Calculate the pH and concentration of species present in a polyprotic acid solution.For a \(3.65 \times 10^{-2}\) M solution of \( \text{H}_2\text{C}_6\text{H}_6\text{O}_6 \), calculate both the pH and the \( \text{C}_6\text{H}_6\text{O}_6^{2-} \) ion concentration.\[ \text{H}_2\text{C}_6\text{H}_6\text{O}_6 + \text{H}_2\text{O} \rightleftharpoons \text{H}_3\text{O}^+ + \text{HC}_6\text{H}_6\text{O}_6^- \quad K_{a1} = 7.9 \times 10^{-5} \]\[ \text{HC}_6\text{H}_6\text{O}_6^- + \text{H}_2\text{O} \rightleftharpoons \text{H}_3\text{O}^+ + \text{C}_6\text{H}_6\text{O}_6^{2-} \quad K_{a2} = 1.6 \times 10^{-12} \]**Calculate:**\[ \text{pH} = \]\[ [\text{C}_6\text{H}_6\text{O}_6^{2-}] = \quad \text{M} \]

Answered: Image /qna-images/answer/ac7330b7-f131-4bfd-87db-2e8eb5442264.jpg

Calculate the pH and concentration of species present in a polyprotic acid solution. For a 3.65x10-2 M solution of H₂C6H606, calculate both the pH and the C6H6062- ion concentration. H₂C6H606+ H₂O HC₂H₂O6 + H₂0 H3O+ + HC6H606 Ka1 = 7.9x10-5 H30++ C6H6062- Ka2 = 1.6x10-12 pH = [C6H606²-] = M

Calculate the pH and concentration of species present in a polyprotic acid solution. For a 3.65x10-2 M solution of H₂C6H606, calculate both the pH and the C6H6062- ion concentration. H₂C6H606+ H₂O HC₂H₂O6 + H₂0 H3O+ + HC6H606 Ka1 = 7.9x10-5 H30++ C6H6062- Ka2 = 1.6x10-12 pH = [C6H606²-] = M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the pH of a 0.370 M aqueous solution of methylammonium chloride, CH3NH3Cl? The Kb of methyl amine, CH3NH2 is 4.4x10-4. You do not need to solve the quadratic equation for this problem. Express your answer to two decimal places.
Find the H3O+H3O+ concentration of a 0.220 MM hypochlorous acid solution (whose acid dissociation constant is Ka=2.9×10−8Ka=2.9×10−8). Express the concentration to two significant figures.
The pH of a 0.86M solution of hydrocyanic acid (HCN) is measured to be 4.64. Calculate the acid dissociation constant K of hydrocyanic acid. Round your answer to 2 significant digits. a K = a Ix10 X Ś
H3PO4 is a weak polyprotic acid with K₁ = 7.2x10³, K₂= 6.3x10^-8, and K3 = 4.2x10^-13. What is the pH of a 0.275 M solution of KH₂PO4? Simplifying assumptions may be made. Give answer to 2 decimal places.
The Kb of pyridine, C5H5N, is 1.7 x 10−9. Calculate the pH of a 0.124 M solution of pyridinium bromide, C5H5NH+Br−.
For the diprotic weak acid H2A, Kal =3.4 •10^-6 and Ka2=8.5 •10^-9. what is the pH of a 0.0700M solution of H2A? pH=What are the equilibrium concentrations of H2A and A2- in this solution? [H2A]=M [A2-]=M
H2C2O4 is a diprotic acid that dissociates as shown below.Ka1 = 5.38 x 10-2 and Ka2 = 5.18 x 10-5. Determine the pH of 0.1 M Sodium hydrogen oxalate (NaHC2O4). (Note: neglect hydroxide formation due to hydrogen oxalate hydrolysis)
What is the pH of an aqueous solution with [H3O+] = 2×10−14 M? Express the pH numerically using one decimal place.
Consider the following data on some weak acids and weak bases: base acid K₁ name formula name formula nitrous acid HNO₂ 4.5 × 10 4 hypochlorous acid HC1O 3.0 × 108 ammonia aniline C6H5NH24.3 × 10-10 NH, 1.8 × 10-5 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution PH 0.1 M KCIO choose one 0.1 M NH4Cl choose one 0.1 M KBr choose one 0.1 M C6H5NH3Br choose one G
For the diprotic weak acid H2A, ?a1 = 2.3×10−6 and ?a2 = 6.8×10−9. What is the pH of a 0.0500 M solution of H2A? pH= What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]= M [A2−]= M
The pH of a 0.84 M solution of barbituric acid (HC₂H₂N₂O3) is measured to be 2.04. Calculate the acid dissociation constant K of barbituric acid. Be sure your answer has the correct number of significant digits. K = 0 a x10 × Ś
The acid dissociation constant K, of hypobromous acid (HB1O) is 2.3 x 10. Calculate the pH of a 1.8 M solution of hypobromous acid. Round your answer to 1 decimal place. pH = 0