Benzene-1,2,3-tricarboxylic acid (C6H3 (CO2H) 3) is a three-protic, water-soluble carboxylic acid with the following pKa values: pKa1 = 2.86, pka2 = 4.30 and pka3 = 6.28. What will be the pH of a 0.075 M solution of this treprotic carboxylic acid?
pH of the solution has been calculated.
Benzene-1,2,3-tricarboxylic acid (C6H3 (CO2H) 3) is a three-protic, water-soluble carboxylic acid with the following pKa values:...
Benzene-1,2,3-tricarboxylic acid (C6H3 (CO2H) 3) is a three-protic, water-soluble carboxylic acid with the following pKa values: pKa1 = 2.86, pka2 = 4.30 and pka3 = 6.28. What will be the pH of a 0.075 M solution of this treprotic carboxylic acid?
How much volume of a 0.102 M NaOH solution must be added to 25.00 ml of a 0.075 M solution of benzene-1,2,3-tricarboxylic acid to obtain a pH equal to 4.80? pKa values: pKa1 = 2.86, pka2 = 4.30 and pka3 = 6.28.
I am unsure as to how to solve this problem.Spectrophotometric properties of a particular indicator are given below. A solution with a volume of 20.0 mL containing 1.40 times 10^-5 M indicator plus 0.050 M benzene-1, 2, 3-tricarboxylic acid (pKa1 = 2.86, pKa2 = 4.30, pKa3 = 6.28) was treated with 20.0 ml. of aqueous KOH. The resulting solution had an absorbance at 604 nm of 0.118 in a 1.00 cm cell. Calculate the molarity of the KOH solution.
Phosphoric acid is a triprotic acid with the following pKa values: pKa1=2.148 pKa2=7.198 pKa3=12.375 You wish to prepare 1.000 L of a 0.0100 M phosphate buffer at pH 7.580. To do this, you choose to mix the two salt forms involved in the second ionization, NaH2PO4 and Na2HPO4, in a 1.000 L volumetric flask and add water to the mark. What mass of each salt will you add to the mixture? Mass NaH2PO4=? Mass Na2HPO4=?
Using Pauling’s rules, calculate the pKa values (all) of following acids: (PKa1,Pka2 or pka3 if acid is polyprotic) H3PO4, H3PO3 and H3PO2
Arsenic acid is a triprotic acid with the following pKa values: pKa 1 = 2.240; pKa2 = 6.960; pKa3 = 11.500. You wish to prepare 1.000 L of a 0.0400 M aresenate buffer at pH 10.430. To do this, you choose to mix the two salt forms involved in the second ionization, Na3AsO4 and Na2HAsO4, in a 1.000 L volumetric flask and add water to the mark. What mass of each salt will you add to the mixture?
Orthophosphate (PO4 3- ) is a soluble polyprotic acid capable of protonating/deprotonating up to 3 protons to produce aqueous H3PO4 0 , H2PO4 - , HPO4 2- and PO4 3- . The pKa values of the associated dissociation reactions are as follows: pKa1=2.1; pKa2 = 7.2; and pKa3 = 12.4. Here you are asked to construct the speciation diagram of orthophosphate showing the concentrations of each of the four orthophosphate species in the pH range 1 -14 for a solution...
A novel triprotic acid (3 carboxylic acids) has pKa1 = 3.0, pKa2 = 5.0, and pKa3 = 6.50. At pH = 4.0, what is the APPROXIMATE percentage of Acid(2H)- (loss of 1 proton) versus total amount of Acid in solution? a. 50% b. 80% c. 0% d. 25% e. 90%
Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.300 M phosphoric acid solution. pKa1 pKa2 pKa3 2.16 7.21 12.32 [H3PO4]= M [H^+]= M [H2PO4 ^−]= M [OH^−]= M [HPO4 ^2−]= M pH= [PO4 ^3−]= M
Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH, and the concentrations of all species in a 0.500 M phosphoric acid solution. pKa1= 2.16 pKa2 = 7.21 pKa3 = 12.32 What's: H3PO4, H2PO4-, HPO4-2, PO4-3, H+ ,OH- , pH