Commercially available concentrated hydrochloric acid is 37,0% w/w HCl

Commercially available concentrated hydrochloric acid is 37,0% w/w HCl. Its density is 1,18 g/mL. Using this information calculate, (a) the molarity of concentrated hcl and (b) the mass and volume (in mL) of solution containing 0,315 moles of HCl

The Correct Answer and Explanation is :

To solve this problem, we first determine the molarity of concentrated HCl, followed by calculating the mass and volume of the solution containing 0.315 moles of HCl.

Step 1: Molarity of Concentrated HCl

Given data:

• Mass percent of HCl = 37.0% w/w
• Density of solution = 1.18 g/mL
• Molar mass of HCl = 36.46 g/mol

1. Find the mass of HCl in 1 liter of solution:

• Mass of 1 L of solution = ( 1.18 \text{ g/mL} \times 1000 \text{ mL} )
  = 1180 g
• Mass of HCl in solution = ( 0.37 \times 1180 )
  = 436.6 g

1. Calculate the number of moles of HCl:
   [
   \text{Moles of HCl} = \frac{436.6}{36.46} = 11.98 \text{ moles}
   ]

• Molarity (M) = ( \frac{11.98}{1} ) = 11.98 M

Step 2: Mass and Volume of Solution Containing 0.315 Moles of HCl

We use the relation:
[
\text{Moles} = Molarity \times Volume (\text{in liters})
]

1. Calculate the volume required:
   [
   V = \frac{0.315}{11.98} = 0.0263 \text{ L} = 26.3 \text{ mL}
   ]
2. Calculate the mass of this volume of solution:

• Mass = Volume × Density
  [
  26.3 \text{ mL} \times 1.18 \text{ g/mL} = 31.1 \text{ g}
  ]

Final Answers:

• Molarity of concentrated HCl = 11.98 M
• Mass of solution containing 0.315 moles of HCl = 31.1 g
• Volume of solution required = 26.3 mL

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