A student wants to prepare 0.5M HCl. The label of a commercial hydrochloric acid shows that S.G.=1.18 and concentration of HCl is 37%. Calculate the volume of commercial hydrochloric acid dose the chemist requires to make up 1.5L of the dilute acid.
So, sg 1.18
so 1 liter has a mass of 1180 grams. 37 percent or 437 grams of HCL, and the remander is water.
Molarity of HCL=(437/36.5)/1=11.97 or in sig figs, 12.0
So you want to dilute it 12/.5=24 times
which means one part acid, 23 parts water.
how much is one part? well, 24 parts is 1.5 L, so one part=1.5/24=62.5 ml of acid, and 1.435 liters of water. Alsways add acid to water, stir, and label.
To calculate the volume of commercial hydrochloric acid required to make up 1.5L of a 0.5M HCl solution, we need to use the known information about the concentration and specific gravity (S.G.) of the commercial hydrochloric acid.
Here's how you can calculate the volume:
Step 1: Calculate the amount of HCl required in moles:
The molarity (M) of a solution is defined as the number of moles of solute per liter of solution. Since we want to prepare a 0.5M HCl solution, we need to determine the amount of HCl in moles that will be needed for 1.5L of the solution.
Molarity (M) = moles of solute / volume of solution (in liters)
0.5M = moles of HCl / 1.5L
Rearranging the equation to solve for moles of HCl:
moles of HCl = Molarity (M) x volume of solution (in liters)
moles of HCl = 0.5M x 1.5L
Step 2: Calculate the mass of HCl required:
To calculate the mass of HCl required, we need to know the molar mass of HCl, which is the sum of the atomic masses of hydrogen and chlorine.
Molar mass of HCl = 1g/mol (hydrogen) + 35.5g/mol (chlorine) = 36.5g/mol
mass of HCl = moles of HCl x molar mass of HCl
Step 3: Calculate the volume of commercial hydrochloric acid:
Based on the concentration of HCl in the commercial hydrochloric acid and the mass of HCl required, we can determine the volume of commercial hydrochloric acid needed.
Concentration = mass of solute / volume of solution (in liters)
37% (in decimal form) = mass of HCl / volume of commercial hydrochloric acid
Rearranging the equation to solve for the volume of commercial hydrochloric acid:
volume of commercial hydrochloric acid = mass of HCl / concentration
volume of commercial hydrochloric acid = (mass of HCl required) / (concentration)
Plug in the known values and calculate the final result.
Note: The specific gravity (S.G.) is not required in this calculation as it only indicates the density of the commercial hydrochloric acid compared to the density of water.
I hope this explanation helps you understand the process of calculating the volume of commercial hydrochloric acid required to make up the dilute acid solution.