Phosphoric acid (H₃PO₄) is a triprotic acid with pKa values of 2.12, 7.21, and 12.32. It is a useful buffer solution for pH values near the pKa values. You have a 0.100 M solution of phosphate buffer with a pH of 2.50. How many mL of 0.500 M NaOH solution must be added to 1.00 L of this buffer solution to convert it to a buffer at pH 7.70?

Phosphoric acid (H₃PO₄) is a triprotic acid with pKa values of 2.12, 7.21, and 12.32. It is a useful buffer solution for pH values near the pKa values. You have a 0.100 M solution of phosphate buffer with a pH of 2.50. How many mL of 0.500 M NaOH solution must be added to 1.00 L of this buffer solution to convert it to a buffer at pH 7.70?

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 106GQ: The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106....

See similar textbooks

Similar questions

What is the pH of water at 25°C that contains 0.60 mg/L of hypochlorous acid (pKa = 7.54)? Assume equilibrium has been achieved and there are equal concentrations of dissociated ions. Neglect the dissociation of water.
Phosphoric acid (H₃PO₄) is a triprotic acid with pKa values of 2.12, 7.21, and 12.32. It is a useful buffer solution for pH values near the pKa values. You have a 0.100 M solution of phosphate buffer with a pH of 2.50. How many mL of 0.500 M NaOH solution must be added to 1.00 L of this buffer solution to convert it to a buffer at pH 7.70? Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH of a 0.62 M solution of carbonic acid? A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.20 M solution of H₂A? What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in 2.0 L of solution?
What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid concentration equivalent to that of its conjugate base?
Determine the pH of a 10-3 mol/L solution of (a) hydrogen sulfate ion (pKa = 1.99), (b) formic acid (pKa = 3.75), (c) hypochlorous acid (pKa = 7.53), (d) phenol (pKa = 9.98)
Calculate the pH of a 0.20 M HA solution, given the pKa of HA is 2.22.
Which is more acidic? Is the most dangerous acid the strongest acid? Include a comparison of pH and pKa 0.05 M HBr solution (Ka = 1 x 109) 0.75 M H2C2O4 solution (Ka = 5.9 x 10-2)
What is the pH of a 0.15 M solution of sodium nitrite? The pKa of nitrous acid is 3.15.
Baking powder contains sodium bicarbonate plus an acidic salt like sodium acid tartrate or calcium acid phosphate. Suggest how baking powder can "raise" breads and pastries when mixed with water and heated.
pka = 1.95 (HClO2) If you have 500 mL of a 0.10 M solution of the acid, what mass of the corresponding sodium salt of the conjugate base do you need to make the buffer with a pH of 1.81 (assuming no change in volume)?
The following solutions were prepared: Solution A: 0.01 mole of perchloric acid (HClO4) dissolved in 1 L of water. Solution B: 0.01 mole of ethylamine hydrochloride (CH3CH2NH3Cl, pKa =10.64) dissolved in 1 L of water. a. Calculate the pH of Solution A.b. Calculate the pH of Solution B.c. Why is the pH of Solutions A different from Solution B?
What is the pH of a 0.173 M solution of a hydrogen sulfide? The pKa at the temperature of the experiment is equal to 7.03.
Explain the steps to determining the presence of Pb2+ ions.