This is a multi-part question. Part 1: Citric acid is a natural tri-protic organic acid that...

This is a multi-part question. Part 1: Citric acid is a natural tri-protic organic acid that has the generic formula of H3Cit, with the following Ka's: Ka1=8.4*10^-4, Ka2=1.8*10^-5, and Ka3=4.0*10^-6. If you start with a 0.2424 M solution of Na2HCit, write all of applicable chemical equations and the math equations, including all equilibria and mass and charge balance, that would be necessary to solve this?

Part 2: For the same citric acid problem above, what is the pH of the original Na2HCit solution?

Part 3: Can you use the shortcut equation here, and why?

Part 4: For the same citric acid system shown, what would be the actual molar concentration of all species present at pH=5.10, if you start with the same 0.2424 M Na2HCit solution?

Expert Solution

queen_honey_blossom answered 2 years ago

Citric Acid is a tri-protic acid with Ka1 = 8.4 x 10^-4 and Ka2 = 1.8...

Citric Acid is a tri-protic acid with Ka1 = 8.4 x 10^-4 and Ka2 = 1.8 x 10^-5 and Ka3 = 4.0 x 10^-6. a) Calculate the pH at the 2nd equivalence point in the titration of 100 mL of a 0.21 M Citric Acid solution with 0.25 M NaOH. b) Calculate the pH, after 15.8 mL of NaOH have been added. c) Calculate the pH, 5 mL after the LAST equivalence point.

Citric acid is a tri-protic acid with Ka1= 8.4x10^-4, Ka2= 1.8x 10^-5 Ka3= 4.0x 10^-6 a)...

Citric acid is a tri-protic acid with Ka1= 8.4x10^-4, Ka2= 1.8x 10^-5 Ka3= 4.0x 10^-6 a) calculate the pH at the 2dn equlivance point in the titration of 100.0 ml of 0.21M citric acid solution with 0.25M NaOH. Calculate the pH after 15.8 ml of NaOH has been added. c) calculate the pH 5.0 ml after the last equivalence point

Citric acid is an organic acid found in citrus fruits that is also a key intermediate...

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