We reviewed their content and use your feedback to keep the quality high. The pH of the solution at the first equivalence point. The major industrial use of maleic acid is its conversion to fumaric acid. Be careful. The lower the pKa of a Bronsted acid, the more easily it gives up its proton. I could just take 10^-pKa1 and get the answer? These values reveal the deprotonation state of a molecule in a particular solvent. Ka2 can be calculated from the pH . If we know which sites bind protons more tightly, we can predict in which direction a proton will be transferred. The pKa measures how tightly a proton is held by a Bronsted acid. "Experimental" often implies to students "untested" or "unreliable", but here it means that someone has done the work to measure how tightly the proton is bound. 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Can someone please explain what the difference between pKa v. pKa1 and pKa2 is? Maleic acid is a weak diprotic acid with : pK a1 = 1.87 pK a2 = 6.07 A 10.00 mL solution of 0.1000 M maleic acid is titrated with 0.1000 M NaOH. Additionally, per the publisher's request, their name has been removed in some passages. It is a weak Bronsted acid. A third method involves the reaction of maleic anhydride with glycolic acid or glycine to produce 2,3-dihydroxysuccinic acid. A proton, H+, is a strong Lewis acid; it attracts electron pairs very effectively, so much so that it is almost always attached to an electron donor. If the chemistry of protons involves being passed from a more acidic site to a less acidic site, then the site that binds the proton more tightly will retain the proton, and the site that binds protons less tightly will lose the proton. A 10.00 mL solution of 0.1000 M maleic acid is titrated with Both are di-carboxylic acid, so they can donate proton twice and have pka1 and pka2 Maleic acid HO 2 CCH=CHCO 2 H (aq) ---> HO 2 CCH=CHCO 2 - (aq)+ H + (aq) pka1 =1.9 In industry, maleic acid is derived by hydrolysis of maleic anhydride, the latter being produced by oxidation of benzene or butane. 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