Ascorbic acid, H2C6H6O6, is a diprotic acid usually known as vitamin C. For this acid, pKa1 is 4.10 and pKa2 is 11.79. When 125 mL of a solution of ascorbic acid was evaporated to dryness, the residue of pure ascorbic acid had a mass of 4.14 g. Calculate the molar concentration of ascorbic acid in the solution before it was evaporated. i I M What was the pH of the ascorbic acid solution before it was evaporated? pH = i What was the concentration of the ascorbate ion, C6H6062, before the solution was evaporated? i M

Ascorbic acid, H2C6H6O6, is a diprotic acid usually known as vitamin C. For this acid, pKa1 is 4.10 and pKa2 is 11.79. When 125 mL of a solution of ascorbic acid was evaporated to dryness, the residue of pure ascorbic acid had a mass of 4.14 g. Calculate the molar concentration of ascorbic acid in the solution before it was evaporated. i I M What was the pH of the ascorbic acid solution before it was evaporated? pH = i What was the concentration of the ascorbate ion, C6H6062, before the solution was evaporated? i 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...

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Ascorbic acid, H2C6H6O6, is a diprotic acid usually known as vitamin C. For this acid, pKa1 is 4.10 and pKa2 is 11.79. When 125 mL of a solution of ascorbic acid was evaporated to dryness, the residue of pure ascorbic acid had a mass of 4.14 g. Calculate the molar concentration of ascorbic acid in the solution before it was evaporated. i I M What was the pH of the ascorbic acid solution before it was evaporated? pH = i What was the concentration of the ascorbate ion, C6H6062, before the solution was evaporated? i M
The amount of tartaric acid is responsible for the tartness of wine and controls the acidity of the wine. Tartaric acid also plays a very significant role in the overall taste, feel and color of a wine. Tartaric acid is a diprotic organic acid The chemical formula for tartaric acid is C4H6O6 and its structural formula is HO2CCH(OH)CH(OH)CO2H. A 50.00 mL sample of a white dinner wine required 21.48 mL of 0.03776 M NaOH to achieve a faint pink color. Express the acidity of the wine in terms of grams of tartaric acid, H2C4H4O6 (M. M. = 150.10) per 100 mL of wine. Assume that the two acidic hydrogens are titrated at the end point. MM H2C4H4O6 = 150.10 MM NaOH = 40.00 Below is the balanced chemical equation for this titration.
Calculate the pH of a 0.020 M solution of phenylacetic acid, C6H5CH2COOH. What will be the pH if the solution is made 0.050 M with its sodium salt, C6H5CH2COONa? Ka= 4.9 x 10-5.
A 20 ml solution of 0.1 M glycine hydrochloride has been prepared. How many moles of the weak acid and conjugate base forms of glycine are present after the addition of 620 µl of 1.0 M NaOH? What is the pH of the resulting solution?
Explain the effect of the pH on the protonation of the functional groups present in ascorbic acid (C6H8O6) and citric acid (C6H8O7).
Physiological pH in humans is pH = 7.3. At this pH, would cellular carboxylic acid citric acid (Kal 7.08 x 104) exist primarily as the undissociated free acid or as its dissociated carboxylate form? From the choices provided below, indicate whether the carboxylic acid will exist primarily in its protonated form as a Free Acid or in its deprotonated form as a Carboxylate Anion by clicking on the corresponding button. At equilibrium in this pH, the concentration of the preferred form of the acid is approximately | times higher than the concentration of its conjugate form. Round to the nearest order of magnitude.
PAP Chemistry-2903012-42100P-1/ Le Chatelier's Principle/ Lesson 128 2. Zinc (Zn) granules react slowly with dilute hydrochloric acid (HCI), but much faster if the acid is concentrated. Zn(s) 2HCI(aq)ZnCl2(aq) + H2(g) Zinc + Hydrochloric Acid Zinc Chloride + Hydrogen What causes the reaction to proceed faster with concentrated acid? The concentrated hydrochloric acid causes more hydrogen gas to be produced. The pressure of hydrogen gas molecules increases as concentration increases. The concentrated hydrochloric acid molecules move faster than in dilute acid. There are more collisions between the zinc and concentrated hydrochloric acid. PREVIOU
For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36
How do I fill out this chart Reactions: NaHCO3(s) + HCl(aq) → NaCl(s) + CO2(g) + H2O(l) Na2CO3(s) + 2HCl(aq) → 2NaCl(s) + CO2(g) + H2O(l)
Acetylsalicylic acid (aspirin) can be synthesized by combining salicylic acid and acetic acid through a condensation reaction. The −OH−OH group from phenol on the salicylic acid condenses with the carboxylic acid group of acetic acid forming acetylsalicylic acid. Draw the structure of acetylsalicylic acid.
What is the pH of an aqueous solution containing 0.50 mol L–1 ethanoic acid, 0.30 mol L–1 sodium ethanoate, and 0.10 mol L–1 HCl? [The pKa of ethanoic acid is 4.75.]
A monobasic acid has a neutralization equivalent of 136 + 1. This acid burns with a sooty flame, gives negative tests for nitrogen, sulfur and the halogens, and is insoluble in water and 5% NaOH. Give a possible structure for this monobasic acid.