume
= 1.50 M × 0.010 L
= 0.015 moles
Therefore, 0.015 moles of FeCl3.6H2O are required to make 10.00 mL of 1.50 M stock solution.
To determine the number of moles of FeCl3 · 6H2O required to make a 10.00 mL of 1.50 M stock solution, we need the molar mass of FeCl3 · 6H2O and the given concentration.
Here's how to calculate it step by step:
Step 1: Find the molar mass of FeCl3 · 6H2O:
The molar mass of FeCl3 is:
Fe: 55.85 g/mol
Cl: 35.45 g/mol
Adding them up:
Molar mass of FeCl3 = (3 × Cl) + Fe = (3 × 35.45) + 55.85 = 162.2 g/mol
To find the molar mass of 6H2O:
H: 1.01 g/mol
O: 16.00 g/mol
Adding them up:
Molar mass of water (H2O) = (2 × H) + O = (2 × 1.01) + 16.00 = 18.02 g/mol
Now, multiply the molar mass of water by 6:
Molar mass of 6H2O = (6 × H2O) = 6 × 18.02 = 108.12 g/mol
Finally, add the molar masses of FeCl3 and 6H2O to find the molar mass of FeCl3 · 6H2O:
Molar mass of FeCl3 · 6H2O = FeCl3 + 6H2O = 162.2 + 108.12 = 270.32 g/mol
Step 2: Calculate the number of moles using the given concentration and volume:
Moles = concentration × volume
Given concentration = 1.50 M
Given volume = 10.00 mL = 0.01000 L
Moles = 1.50 M × 0.01000 L = 0.0150 mol
Therefore, 0.0150 moles of FeCl3 · 6H2O are required to make a 10.00 mL of 1.50 M stock solution.