2. Determine the predominating species at pH-8.00.A. H3C6H5O7C. HC₂H5O7²-D. C₂H5O7³-B. H₂C6H5O7Answer:3. What is the fraction of H₂C6H5O7 at pH=4.00? Round-off your answer into four significant figures. Do notexpress your answer in scientific notation. Write 0 before the decimal point if the value is less than 1 (eg. 0.125).Answer:4. What is the molar concentration of H₂C6H5O7 at pH=4.00? Round-off your answer into four significantfigures. Do not include units nor express your answer in scientific notation. Write 0 before the decimal point if thevalue is less than 1 (eg. 0.125).Answer:4 Consider a 0.10 M citric acid with Ka values given:H3C6H5O7 (aq) + H₂O(1)H₂C6H5O7 (aq) +H3O* (aq)H₂C6H5O7 (aq) + H₂O(1)HC6H5072 (aq) +H3O+ (aq)HC6H507² (aq) + H₂OC6H507³ (aq) + H30* (aq)1. Determine the predominating species at pH=5.00.A. H3C6H5O7C. HC6H5O7²-B. H₂C6H5O7D. C₂H5O7³-Answer:2. Determine the predominating species at pH=8.00.A. H3C6H5O7CIHC₂H5O7²-D. C6H5O7³-B. H₂C6H5O7Answer:Ka = 7.5 x 10-4Ka = 1.7 x 10-5Ka = 4.0 x 10-7

Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts…

Consider a 0.10 M citric acid with Ka values given: H3C6H5O7 (aq) + H₂O(1) H₂C6H5O7 (aq) + H₂O(1) HC6H507² (aq) + H₂O (1) H₂C6H5O7 (aq) + H30* (aq) H30* (aq) HC6H5072 (a (aq) + C6H507³(aq) + H30* (aq) 1. Determine the predominating species at pH=5.00. A. H3C6H5O7 C. HC6H5O7²- B. H₂C6H5O7 D. C6H507³- Answer: Ka = 7.5 x 10-4 Ka = 1.7 x 10-5 Ka = 4.0 x 10-7

Consider a 0.10 M citric acid with Ka values given: H3C6H5O7 (aq) + H₂O(1) H₂C6H5O7 (aq) + H₂O(1) HC6H507² (aq) + H₂O (1) H₂C6H5O7 (aq) + H30* (aq) H30* (aq) HC6H5072 (a (aq) + C6H507³(aq) + H30* (aq) 1. Determine the predominating species at pH=5.00. A. H3C6H5O7 C. HC6H5O7²- B. H₂C6H5O7 D. C6H507³- Answer: Ka = 7.5 x 10-4 Ka = 1.7 x 10-5 Ka = 4.0 x 10-7

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

Hydrogen phosphate ion is an anion with the chemical formula H2PO4–. In the aqueous state, it undergoes the following reactions: (i) H2PO4– (aq) + H2O (ℓ) ⇌ H3O+ (aq) + HPO42– (aq) (ii) H2PO4– (aq) + H3O+ (aq) ⇌ H3PO4 (aq) + H2O (ℓ) Which of the following statements is true about the above reactions? Question 2 options: In reaction (i) hydrogen phosphate acts as a Brønsted-Lowry base and in reaction (ii) it acts as a Brønsted-Lowry acid. In reaction (i) and (ii) hydrogen phosphate acts as a Brønsted-Lowry base. In reaction (i) hydrogen phosphate acts as a Brønsted-Lowry acid and in reaction (ii) it acts as a Brønsted-Lowry base. In reaction (i) and (ii) hydrogen phosphate acts as a Brønsted-Lowry acid.
Please answer all (3)
Identify the correct net lonic equation for the reaction that occurs when solutions of HF and KOH are mlxed. 16 Multiple Cholce 01:27.29 O H(aq) - OH(aq) → H20() HF(aq)- KOH(s) → H20(1) - KF(aq) HF(aq)- OH (aq) H20(1) - F(aq) O HF(aq) - KOH(aq) H20(1) - KF(S) HTac)- KOH(ag)- H-O) - K(ac)
1)Write the balanced chemical reaction for the neutralization of the monoprotic acid: - HCl -acetic acid (CH3COOH) 2)Write the chemical reaction for the neutralization of the triprotic acid citric acid (C6H8O7) 3)write the balanced chemical reaction for the neutralization of the diprotic acid H2SO4
The Ka of the conjugate acid of a pesticide is 6.7 x 10-6. What is the Kb of the pesticide at 25°C? 1.5 x 1019 1.5 x 10-9 6.7 x 10-8 6.7 x 10-20
What is the H+ concentration for an aqueous solution with pOH = 2.70 at 25 ° C? %3D Express your answer to two significant figures and include the appropriate units. View Available Hint(s) HẢ ? [H+] = Value Units %3D Cubmi4
Q33
Payal
If the hydrogen ion concentration of a 0.100 M HC3H5O3 solution is 0.0038 M, what is the ionization constant for lactic acid?
(Q15) What type of solution is expected to result when the ionic salt potassium nitrite (KNO2) is added to solution (nitrous acid is a weak acid)? Supercritical Neutral Cannot be determined Basic O Acidic
What is the concentration of citric acid H3C6H5O7 in a 0.400 M solution of citric acid? please explain in detail
2- Given HCO3(aq) + HSO3 (aq) = H₂CO3(aq) + S03² (aq) The Bronsted - Lowry acids in the above equation are O O O O . HCO3(aq) and HSO3(aq) HSO3(aq) HSO3(aq) 2- and S03² (aq) and H₂CO3(aq) HCO3(aq) and H₂CO3(aq)