General Chemistry
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What is the pH and [H+] of a 0.24 M H3A (Ka1 = 6.3x10-3, Ka2 = 5.9x10-8, Ka3 = 2.2x10-12) polyprotic acid solution?
A solution containing HCl and H3AsO4 was prepared. A 50.00 mL sample of this solution was titrated using 0.100 M NaOH. The first and second equivalence points were reached after the addition of 125.00 mL and 175.00 mL of the base, respectively. Which of the following is the approximate pH titration curve for the given scenario?
Commonly found in cola drinks, phosphoric acid (H3PO4) is a triprotic acid. If a sample of cola has a pH of 2.80 and the total concentration of phosphoric acid species is 0.500 M, what are the concentrations of H3PO4, H2PO4-, HPO42-, and PO43-? The Ka values for phosphoric acid are: Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13.
Calculate the pH and the molarities of all species (H3AsO4, H2AsO3–, HAsO42–, AsO43–, H3O+, and OH–) in a 9.50 % (by mass) solution of arsenic acid with a density of 1.1033 g/mL. The equilibrium constants are:
Ka1 = 6.46×10–3
Ka2 = 1.14×10–7
Ka3 = 3.16×10–12
Arsenic acid is a tripotic acid. What is the pH of a 0.035 M solution of arsenic acid?
Determine the pH of 0.75 M Na3PO4 if the Ka values are given as:
Ka1 = 5.7 × 10− 3, Ka2 = 1.1 × 10− 7, Ka3 = 3.2 × 10− 12