A commercially sold conc. HCl is 35% HCl by mass. If the density of this commercial acid is 1.46 g/mL, the molarity of this solution is:
(Atomic mass : Cl = 35.5 amu, H = 1 amu)
Solution
<p>35% HCl by mass means in 100 gm HCl solution 35 gm HCl present.</p>
<p>Now, volume of 100 gm HCl solution</p>
<p>$= {{100} \over {1.46}}$ ml</p>
<p>$= {{{{100} \over {1.46}}} \over {1000}}$ l</p>
<p>Moles of HCl $= {{35} \over {36.5}}$</p>
<p>Now, molarity $= {{moles\,of\,solute} \over {volume\,of\,solution\,(in\,L)}}$</p>
<p>$= {{{{35} \over {36.5}}} \over {{{{{100} \over {1.46}}} \over {1000}}}} = 14$</p>
About this question
Subject: Chemistry · Chapter: Some Basic Concepts of Chemistry · Topic: Mole Concept
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