How do you calculate the mass of HCI required to prepare 2.5 liters of a 0.08 molar solution of HCI?

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Answer 1 · 2016-08-26T01:13:23

Easy.

$2.5$ $liters$ of a $0.08$ $molar$ solution of $HCI$ gives us $mol$ $es$ of $HCl$ in the solution

$Molarity$ * $Volume$ = $mol$ $es$

$0.08$ $(mol)/cancel L$ * $2.5 cancel L$ = $0.2 mol$ $es$ $HCl$

Now you must convert $mol$ $es$ to $grams$

$Molar$ $mass$ of $HCl$
$H = 1.01 (g)/(mol)$
$Cl = 35 (g)/(mol)$

$HCl = 1+35=36(g)/(mol)$

$(0.2 cancel mol)/1$ * $36 (g)/(cancel mol)$ = $color (red) (7.2 g)$ $HCl$