Prepare 1m HCl the purity of HCl is 36%
Understand the Problem
The question is asking how to prepare a 1M solution of hydrochloric acid (HCl) using an HCl solution that has a purity of 36%. It requires calculating the volume of the concentrated HCl needed and diluting it with a suitable solvent (usually water) to achieve the desired molarity.
Answer
$83.3 \, \text{mL}$
Answer for screen readers
$83.3 , \text{mL}$
Steps to Solve

Determine the molarity and density of the concentrated solution To calculate the volume of the concentrated HCl needed, we first need to know the density and molarity of the concentrated HCl solution. A 36% HCl solution typically has a density of about $1.18 , \text{g/mL}$ and a molarity of about $12 , \text{M}$.

Calculate the amount of HCl required for a 1M solution To make a 1M solution, use the formula: $$ C_1V_1 = C_2V_2 $$ Where:
 $C_1$ is the concentration of the concentrated solution ($12 , \text{M}$),
 $V_1$ is the volume of the concentrated solution we need to find,
 $C_2$ is the desired concentration ($1 , \text{M}$),
 $V_2$ is the final volume of the diluted solution (let's assume $1 , \text{L}$).
Rearranging the formula gives:
$$ V_1 = \frac{C_2 \times V_2}{C_1} $$

Substituting the values into the equation Now we plug in the values we have:
$$ V_1 = \frac{1 , \text{M} \times 1 , \text{L}}{12 , \text{M}} $$ 
Calculating the volume of concentrated HCl needed Calculating gives:
$$ V_1 = \frac{1}{12} , \text{L} = 0.0833 , \text{L} $$ Convert this to mL by multiplying by 1000:
$$ V_1 = 0.0833 , \text{L} \times 1000 , \text{mL/L} = 83.3 , \text{mL} $$ 
Prepare the solution Measure $83.3 , \text{mL}$ of the concentrated HCl solution and dilute it with water until the total volume reaches $1 , \text{L}$.
$83.3 , \text{mL}$
More Information
To prepare a 1M solution from a concentrated 36% HCl solution requires careful measurements and safety precautions, as HCl is a strong acid. Always add acid to water, never the other way around, to prevent exothermic reactions that could cause splattering.
Tips
 Not using the correct density or molarity for the concentrated solution.
 Forgetting to account for the final volume when calculating the dilution.
 Adding water to the concentrated acid instead of the acid to the water, which can be dangerous.
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