_______g of MnSO4 H2O are needed to prepare a solution of 100.00mL of 0.100 M MnSO4.
Thank You
tried using M1V1=M2V2 but without sucess
You want 100 mL of 0.100 M MnSO4.H2O. How many moles is that? M x L = moles.
How many grams is that? moles = grams/molar mass.
oh thanks I get it now..
To calculate the grams of MnSO4 H2O needed to prepare a solution of 100.00 mL of 0.100 M MnSO4, we need to use the formula:
Molarity (M) = moles/volume (L)
First, let's find the moles of MnSO4 in the solution:
Moles = Molarity (M) × Volume (L)
Volume (L) = Volume (mL) / 1000
Since the volume is given as 100.00 mL, converting it to liters:
Volume (L) = 100.00 mL / 1000 = 0.100 L
Now, let's calculate the moles of MnSO4:
Moles of MnSO4 = Molarity (MnSO4) × Volume (L)
Given that the molarity of MnSO4 is 0.100 M:
Moles of MnSO4 = 0.100 M × 0.100 L = 0.010 moles
Next, we need to determine the molar mass of MnSO4 H2O. The molar mass of MnSO4 is 151.00 g/mol, and the molar mass of water (H2O) is 18.015 g/mol.
Molar mass of MnSO4 H2O = 151.00 g/mol + (2 × 1.008 + 16.00) g/mol = 169.02 g/mol
Now, we can calculate the grams of MnSO4 H2O needed:
Grams = Moles × Molar mass
Grams = 0.010 moles × 169.02 g/mol = 1.690 g
Therefore, 1.690 grams of MnSO4 H2O are needed to prepare a solution of 100.00 mL of 0.100 M MnSO4.