How much SrCl2 is needed to make 100ml of 2.0 molar SrCl2 solution?
How many mols do you need? That's mols = M x L = ?
Then mols = grams/molar mass. You know mols and molar mass, solve for grams.
molar means moles per liter of solution
0.1 L of 2.0 M solution contains 0.2 moles of solute
To calculate the amount of SrCl2 needed to make a 2.0 molar solution in 100 ml, you'll need to know the molar mass of SrCl2 and use the formula:
Amount (in moles) = concentration (in moles/liter) * volume (in liters)
First, determine the molar mass of SrCl2 by adding up the atomic masses of strontium (Sr) and chlorine (Cl). The atomic mass of Sr is 87.62 g/mol, and the atomic mass of Cl is 35.45 g/mol.
Molar mass of SrCl2 = 87.62 g/mol + 2*(35.45 g/mol) = 147.02 g/mol
Next, convert the volume from milliliters (ml) to liters (L) by dividing by 1000:
Volume (in liters) = 100 ml / 1000 = 0.1 L
Now, use the formula mentioned earlier to calculate the amount of SrCl2:
Amount (in moles) = 2.0 mol/L * 0.1 L = 0.2 moles
Finally, to find the mass of SrCl2 needed, multiply the amount in moles by the molar mass:
Mass = Amount (in moles) * Molar mass
= 0.2 moles * 147.02 g/mol
= 29.4 grams
Therefore, you will need 29.4 grams of SrCl2 to make a 2.0 molar solution in 100 ml.