Calculate mass of silver nitrate needed to prepare a solution of concentration 0.01 moles per liter.
How much do you want to prepare?
moles needed = M x L = ??
Then moles = grams/molar mass.
1.47×10^-5
To calculate the mass of silver nitrate needed to prepare a solution of a specific concentration, we can use the formula:
Mass = Molarity × Volume × Molar mass
First, let's determine the molar mass of silver nitrate (AgNO3).
Ag (silver) has a molar mass of 107.87 g/mol.
N (nitrogen) has a molar mass of 14.01 g/mol.
O (oxygen) has a molar mass of 16.00 g/mol.
So, the molar mass of AgNO3 is:
Ag: 107.87 g/mol
N: 14.01 g/mol
O: 16.00 g/mol × 3 (since there are 3 oxygen atoms in AgNO3)
Molar mass of AgNO3 = 107.87 g/mol + 14.01 g/mol + (16.00 g/mol × 3) = 169.87 g/mol
Now, let's calculate the mass of silver nitrate needed.
Given:
Concentration (C) = 0.01 moles per liter (mol/L)
Volume (V) = 1 liter (L)
Molar mass (M) = 169.87 g/mol
Mass (m) = C × V × M
= 0.01 mol/L × 1 L × 169.87 g/mol
= 1.6987 g
Therefore, you would need 1.6987 grams of silver nitrate to prepare a solution of concentration 0.01 moles per liter.