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Commercially availiable concentrated hydrochloric acid contains `38% HCl` by mass. (a) What is the molarity of this solution? The density is `1.19g mL^(-1)` ? (b) What volume of concentrated `HCl` is required to make `1.00 "litre"` of `0.10M HCl`? |
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Answer» (a) `"Mass of" HCl= 38 g`, `"density of solution"=1.19g//mL`, `"Mass of solution" -100 g` `"Molarity"=("Moles of"HCl)/("Volume of solution in litre")` `=("Mass of "HCl)/("Molar mass of "HClxx("Weight of solution")/("density of solution"xx1000))` `=(38)/(36.5xx(100)/(1.19xx1000))=12.4` (b) MIlli-moles of solute does not change on dilution and this, `{:(MxxV_(mL),=,MxxV_(mL),,),("(for conc.)",=,"(for dil)",,):}` `12.4xxV= 0.1xx100 ` `V= 8.06mL` |
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