What is the H3O+ concentration of a 0.100 M of a wveak organic acid ( HA) with Ka = 3.5 x 10-8 ?HA(aq) + H20(1) = H3O*(ag) + A (ag).2.8 x 10-54.4 × 10-55.9 x 10-51.9 × 10-4

Answered: Image /qna-images/answer/d3b8b978-4a0d-4ea5-abac-fcf88d56e6d8.jpg

Vhat is the H3O* concentration of a 0.100 M of a weak organic acid ( HA ) with Ką = 3.5 x 10-8 ? HA(aq) + H2O(1) = H3O*(aq) + A*(aq). 2.8 x 10-5 4.4 × 10-5 5.9 x 10-5 O 1.9 × 10-4

Vhat is the H3O* concentration of a 0.100 M of a weak organic acid ( HA ) with Ką = 3.5 x 10-8 ? HA(aq) + H2O(1) = H3O(aq) + A(aq). 2.8 x 10-5 4.4 × 10-5 5.9 x 10-5 O 1.9 × 10-4

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

Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the dry texture of certain wines. Tartaric acid, H2C4H4O6, is a diprotic acid with the following Ką values: Ka1 = 1.00 x 10-3; Ka2 = 4.60 x 10-5 a. Write the equation for the 1st jonization of tartaric acid. b. Write the equation for the 2nd ionization of tartaric acid. c. Write the Ką expression for the 1st ionization. d. Write the Ką expression for the 2nd ionization. e. What is the equilibrium concentrations of the reactants and products from the 1st ionization of a 0.250M solution of tartaric acid? f. What is the equilibrium concentrations of the reactants and products from the 2nd ionization? g. What is the total [H30+] and the overall pH of the solution of tartaric acid?
Case 3: pH with known K: The dissociation of ammonia (NH3) in water is shown below: NH3 (aq) + H2O (m = NH4*(aq) + OH-(aq) At 25°C, Kb, is 1.8 × 10-5 (7) Calculate the pH of a mixture of 0.192 mol NH3 and 0.116 mol NH4C1 diluted to 400.0 mL with distilled water.
Complete the abundance diagram by identifying the species present in an aqueous solution of 1.00 M acetic acid (CH, COOH). The K』 of acetic acid is 1.8 × 10-5. Percent Abundance 50%- EX 7 pH What is the approximate pH of a solution of 1.00 M CH3COOH? Answer Bank CH3COO~ CH3COOH OH- H3O⁺ 14
What is the pH for the following aqueous solutions? a. 0250 M Ammonia (Kb = 1.8 X 10-5) b. 0385 M Hydrochloric Acid
I'm confused on how to do number 4 a and b
Calculate the concentration of each species present in a 0.025 M solution of phthalic acid, C6H4(CO2H)2. C6HĄ(CO2H),(aq) + H,O(1) = H;0*(aq) +C6H4(CO2H)(CO2)¯(aq) Ką=1.1×10-3 CoH4(CO,H)(CO2)-(aq)+ HzO(1)= H30*(aq) + CgHq(CO2),²-(aq) Ką=3.9x 10-6
Calculate the concentration for the following pH: pH = 7.00 (A) (H:0*] = 1 x 10-9 M (B) (H30*] = 1 x 10-7 M (C) (H304] = 2x 107 M (D) (H30*] = 1 x 10-3 M 34Help Asha balance the following equation by completing the equation with the correct numbers: _P4+_F2› PF3 35.Asha balance the following equation by completing the equation with the correct numbers: _H2 + _F2>HF can you help me with these last 3... please . I don't understand it
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
Pls help ASAP
Is a Brønsted-Lowry acd, highlighted reactant reaction Bronsted-Lowry Bronsted-Lowry acid base neither HCIO,(aq) + OH (aq) Clo, (a0) + H,O() 1 CIO,(30) + H,O) → HC1O3(aq) + OH (aq) ClO3 (30) + H,OM- HCIO3(aq) + OH (aq) HCIO,(aq) + OH (aq) Clo, (aq) + H,O()
Please don't provide handwriting solution
When you cool down water to 10°C, Kw = 2.9 x 10-15, as compared to the value of Kw at 25°C which is 1 x 10-14 (a bigger K at a higher temp). Which statement is true? a) Dissociation of H₂O is endothermic; the pH of neutral water at 10°C is 14.5 b) Dissociation of H₂O is exothermic; the pH of neutral water at 10°C is 14.5 c) Dissociation of H₂O is endothermic; the pH of neutral water at 10°C is 7.27 d) Dissociation of H₂O is exothermic; the pH of neutral water at 10°C is 7.27 e) Dissociation of H₂O is endothermic; the pH of neutral water at 10°C is 7 f) Dissociation of H₂O is exothermic; the pH of neutral water at 10°C is 7