What is the molarity of the masonic acid solution? #H_2C_3H_2O_4 + 2NaOH -> Na_2C_3H_2O_4 + 2H_2O#

Question

A solution of malonic acid, #H_2C_3H_2O_4#, was standardized by titration with 0.1000 M #NaOH# solution. If 20.76 mL of the #NaOH# solution were required to neutralize completely 13.15 mL of the malonic acid...

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Answer 1 · 2016-07-07T16:58:31

#"Concentration of malonic acid "~=# #8xx10^-2*mol*L^-1#

#"Moles of NaOH"# #=# #0.1000*mol*L^-1xx20.76xx10^-3L=2.076xx10^-3*mol#

#"Concentration of malonic acid"# #=# #(1/2xx2.076xx10^-3*mol)/(13.15xx10^-3*L)# #=# #??mol*L^-1#

Note that I had to use #1/2xx2.076xx10^-3*mol" with respect to malonic acid"# as malonic acid is a diacid, #HO(O=C)CH_2C(=O)OH#.