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
As Ka1 and Ka2 are very very small in comparison to Ka1 ,hence the concentration of hydronium ion comes from first dissociation.
[H+] = (Ka1×C)1/2
= (7.5×0.515×10-3)1/2
=6.2×10-3 M
(a) is correct option
What is the equilibrium pH of a 0.515 M solution of H3PO4 (aq)? (Ka1 = 7.5...
What is the equilibrium concentration of H2PO4– in a 0.202 M solution of H3PO4(aq)? (Ka1 = 7.5 x 10^-3,Ka2 =6.2x10–8,Ka3 =4.8x10–13) please list full step by step on how to solve problem.
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.
Phosphoric acid has a formula of H3PO4, and has a Ka1 of 7.5×10–3 , Ka2 of 6.2×10–8 , and Ka3 of 4.2×10–13 at 25 ºC. What is the equilibrium constant for the following reaction at 25°C? HPO42–(aq) + H2O(l) ⇄ H2PO4–(aq) + OH–(aq) A.) 4.2×10–13 B.) 1.3×10–12 C.) 2.4×10–2 D.) 7.5×10–3 E.) 1.6×10–7
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.)
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
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?
What is the pH of a 6.00 M H3PO4 solution? Ka1= 7.5x10^-3 Ka2= 6.2x10^-8 Ka3= 4.2x10^-13 Pearson retur Learn Ch 17: Acids and Bases QUESTION ANSWER 2.12 Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. K is the equilibrium constant for the dissociation of a weak acid and K is the equilibrium constant for the dissociation of a...
Phosphoric acid has the following dissociation constants: Ka1 = 7.5×10-3; Ka2 = 6.2×10-8; and Ka3 =4.8×10-13, how to prepare a buffer solution of pH 7.40?
Phosphoric acid has three protons that can ionize. The Kas are as follows: Ka1 = 6.9 x 10-3 Ka2 = 6.4 x 10-8 Ka3 = 4.8 x 10-11 Which of these constants would you use to calculate the pH of a 0.1 M solution of H3PO4? A. Ka1, Ka2, and Ka3 B. Ka1, and Ka2 C. Ka1 only D. Ka2, and Ka3 E. Ka1, and Ka3
What is the pH of a solution of 0.750 M KH2PO4, potassium dihydrogen phosphate? thanks!! At 25 C phosphoric acid, H3PO4, has the following equilibrium constants: H30+ (aq) + H2 PO4 (aq) H30+ (aq) + HP042-(aq) Kal 7.5 x 10-3 Ka2=6.2×10-8 Kas4.2 x 10-13 H, PO4 (aq) + H20(1) H,PO4-(aq) + H2O(1) 근 HPO(a)+H2O()HO (a)P (aq) ▼ Part A At 25 C phosphoric acid, H3PO4, has the following equilibrium constants: H30+ (aq) + H2 PO4 (aq) H30+ (aq) + HP042-(aq)...