## Vitamin C Dissociation and Equilibrium Concentrations### Problem Statement3. A typical vitamin C tablet contains pure ascorbic acid \( \text{H}_2\text{C}_6\text{H}_6\text{O}_6 \) (a weak, diprotic acid). If 2 tablets are dissolved in about a cup of water, the resulting concentration of the ascorbic acid is 0.0115 M.---### a. First Ionization Equation**Task:** Write the equation for the dissociation for the first ionization (loss of the first acidic hydrogen, H). This ionization has a \( K_a \) of \( 8.00 \times 10^{-5} \).\[ \text{H}_2\text{C}_6\text{H}_6\text{O}_6 (aq) \rightleftharpoons \text{H}^+ (aq) + \text{HC}_6\text{H}_6\text{O}_6^- (aq) \]---### b. Equilibrium Concentration Calculation**Task:** Determine the equilibrium concentration for all species from the first ionization.To solve this, consider that initially:- [H₂C₆H₆O₆] = 0.0115 M- [H⁺] = 0 M- [HC₆H₆O₆⁻] = 0 MUse the ionization constant \( K_a \) to calculate the changes in concentration at equilibrium. The solution involves setting up an ICE table (Initial, Change, Equilibrium) and using the value of \( K_a \) to solve for the concentrations algebraically.---No graphs or diagrams are present in the image. **c.** Give the equation for the dissociation for the second ionization (loss of the second acidic H from the CB of step a).**d.** What is the equilibrium concentration for all species in the second ionization if the Ka for the second H is 1.6 x 10^-12?**e.** Combining your answers from b and d, what is the total H3O^+ concentration, pH, pOH, and % ionization?

a.) To write the dissociation equation , we just ionise the given compound into its ions . b.) To…

3. A typical vitamin C tablet contains pure ascorbic acid H2C6H6O6 (a weak, diprotic acid). If 2 tablets are dissolved in about a cup of water, the resulting concentration of the ascorbic acid is 0.0115 M. a. Give the equation for the dissociation for the first ionization (loss of the first acidic H). This ionization has a Ka of 8.00 x 10-5. b. What is the equilibrium concentration for all species from the first ionization?

3. A typical vitamin C tablet contains pure ascorbic acid H2C6H6O6 (a weak, diprotic acid). If 2 tablets are dissolved in about a cup of water, the resulting concentration of the ascorbic acid is 0.0115 M. a. Give the equation for the dissociation for the first ionization (loss of the first acidic H). This ionization has a Ka of 8.00 x 10-5. b. What is the equilibrium concentration for all species from the first ionization?

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...

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