In the titration of 250.0 mL of 0.20 M H3PO4 with 0.10 M NaOH, the pH of the solution after the addition of some NaOH is 4.66. Which of the following phosphate-containing species is present in the largest
amount? For H3PO4, Ka1 = 7.5 × 10–3, Ka2 = 6.2 × 10–8, and Ka3 = 4.8 × 10–13.
In the titration of 250.0 mL of 0.20 M H3PO4 with 0.10 M NaOH, the pH...
What is the equilibrium pH of a 0.515 M solution of H3PO4 (aq)? (Ka1 = 7.5 × 10–3 , Ka2 = 6.2 × 10–8 , Ka3 = 4.8 × 10–13) a. 1.23 b. 3.75 c. 12.32 d. 6.30 e. 7.21
5. Calculate the pH at 25°C of a 0.85 M aqueous solution of phosphoric acid (H3PO4). 5. (Ka1, Ka2, and Ka3 for phosphoric acid are 7.5 × 10−3, 6.25 × 10−8, and 4.8 × 10−13, respectively.)
Question 3: Draw the titration curve (pH versus mL of NaOH added) that would be obtained from the titration of 30 mL of a 0.10 M solution of an unknown triprotic acid, H3A (Kat = 1.26 x 10-3; Ka2 = 5.6 x 10-6, Ka3 = 3.32 x 10-10) with 0.10 M NaOH. Indicate the volume needed to reach the first second, and third equivalence points and the pH at the half equivalence points for the three titration regions.
Question 15 0/4 pts The acid ionization constants of phosphoric acid (H3PO4) are Ka1 = 7.5 x 10-3. Ka2 = 6.2 x 10-8 and Ka3 - 4.2 x 10-13 at 25.0°C. What is the molar concentration of phosphate ion in a 2.5 M aqueous solution of phosphoric acid?
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added, the pH of the resulting solution was 6.70. After 50.0 mL of NaOH was added, the pH of the solution was 8.00. What are the values of Ka1 and Ka2? 6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
The pH of the solution formed by mixing 50 mL of 0.1 M NaH2PO4 and 10 mL of 0.2 M NaOH You calculate. (Ka1 = 7.5 x 10-3, Ka2 = 6.32 x 10-8, Ka3 = 4.5 x 10-13) a)7.02 b) 5.71 c) 9.69 d) 6.28 e) anything
Consider the titration of 100.0 mL of the weak diprotic acid H2A (0.10 M) with 0.20 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) 1. Before any NaOH is added 2. After 25.0 mL of 0.20 M NaOH is added 3. After 50.0 mL of 0.20 M NaOH is added 4. After 75.0 mL of 0.20 M NaOH is added 5. After 200.0...
Phosphoric acid, H3PO4, is a triprotic acid with the following acid dissociation constants: Ka1 = 7.5 × 10-3 Ka2 = 6.2 × 10-8 Ka3 = 4.2 × 10-13 Which of the following combinations would be best for preparing a pH 7 buffer? a. H3PO4 and NaH2PO4 b. H3PO4 and HCl c. Na2HPO4 and Na3PO4 d. NaH2PO4 and Na2HPO4 e. H3PO4 and Na3PO4
Find the concentration of all species in solution for a 0.10 M solution of H3PO4, a triprotic weak acid. acetic acid: Ka = 1.7 x 10-5 ammonia: Kb = 1.8 x 10-5 carbonic acid: Ka1 = 4.3 x 10-7; Ka2 = 4.8 x 10-11
A titration is carried out for 20.0mL of 0.10 M Oxalic Acid (weak acid) with 0.10 M of a strong base NaOH. Calculate the pH at these volumes of added base solution: (a) 0.0 mL (b) 5.0 mL (c) 10.0 mL (d) 15.0 mL (e) 20.0 mL (f) 25.0 mL (g) 30.0 mL Oxalic acid Ka1 = 5.9 x 10-2 Ka2 = 6.4 x 10-5