Question

In: Chemistry

Phosphoric acid is a triprotic acid (Ka1=6.9×10−3Ka1=6.9×10−3, Ka2=6.2×10−8Ka2=6.2×10−8, and Ka3=4.8×10−13Ka3=4.8×10−13). To find the pH of a...

Phosphoric acid is a triprotic acid (Ka1=6.9×10−3Ka1=6.9×10−3, Ka2=6.2×10−8Ka2=6.2×10−8, and Ka3=4.8×10−13Ka3=4.8×10−13).

To find the pH of a buffer composed of H2PO−4(aq)H2PO4−(aq) and HPO2−4(aq)HPO42−(aq), which pKaKa value should be used in theHenderson–Hasselbalch equation?

pKa1Ka1 = 2.16

pKa2Ka2 = 7.21

pKa3Ka3 = 12.32

Calculate the pH of a buffer solution obtained by dissolving 18.018.0 g of KH2PO4(s)KH2PO4(s) and 30.030.0 g of Na2HPO4(s)Na2HPO4(s) in water and then diluting to 1.00 L.

pH=

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago
Next > < Previous

Related Solutions

Phosphoric acid is a triprotic acid (Ka1 = 6.9× 10–3, Ka2 = 6.2× 10–8, and Ka3...
Phosphoric acid is a triprotic acid (Ka1 = 6.9× 10–3, Ka2 = 6.2× 10–8, and Ka3 = 4.8× 10–13). To find the pH of a buffer composed of H2PO4–(aq) and HPO42–(aq), which pKa value would you use in the Henderson-Hasselbalch equation? Calculate the pH of a buffer solution obtained by dissolving 15.0 g of KH2PO4(s) and 33.0 g of Na2HPO4(s) in water and then diluting to 1.00 L.
Given: Ka1= 7.5*10^-3 Ka2=6.2*10^-8 Ka3=4.2*10^-13 What is the pH of a solution of 0.550 M K2HPO4,...
Given: Ka1= 7.5*10^-3 Ka2=6.2*10^-8 Ka3=4.2*10^-13 What is the pH of a solution of 0.550 M K2HPO4, potassium hydrogen phosphate? What is the pH of a solution of 0.400 M KH2PO4, potassium dihydrogen phosphate?
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13)...
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after adding 25.9 mL of 0.1000M NaOH. ** All volumes should have a minimum of 2 decimal places.
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13)...
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after adding 28.2 mL of 0.1000M NaOH. All volumes should have 2 decimal places
The triprotic acid H3A has ionization constants of Ka1 = 6.2× 10–3, Ka2 = 9.6× 10–9,...
The triprotic acid H3A has ionization constants of Ka1 = 6.2× 10–3, Ka2 = 9.6× 10–9, and Ka3 = 6.3× 10–12. Calculate the following values for a 0.0790 M solution of NaH2A A)Calculate the following values for a 0.0790 M solution of NaH2A. H+=? H2A-/H3A=? B)Calculate the following values for a 0.0790 M solution of Na2HA. H+=? HA2-/H2A-=?
Arsenic acid (H3AsO4) is triprotic, with Ka1=5.5 x 10-3 (10 to the negative 3), Ka2=1.7 x...
Arsenic acid (H3AsO4) is triprotic, with Ka1=5.5 x 10-3 (10 to the negative 3), Ka2=1.7 x 10-7(10 to the negative 7), and Ka3=5.1 x 10-12 (10 to the negative 12). What is the pH of a 0.80 M solution of arsenic acid.,
The triprotic acid H3A has ionization constants of Ka1 = 1.6× 10–3, Ka2 = 2.4× 10–9,...
The triprotic acid H3A has ionization constants of Ka1 = 1.6× 10–3, Ka2 = 2.4× 10–9, and Ka3 = 6.4× 10–11. Calculate the following values for a 0.0800 M solution of NaH2A. [H+] = M [H2A-]/[H3A] =    Calculate the following values for a 0.0800M solution of Na2HA. [H+] = M [HA2-]/[H2A-] = This is all the information this problem comes with Hint: Consider H2A– to be the intermediate form of a diprotic acid, surrounded by H3A and HA2–. Consider...
Citric acid is a tri-protic acid with Ka1= 8.4x10^-4, Ka2= 1.8x 10^-5 Ka3= 4.0x 10^-6 a)...
Citric acid is a tri-protic acid with Ka1= 8.4x10^-4, Ka2= 1.8x 10^-5 Ka3= 4.0x 10^-6 a) calculate the pH at the 2dn equlivance point in the titration of 100.0 ml of 0.21M citric acid solution with 0.25M NaOH. Calculate the pH after 15.8 ml of NaOH has been added. c) calculate the pH 5.0 ml after the last equivalence point
Phosphoric acid is a triprotic acid, and the Ka values are given below. Calculate pH, pOH,...
Phosphoric acid is a triprotic acid, and the Ka values are given below. Calculate pH, pOH, [H3PO4], [H2PO4 2- ], [HPO4 - ], and [PO4 3- ] at equilibrium for a 5.00 M phosphoric acid solution. Ka1 = 7.5 x 10-3 Ka2 = 6.2 x 10-8 Ka3 = 4.2 x 10
Phosphoric acid, H3PO4(aq), is a triprotic acid. Calculate the pH and concentrations of H3O + (aq),...
Phosphoric acid, H3PO4(aq), is a triprotic acid. Calculate the pH and concentrations of H3O + (aq), H3PO4(aq), H2PO4 − (aq), HPO4 2− (aq), PO4 3− (aq), and OH− (aq) in a 0.100-M phosphoric acid solution at 25°C.
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT