0.1825 g of Fe(NH4)2(SO4)2•6H2O is dissolved in 250.00 mL of solution; this is Solution A. 5.00 mL of Solution A is transferred to another flask, and it is diluted to a total of 100.0 mL to make another solution, which is Solution B. Next, 3.00 mL of Solution B is diluted to a total of 10.0 mL to make Solution C.
a) what is the molar concentration of Solution A?
b) what is the molar concentration of Solution B?
c) what is the molar concentration of Solution C?
mols Fe(NH4)2(SO4)2.6H2O = grams/molar mass = ?. Then (A) = mols /L = ? Let's call this Y.
(B) = (A) x (5.00/100) = ?
(C) = done the same way as (B).
To find the molar concentration of each solution, we need to calculate the number of moles of Fe(NH4)2(SO4)2•6H2O in each solution, and then divide this value by the volume of the solution in liters.
a) To find the molar concentration of Solution A:
1. Calculate the number of moles of Fe(NH4)2(SO4)2•6H2O in Solution A:
- Mass of Fe(NH4)2(SO4)2•6H2O = 0.1825 g
- Molar mass of Fe(NH4)2(SO4)2•6H2O = (55.85 g/mol * 1) + (14.01 g/mol * 2) + (32.07 g/mol * 2) + (16.00 g/mol * 2 * 6) = 392.14 g/mol
- Moles of Fe(NH4)2(SO4)2•6H2O in Solution A = Mass / Molar mass = 0.1825 g / 392.14 g/mol
2. Convert the volume of Solution A to liters:
- Volume of Solution A = 250.00 mL = 250.00 mL * (1 L / 1000 mL)
3. Calculate the molar concentration of Solution A:
- Molar concentration of Solution A = Moles / Volume = Moles / (Volume in liters)
b) To find the molar concentration of Solution B, you will repeat the same steps as for Solution A, using the given values for Solution B.
c) To find the molar concentration of Solution C, you will repeat the same steps as for Solution A, using the given values for Solution C.
Note: The molar concentration is expressed in units of moles per liter (mol/L) or molarity (M).