Explain the effect of the pH on the protonation of the functional groups present in ascorbic acid (C6H8O6) and citric acid (C6H8O7).

You have 1 M (1 mol/L) solution of amino acid. This amino acid has an alpha carboxyl group with pKa = 2.0 and an alpha- amino group with pKa = 10.0. The pH of the solution is 7.0. Calculate the concentration of the molecular form of this amino acid that has carboxyl group protonated (COOH) and, at the same time, the amino group deprotonated (NH2).

Pleas give the structure of the major organic product in the reaction

M11.

Alanine (HA) is a diprotic amino acid with Kal = 4.53 x 10-3 and K₁2 = 1.36 x 10-10. Determine the pH of each of the solutions. A 0.241 M alanine hydrochloride (H₂A+CI-) solution. pH = A 0.241 M alanine (HA) solution. pH = A 0.241 M sodium alaninate (Na+ A¯) solution. pH =

Write the molecular equation for the reaction of CH3COOH  and NaOH. Write the net ionic equation for the reaction of CH3COOH and NaOH.

Calculate the ratio of dihydrogen phosphate to hydrogen phosphate in blood at pH 7.4. The Ka is 6.3 × 10−8.

Write the acidic equilibrium equation for HC₆H₅CO₂

What is the equilibrium constant for the following reaction that occurs when disodium citrate(Na2HC6H5O7) dissolves in water at 25ºC? The acid dissociation constants for citric acid, H3C6H5O7 , are:Ka1 = 7.4 × 10–4 , Ka2 =1.7 × 10–5 , and Ka3 = 4.0 × 10–7 . HC6H5O72– (aq) + H2O(l) ⇌ H2C6H5O7– (aq) + OH– (aq)

For an acid HA with a pKa of 5.2, what is the ratio of the concentration of the conjugate base to that of the acid at pH 7.2.