how to make 3.0 liters of a 0.98 molar HCl solution from a 10.5 molar HCl stock solution.
c1v1 = c2v2
c = concn
v = volume
0.98M x 3.0L = 10.5M x ?L
Solve for ?L.
Take ?L of the 10.5M solution, add to a 3.0L volumetric flask and make to the mark with distilled water. The resulting solution will be 0.98M.
fft
To make 3.0 liters of a 0.98 molar HCl solution from a 10.5 molar HCl stock solution, you will need to perform a dilution. Dilution involves adding a calculated amount of solvent (usually water) to a known concentration of solute (stock solution) to achieve a desired lower concentration.
To calculate the amount of stock solution needed, you can use the formula:
C₁V₁ = C₂V₂
Where:
C₁ = initial concentration (molarity) of the stock solution
V₁ = initial volume of the stock solution
C₂ = final concentration of the diluted solution
V₂ = final volume of the diluted solution
In this case, you have:
C₁ = 10.5 M (Concentration of stock solution)
V₁ = ? (Volume of stock solution)
C₂ = 0.98 M (Desired final concentration)
V₂ = 3.0 L (Desired final volume)
Rearranging the formula to solve for V₁:
V₁ = (C₂ * V₂) / C₁
Plugging in the values:
V₁ = (0.98 M * 3.0 L) / 10.5 M
V₁ = 0.28 L
So, you need to measure 0.28 liters (280 mL) of the 10.5 molar HCl stock solution and then add water to a total volume of 3.0 liters to obtain a 0.98 molar HCl solution.