Explain how t make 1.5L of a 2.25M solution of H2SO4 from 6.0M stock solution.
How many moles do you need in the diluted solution? That will be M x L = ??
So you must use?? moles of the stock to obtain that. M stock = moles stock/L stock. You know moles and M, solve for L.
thank you!
To make 1.5L of a 2.25M solution of H2SO4 from a 6.0M stock solution, you will need to dilute the stock solution with a suitable amount of solvent. Here are the steps to calculate the required volumes:
1. Determine the number of moles of H2SO4 needed in the final solution.
Number of moles = Molarity × Volume
The number of moles of H2SO4 in the final solution is given by:
Moles = Molarity × Volume
= 2.25 M × 1.5 L
= 3.375 moles
2. Calculate the volume of the stock solution required using the equation:
Volume of stock solution = Moles ÷ Molarity
Volume = 3.375 moles ÷ 6.0 M
= 0.5625 L
3. Subtract the volume of the stock solution from the total desired volume to determine the amount of solvent needed.
Solvent volume = Total volume - Volume of stock solution
= 1.5 L - 0.5625 L
= 0.9375 L (or 937.5 mL)
So, to make 1.5L of a 2.25M solution of H2SO4 from a 6.0M stock solution, you will need to mix 0.5625L (or 562.5 mL) of the stock solution with 0.9375L (or 937.5 mL) of a suitable solvent, such as water.