In this acid base reaction: #NaOH+HCl->NaCl+H_2O#, if we measured out 10.0 mL of a 2.0 M solution of #HCl#, how many grams of sodium hydroxide(#NaOH#; MW=40 g/mol) would we need to neutralize the #HCl# solution?

1 Answer
anor277
Sep 27, 2016

#0.8*g# of sodium hydroxide are required.

Explanation:

You have the stoichiometric equation. There is clearly 1:1 equivalence. Thus #"moles of hydrochloric acid"# #=# #"moles of sodium hydroxide"#.

#"Moles of hydrochloric acid"# #=# #10.0xx10^-3Lxx2.0*mol*L^-1# #=# #0.020# #mol# #HCl#.

#"Mass of sodium hydroxide req'd"# #=# #0.020*molxx40.00*g*mol^-1# #=# #0.80*g#.

It would be hard to measure such a quantity of sodium hydroxide as it is deliquescent, and once removed from the tin (or if the tin is poorly sealed), it would absorb moisture from the atmosphere.

Related questions
See all questions in Main Characterstics or Lewis/Bronsted Definition
Impact of this question
2126 views around the world
You can reuse this answer
Creative Commons License