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

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...

Answer 1

#"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#.

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Answer 2

Xavier Avery

To determine the molarity of the oxalic acid solution (H2C2O4), you need to know the volume of the solution and the number of moles of oxalic acid present. You can calculate the number of moles of oxalic acid by using the stoichiometry of the reaction and the concentration of the sodium hydroxide (NaOH) solution used to titrate the oxalic acid solution.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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

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...

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