Calculate the mass of anhydrous `HCI` in `10mL` of concentrated `HCI` (density `=1.2 g/mL`) solution having `37% HCI` by mass.

Options

A. `4.44g`
B. `4.44 mg`
C. `4.44 xx 10^(-3)`
D. `0.444 mug`

Answer

To solve the problem of calculating the mass of anhydrous HCl in 10 mL of concentrated HCl solution, follow these steps:

### Step 1: Calculate the mass of the HCl solution
We know the density of the HCl solution and its volume. The formula to calculate mass using density is:

\[ \text{Mass} = \text{Density} \times \text{Volume} \]

Given:
- Density of HCl solution = 1.2 g/mL
- Volume of HCl solution = 10 mL

Substituting the values:

\[ \text{Mass of HCl solution} = 1.2 \, \text{g/mL} \times 10 \, \text{mL} = 12 \, \text{g} \]

### Step 2: Calculate the mass of anhydrous HCl
Now that we have the mass of the HCl solution, we can calculate the mass of anhydrous HCl using the percentage by mass.

Given:
- Mass percentage of HCl = 37%

To find the mass of anhydrous HCl:

\[ \text{Mass of anhydrous HCl} = \text{Mass of solution} \times \left(\frac{\text{mass percentage}}{100}\right) \]

Substituting the values:

\[ \text{Mass of anhydrous HCl} = 12 \, \text{g} \times \left(\frac{37}{100}\right) = 12 \, \text{g} \times 0.37 = 4.44 \, \text{g} \]

### Final Answer
The mass of anhydrous HCl in 10 mL of concentrated HCl solution is **4.44 g**.

---