What reaction occurs when 25.0 mL of 0.600 M NaOH are mixed with 15.0 mL of 0.400 M HNO3? What is the balanced equation and the net ionic equation?

1 Answer
anor277
Mar 8, 2016

The net ionic equation is simply:

#H_3O^+ + ""^(-)OH rarr 2H_2O(l)#

Explanation:

The sodium ions and the nitrate ions are simply along for the ride.

Of course, it is clear that there is an excess of base.

Moles of #NaOH# #=# #25.0xx10^-3*Lxx0.600*mol*L^-1# #=# #??mol#

Moles of #HNO_3# #=# #15.0xx10^-3*Lxx0.400*mol*L^-1# #=# #??mol#

The balanced equation is:

#NaOH(aq) + HNO_3(aq) rarr NaNO_3(aq) + H_2O(l)#.

I leave it to you to calculate the end concentration of sodium hydroxide. Remember, you have added the volumes so now the volume of the solution is #40.0# #mL#.

Related questions
See all questions in Main Characterstics or Lewis/Bronsted Definition
Impact of this question
1329 views around the world
You can reuse this answer
Creative Commons License