Prepare 1m HCl the purity of HCl is 36%

Steps to Solve

1. 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 $12 , \text{M}$.

2. 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:
$$ V_1 = \frac{C_2 \times V_2}{C_1} $$

3. Substituting the values into the equation Now we plug in the values we have:
   $$ V_1 = \frac{1 , \text{M} \times 1 , \text{L}}{12 , \text{M}} $$

4. 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:
   $$ V_1 = 0.0833 , \text{L} \times 1000 , \text{mL/L} = 83.3 , \text{mL} $$

5. Prepare the solution Measure $83.3 , \text{mL}$ of the concentrated HCl solution and dilute it with water until the total volume reaches $1 , \text{L}$.