What volume of 0.500 M #NaOH# is needed to neutralize 45.0 mL of 0.400 M #HCl#?

1 Answer
anor277
May 3, 2016

#NaOH(aq) + HCl(aq) rarr NaCl(aq) + H_2O(l)#

Explanation:

Clearly there is a 1:1 equivalence, and as a first step we calculate the number of moles of hydrochloric acid:

#45.0xx10^-3*Lxx0.400*mol*L^-1# #=# #1.80xx10^-2*mol" hydrochloric acid"#.

We find an equivalent molar quantity of sodium hydroxide:

#(1.80xx10^-2*mol)/(0.500*mol*L^-1)xx10^3*mL*L^-1# #=# #36.0*mL#.

This volume is reasonable, in that it is LESS than the volume of the less concentrated acid.

Related questions
See all questions in Neutralization
Impact of this question
142894 views around the world
You can reuse this answer
Creative Commons License