Question #171b9

1 Answer
anor277
Nov 24, 2015

About #26# #mL# of the magnesium solution.

Explanation:

#2HCl(aq) + Mg(OH)_2(s) rarr MgCl_2(aq) + 2H_2O(l)#

The equation above is balanced, and gives a stoichiometric picture of the reactivity. Two equiv hydrochloric acid are required to neutralize the magnesium salt.

If #35.75# #mL#, #0.175# #mol*L^-1# hydrochloric acid were used, then this represents a molar quantity of #35.75xx10^(-3)cancelLxx0.175# #mol*cancelL^-1# #=# #6.26xx10^(-3) mol# #HCl#.

By the stoichiometry of the reaction, there were thus #3.23xx10^(-3) mol# #Mg(OH)_2#.

We had #0.125# #mol*L^-1# magnesium hydroxide solution available; thus #(3.23xx10^-3 cancel(mol))/(0.125*cancel(mol)*L^-1)# gives an answer in litres (why?).

Related questions
See all questions in Neutralization
Impact of this question
1723 views around the world
You can reuse this answer
Creative Commons License