what mass of silver nitrate is needed to prepare 100cm3 of silver nitrate solution,
concentration 0.2mol/dm3?
the mass of one mole of silver nitrate is 170g
How many mols do you need? That's M x L = mols
Then mols = grams/molar mass. You know mols and molar mass, calculate grams.
To calculate the mass of silver nitrate needed, we need to use the formula:
mass = number of moles × molar mass
Given:
Volume of silver nitrate solution (V) = 100 cm³ = 100/1000 dm³ = 0.1 dm³
Concentration of silver nitrate solution (C) = 0.2 mol/dm³
Molar mass of silver nitrate (M) = 170 g/mol
First, let's calculate the number of moles of silver nitrate needed:
moles = concentration × volume
moles = 0.2 mol/dm³ × 0.1 dm³
moles = 0.02 mol
Now, we can calculate the mass of silver nitrate:
mass = moles × molar mass
mass = 0.02 mol × 170 g/mol
mass = 3.4 g
Therefore, to prepare 100 cm³ of a silver nitrate solution with a concentration of 0.2 mol/dm³, you will need 3.4 grams of silver nitrate.
To find the mass of silver nitrate needed to prepare 100 cm3 of a solution with a concentration of 0.2 mol/dm3, we need to calculate the number of moles required first.
Step 1: Calculate the number of moles:
The formula to calculate the number of moles is:
Number of moles = Concentration x Volume
Given:
Concentration = 0.2 mol/dm3
Volume = 100 cm3 (which needs to be converted to dm3)
To convert cm3 to dm3, divide the volume by 1000:
Volume (in dm3) = 100 cm3 / 1000 = 0.1 dm3
Now we can calculate the number of moles:
Number of moles = 0.2 mol/dm3 x 0.1 dm3 = 0.02 moles
Step 2: Calculate the mass of silver nitrate:
It is given that the molar mass of silver nitrate is 170g/mol.
To find the mass, use the formula:
Mass = Number of moles x Molar mass
Mass = 0.02 moles x 170 g/mol = 3.4 grams
Therefore, you would need 3.4 grams of silver nitrate to prepare 100 cm3 of a silver nitrate solution with a concentration of 0.2 mol/dm3.