Question

In: Chemistry

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.

Solutions

Expert Solution

pKa1 = -log Ka1

pKa1 = 2.15

millimoles of H3PO4 = 50 x 0.1 = 5

millimoles of NaOH = 25.9 x 0.1 = 2.59

H3PO4 + NaOH --------------------> NaH2PO4 + H2O

5                2.59                                   0                   0

2.41             0                                     2.59               0

pH = pKa + log [NaH2PO4 / H3PO4]

pH = 2.15 + log (2.59 / 2.41)

pH = 2.18


Related Solutions

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
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.
Consider the titration of 100.00mL of 1.00 M H3PO4 with 1.00M NaOH. ka1= 7.5x10^-3, ka2= 6.2x10^-8,...
Consider the titration of 100.00mL of 1.00 M H3PO4 with 1.00M NaOH. ka1= 7.5x10^-3, ka2= 6.2x10^-8, ka3= 4.2x10^-13 a. calculate the pH before any base is added. Hint: first write down the major species and pick out the strongest acid. b. calculate the pH after 25.00 mL of base is added C. calculate pH after 50.00mL base is added d. calculate pH after 100.0 mL base is added e. calculate pH after 150.00 mL base is added f. calculate pH...
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 of a solution produced during the titration of 50.00 mL of 2.0 M...
Calculate the pH of a solution produced during the titration of 50.00 mL of 2.0 M acetic acid with 1.0 M potassium hydroxide and the following volumes of base added: a) 0.00 mL b) 25.0 mL c) 50.0 mL d) 100.0 mL e) 125.0 mL
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=
Calculate the pH at 25°C of a 0.65 M aqueous solution of phosphoric acid (H3PO4). (Ka1,...
Calculate the pH at 25°C of a 0.65 M aqueous solution of phosphoric acid (H3PO4). (Ka1, Ka2, and Ka3 for phosphoric acid are 7.5 × 10−3, 6.25 × 10−8, and 4.8 × 10−13, respectively.) Please show how you do the quadratic equation. I am struggling with this in particular. Thank you!
calculate the pH during the titration of 50.00 ml of .400 M HCl with .800 M...
calculate the pH during the titration of 50.00 ml of .400 M HCl with .800 M KOH after 0, 12.50, 25.00, and 40.00 ml of KOH have been added. Graph the titration curve.
Calculate the pH during the titration of 40.00 mL of 0.1000M propanoic acid (HPr; Ka=1.3x10-5) after...
Calculate the pH during the titration of 40.00 mL of 0.1000M propanoic acid (HPr; Ka=1.3x10-5) after adding 22.18 mL of 0.1000M NaOH. ** All volumes should have a minimum of 2 decimal places
Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid , Ka...
Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid , Ka = 4.9 x 10-5, with 0.100 M NaOH at the following points: SHOW ALL WORK IN NEAT DETAIL ON A SEPARATE PAGE. (Be sure to write chemical equations and Ka or Kb expressions when needed.) a. (4 Pts) Before any NaOH is added. b. (4 Pts) After 18.7 mL of NaOH are added. c. (4 Pts) After 25.00 mL of NaOH are added. d....
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT