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Chapter 12: Problem 106

Concentrated hydrochloric acid is usually available at a concentration of 37.7 percent by mass. What is its molar concentration? (The density of the solution is \(1.19 \mathrm{~g} / \mathrm{mL} . ?\)

Short Answer

Expert verified
The molar concentration of the solution is \(12.3 \mathrm{~M}\).

Step by step solution

01

Convert mass percent to fraction

Mass/mass % needs to be converted into a fraction for the purpose of calculations. Here, the given mass percent is 37.7%, so the fraction would be \(0.377\). This implies that there is 0.377 g of HCl for every 1 g of solution.
02

Compute mass of HCl in 1mL solution

Using the given density of the solution as 1.19 g/mL, multiply this by the fraction of the HCl in the solution to get the amount of HCl in one mL of solution. So, \(1.19 \mathrm{~g/mL} \times 0.377 \) = \(0.448 \mathrm{~g}\) of HCl per mL of solution.
03

Convert grams to moles

To find the molar concentration, it is necessary to convert the mass of HCl to moles. Use the molar mass of HCl, 36.46 g/mol. Therefore, \(0.448 \mathrm{~g} \div 36.46 \mathrm{~g/mol} = 0.0123 \mathrm{~moles}\) of HCl per mL.
04

Convert volume from mL to L

Lastly, convert the volume from mL to L since molar concentration is measured in mol/L. There are 1000 mL in a liter, so \(0.0123 \mathrm{~mol/mL} \times 1000 = 12.3 \mathrm{~M}\) Molar concentration.

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Most popular questions from this chapter

Calculate the amount of water (in grams) that must be added to (a) \(5.00 \mathrm{~g}\) of urea \(\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}\) in the preparation of a 16.2 percent by mass solution, and (b) \(26.2 \mathrm{~g}\) of \(\mathrm{MgCl}_{2}\) in the preparation of a 1.5 percent by mass solution.

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