29. pKa3Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning thatone molecule of the acid has three acidic protons. Estimate4pKalpKa22.167.2112.32the pH and the concentrations of all species in a 0.500 Mphosphoric acid solution.[H,PO,] =M[H*] =M[H,PO,] =M[OH-] =M[HPO; ] =MpH[PO] =M

Answered: Image /qna-images/answer/7a5fb8c9-3589-4202-9a7c-ac221ed54e86.jpg

Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning that pKal pKa2 pKa3 one molecule of the acid has three acidic protons. Estimate 2.16 7.21 12.32 the pH and the concentrations of all species in a 0.500 M phosphoric acid solution. [H,PO,] = M [H*] = M [H,PO,] = M [OH-] = M [HPO] = M pH = [PO] = M

Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning that pKal pKa2 pKa3 one molecule of the acid has three acidic protons. Estimate 2.16 7.21 12.32 the pH and the concentrations of all species in a 0.500 M phosphoric acid solution. [H,PO,] = M [H*] = M [H,PO,] = M [OH-] = M [HPO] = M pH = [PO] = M

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 118QRT

See similar textbooks

Similar questions

Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
Leucine is an amino acid with this Lewis structure: Write the Lewis structure for the zwitterion form of leucine.
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Please don't provide handwritten solution... In the laboratory, a general chemistry student measured the pH of a 0.513 M aqueous solution of triethanolamine, C6H15O3N to be 10.721. Use the information she obtained to determine the Kb for this base.
calculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in a 71.0mL of 0.10M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75x10^-5.
Look up the appropriate Ka1 and Ka2 values for oxalic acid andascorbic acid, and repeat these calculations for these two weak, diprotic acids. Calculate the pH of both solutions and rank the acidities of the carbonic acid, oxalic acid, and ascorbic acidsolutions. In what ways is the ranking consistent with the magnitudes of the ionization constants?
3. The pH of a solution is 6.7. From this statement alone, can you conclude that the solution is acidic? If not, what additional information would you need? Can the pH of a solution be zero or negative? If so, give examples to illustrate these values. 5. At 25°C, calculate the molar H3O+ and OH-1 concentrations of the following:a. 0.0300 M C6H5COOHb. 0.0600 M NH3c. 0.200 M C6H5COONa (sodium benzoate)d. 0.0860 M KOHe. 0.0689 M HCl
A certain diprotic acid has a Ka1= 5.87e-4 and a Ka2= 5.55e-9. Calculate the pH of 737mL of a 0.259 molar solution of the acid to which has been added to 737mL of 0.259 molar aolution of potassium hydroxide.
Calculate the pH of a solution prepared by dissolving 1.75 g of sodium acetate, CH3COON,, in 53.5 mL of 0.15 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5.