▼Part ACalculate the concentration of all species in a 0.145 M solution of H₂CO3.H₂CO3(aq) +H₂O(1) H3O+ (aq) + HCO3(aq) Ka1 = 4.3x10-7HCO3(aq) +H₂O(1) H3O+ (aq) +CO3²- (aq) Ka2 = 5.6x10-11Enter your answers numerically separated by commas. Express your answer using two significant figures.15. ΑΣΦ[H₂CO3], [HCO3 ], [CO32], [H3O+], [OH-] =SWO ?mol L-1

Answered: Image /qna-images/answer/30d78b27-7b9a-458e-a18a-73dfe36d8e7c.jpg

▼ Part A Calculate the concentration of all species in a 0.145 M solution of H₂CO3. H₂CO3(aq) +H₂O(1) H3O+ (aq) + HCO3(aq) Ka1 = 4.3x10-7 HCO3(aq) +H₂O(H₂O* (aq) +CO3² (aq) Ka2 = 5.6x10-11 Enter your answers numerically separated by commas. Express your answer using two significant figures. 15. ΑΣΦ [H₂CO3], [HCO3 ], [CO32], [H3O+], [OH-] = SWO ? mol L-1

▼ Part A Calculate the concentration of all species in a 0.145 M solution of H₂CO3. H₂CO3(aq) +H₂O(1) H3O+ (aq) + HCO3(aq) Ka1 = 4.3x10-7 HCO3(aq) +H₂O(H₂O* (aq) +CO3² (aq) Ka2 = 5.6x10-11 Enter your answers numerically separated by commas. Express your answer using two significant figures. 15. ΑΣΦ [H₂CO3], [HCO3 ], [CO32], [H3O+], [OH-] = SWO ? mol L-1

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.49EP: Is the monoprotic acid Y or the monoprotic acid Z the stronger acid in each of the following...

See similar textbooks

Similar questions

The dissociation of 0.15 M phosphoric acid is given by: H3PO4(aq) + H2O(l) ⇄ H2PO4^-(aq) + H3O^+(aq) Ka = 7.1 x 10-3 (at 25°C) H2PO4^-(aq) + H2O(l) ⇄ HPO4^2-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) HPO4^2-(aq) + H2O(l) ⇄ PO4^3-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) B. Applying the systematic method in solving acid-base equilibria problems, calculate the pH of the following: a. 0.050 M H3PO4 b. 0.050 M NaH2PO4 c. 0.050 M Na2HPO4 d. 0.050 M Na3PO4
What is the concentration of each species present in a 0.010-M solution of phthalic acid, C6H4(CO2H)2? C6H4(CO2H)2(aq) + H2O(l) ⇌ H3O+(aq) + C6H4(CO2H)(CO2)-(aq) Ka1 = 1.1 x 10-3 C6H4(CO2H)(CO2)(aq) + H2O(l) ⇌ H3O+(aq) + C6H4(CO2)22-(aq) Ka2 = 3.9 x 10-6
In the following equation HNO2 (aq) + H2O (l) ↔ H3O+ (aq) + NO2-(aq), 0.37 M of nitrous acid was found in the resulting aqueous solution. Ka for HNO2 is 4.5 x10 -4. What will be the percent ionization of the weak acid? 0.034% 0.038% 0.045% 0.048%
The dissociation of 0.15 M phosphoric acid is given by:H3PO4(aq) + H2O(l) ⇄ H2PO4-(aq) + H3O+(aq)Ka = 7.1 x 10-3 (at 25oC) H2PO4-(aq) + H2O(l) ⇄ HPO42-(aq) + H3O+(aq)Ka = 6.3 x 10-8 (at 25oC) HPO42-(aq) + H2O(l) ⇄ PO43-(aq) + H3O+(aq)Ka = 4.5 x 10-13 (at 25oC)Use the systematic method (Mass-Balance Equations, Charge-Balance Equations, or Proton-Balance Equations) to calculate the pH of the following:a. 0.050 M NaH2PO4b. 0.050 M Na2HPO4c. 0.050 M Na3PO4
Malic acid is a weak diprotic organic acid with Ka1 = 4.0 × 10-4 and Ka2 = 9.0 × 10-5.a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2 . Write the chemical equation that represents Ka1 × Ka2. b Qualitatively describe the relative concentrations of H2A, HA-, A2-, and H3 O+ in a solution that is about one molar in malic acid.c Calculate the pH of a 0.0175 M malic acid solution and the equilibriumconcentration of [H2 A].d What is the A2- concentrationin in solutions b and c?
Which of the following is a representation of the ion product of water? H2O(ℓ)+H2O(ℓ)⇌H3O+(aq)+OH−(aq)H2O(ℓ)+H2O(ℓ)⇌H3O+(aq)+OH-(aq) Kw=[H+][OH−][H2O]Kw=[H+][OH-][H2O] Kw=[H+][OH−][H2O]2Kw=[H+][OH-][H2O]2 Kw=[H2O]2Kw=[H2O]2 Kw=[H+][OH−]Kw=[H+][OH-] Kw=[H+][H2O]
Hydroxylamine, HONH2, readily forms salts such as hydroxylamine hydrochloride which are used as antioxidants in soaps. Hydroxylamine has Kb of 9.1 × 10–9. What is the pH of a 0.054 M HONH2 solution? Please report 2 decimal places.
Which of the following is true on the self-ionization properties of water at 25℃? a. In pure H2O, the [H3O+] = [OH-] = 1.00 × 10-7 M. b. In pure H2O, Keq2[H2O] = Kw = 1.00 x 10-14. c. In pure H2O, the solution is basic if [OH-] < 1.00 × 10-7 M and [H3O+] > 1.00 × 10-7 M. d. In pure H2O, its concentration remains constant at approximately 50 M.
Hydrogen fluoride (HF) behaves as a weak acid in aqueous solution. Two equilibria influencewhich fluorine-containing species are present in solution.HF (aq) + H2O (l) ⇌ H3O+ (aq) + F- (aq) Ka = 6.8 x 10-4F- (aq) + HF (aq) ⇌ HF2- Kc = 2.6 x 10-1A. Is fluoride in pH 7.00 drinking water more likely to be present as F− or HF2−?B. What is the equilibrium constant for the following equilibrium?2 HF(aq) + H2O(?) ⇌ H3O+(aq) + HF2−(aq)C. What are the pH and equilibrium concentration of HF2− in a 0.150 M solution of HF?
For a 0.0359 M aqueous solution of cyanic acid, HCNO (Ka = 3.5*10-4), determine the following. What are the major and minor species present? Include phase. What is the major species (other than water)? What is the concentration of the minor species in the solution? What is the concentration of the major species in the solution? What is the concentration of H3O+ in the solution? What is the concentration of OH- in the solution? Find the pH.
The pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium reactions: CO2(aq)+H2O(l)H2CO3(aq)H2CO3(aq)+H+(aq) Acids formed during normal cellular respiration react with the HCO3 to form carbonic acid, which is in equilibrium with CO2(aq) and H2O(l). During vigorous exercise, a persons H2CO3 blood levels were 26.3 mM whereas his CO2 levels were 1.63 mM. On resting, the H2CO3 levels declined to 24.9 mM. What was the CO2 blood level at rest?
Is the monoprotic acid Y or the monoprotic acid Z the stronger acid in each of the following situations? a. At equal concentrations, Y dissociates to a greater extent than Z in water. b. Ka for Z is larger than Ka for Y. c. The equilibrium position for the dissociation of Y lies farther to the right than that for Z. d. Proton transfer to water occurs to a lesser extent for Z than for Y.