Hi,
A bottle of concentrated Hydrochloric acid (HCl) has the following information stated on it: -
Hydrochloric acid 37%
1L ~ 1190kg
How do I prepare 0.1N HCl from this concentrated HCl?
Normality = equivalents/liter of solution.
I think 1 L has a mass of 1.190 kg (or 1190 grams), not 1190 kg.
Of that 1190, how much is HCl.
1190 g x 0.37 = y grams HCl
How many equivalents is that?
y/equivalent mass (and in this case, equivalent mass and molar mass are the same) so y/approx 36.5 (but you do it exactly) = z so the normality is z/1 L = same as z normal which should be about 12 N.
Now just use the dilution formula.
12N*volume = 0.1N*volume you want to prepare.
To prepare 0.1N HCl (Hydrochloric acid) solution from the concentrated HCl (37%), you will need to perform the following steps:
Step 1: Determine the molecular weight of HCl.
The molecular weight of HCl is calculated by adding the atomic weights of hydrogen (H) and chlorine (Cl). The atomic weight of hydrogen is approximately 1 gram/mole, and the atomic weight of chlorine is approximately 35.5 grams/mole. Therefore, the molecular weight of HCl is 1 + 35.5 = 36.5 grams/mole.
Step 2: Convert the concentration of the concentrated HCl to molarity.
The concentration of the concentrated HCl is given as 37%. This means that 100 mL of the solution contains 37 grams of HCl. However, since the provided value is in terms of volume percent, we need to convert it to weight percent before proceeding to calculate the molarity.
To convert the volume percent to weight percent, we need to determine the density of the concentrated HCl. The density value provided on the bottle is 1190 kg/L. Since 1 L of solution weighs 1190 kg, the weight of the concentrated HCl can be calculated as follows:
Weight of concentrated HCl = (Volume of concentrated HCl x Density of concentrated HCl)
Weight of concentrated HCl = (1L x 1190 kg/L) = 1190 kg
Hence, the weight percent can be calculated by dividing the weight of HCl by the weight of the solution:
Weight percent = (Weight of HCl / Weight of solution) x 100 = (37 / 1190) x 100 = 3.11%
Now, to calculate the molarity, we need to convert the weight percent to molarity using the molecular weight:
Molarity in terms of weight percent = (Weight percent x 10) / Molecular weight
Molarity = (3.11 x 10) / 36.5 = 0.852 M
Step 3: Calculate the volume of concentrated HCl required.
To prepare 0.1N HCl from the concentrated HCl, we need to calculate the volume of the concentrated HCl required. The equation for molarity is:
Molarity = (Number of moles of solute) / (Volume of solution in liters)
Rearranging the equation:
Number of moles of solute = (Molarity) x (Volume of solution in liters)
Number of moles of solute = (0.1) x (1) = 0.1 moles
To calculate the volume of concentrated HCl required, we use the equation:
(Number of moles of solute) = (Concentration of concentrated HCl in moles/L) x (Volume of concentrated HCl in L)
Rearranging the equation:
Volume of concentrated HCl in L = (Number of moles of solute) / (Concentration of concentrated HCl in moles/L)
Volume of concentrated HCl in L = 0.1 moles / 0.852 moles/L = 0.117 L (or 117 mL)
Therefore, to prepare 0.1N HCl solution, mix 117 mL of the concentrated HCl with distilled water and then make up the final volume to 1 liter.