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
Phosphoric acid, H3PO4, is a triprotic acid with the following acid dissociation constants: Ka1 = 7.5 × 10-3 Ka2 = 6.2...
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?
2) The acid-dissociation constants of phosphoric acid (H3PO4) are Kaj = = 7.5 x 10-3 Ka2 = 6.2 x 10-8, and Kaz = 4.2 x 10-13 at 25.0°C. What is the pH of a 2.00 M aqueous solution of phosphoric acid?
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
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?
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To find the pH of a buffer composed of H,PO, (aq) and HPO2 (aq), which pKa value should be used in the Henderson-Hasselbalch equation? O pK al = 2.16 OpKq2 = 7.21 O pK a3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 19.0 g of KH,PO4(s) and 30.0 g of Na, HPO4(s) in...
Phosphoric acid is a triprotic acid with the p?a values p?a1=2.148, p?a2=7.198, and p?a3=12.375. You wish to prepare 1.000 L of a 0.0300 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= g mass Na2HPO4= g What other combination...
25) The acid-dissociation constants of phosphoric acid (H2PO4) are KZ1 = 7.5 x 10-3, K22= 6.2 x 10-8, and K 3 = 4.2 x 10-13 at 25.0°C. What is the pH of a 2.00 M aqueous solution of phosphoric acid? 26) Zº is a weak base. An 0.350 M aqueous solution of NaZ is prepared. The pH of the solution was 8.93 at 25.0°C. The Ky of Zº is:
Phosphoric acid is a triprotic acid (Kal 6.9x10-3, Ka2 6.2x 10-8, and Ka3 4.8x 10-3). To find the pH of a buffer composed of H2PO4 (aq) and HPO4 (aq), which pKa value would you use in the Henderson-Hasselbalch equation? O pkat 2.16 O pKa2 7.21 рказ 12.32 Calculate the pH of a buffer solution obtained by dissolving 15.0 g of KH2PO4(s) and 25.0 g of Na2HPO4(S) in water and then diluting to 1.00 L Number pHL
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
You are instructed to create 400. mL of a 0.40 M phosphate buffer with a pH of 6.4. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. (Enter all numerical answers to three significant figures.) H3PO4(s) + H2O(l) H3O+(aq) + H2PO4−(aq) Ka1 = 6.9 ✕ 10−3 H2PO4−(aq) + H2O(l) H3O+(aq) + HPO42−(aq) Ka2 = 6.2 ✕ 10−8 HPO42−(aq) + H2O(l) H3O+(aq) + PO43−(aq) Ka3 = 4.8 ✕ 10−13 Which of the available chemicals will you use...