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.

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