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 asolution of ascorbic acid was evaporated to dryness, the residue of pure ascorbic acid had a mass of 3.64 g.Your answer is correct.Calculate the molar concentration of ascorbic acid in the solution before it was evaporated. 0.164HintYour answer is partially correct.What was the pH of the ascorbic acid solution before it was evaporated? pH = 2.44What was the concentration of the ascorbate ion, C6H6062, before the solution was evaporated?iMM

Answered: Ascorbic acid, H2C6H6O6, is a diprotic…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 7P

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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.
The amino acid tyrosine has pKa = 2.20 for deprotonation of its carboxylic acid group. What are the relative concentrations of tyrosine and its conjugate base at a pH of (a) 7, (b) 2.2, (c) 1.5?
The pKb of the organic base nicotine (denoted Nic) is 5.98. Write the corresponding protonation reaction, the deprotonation reaction of the conjugate acid, and the value of pKa for nicotine.
1) Calculate the pH (aq., 25 °C) of a 0.073 M Novocaine (C13H21O2N2CI) solution, which is the salt of the base procaine and hydrochloric acid. The pKb of procaine = 5.155. oltion (lom 2) Calculate the pH (aq., 25 °C) of a 0.100 M potassium hypochlorite solution. The pKa of hypochlorous acid = 7.54.
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
a) Calculate the pH of an aqueous solution of the salt NaA, which was made to a concentration of 0.080 M NaA. The Ka of the weak acid HA is 2.0 x 10-5. Your pH should go to two places past the decimal point (i.e. 1.35). b) Aniline, C6H5NH2, has a pKb of 9.40. What is the pH of a solution which is 0.12 M in aniline and 0.38 M in anilinium ion, C6H5NH3+? Your answer should be to two places past the decimal.
What is the pH of a 0.10 M N(CH3)3(aq)? The base ionization constant of trimethylamine is Kb= 6.5×10–5. Enter your answer with correct units and significant figures.
Benzoic acid, HC7H5O2, and its salts are used as food preservatives. Ka for benzoic acid is 6,3 x 10–5. A solution of sodium benzoate, NaC7H5O2, in water has a concentration of 0,015 mol.dm–3. What is the pH of this solution?
Given the identity of the base, its concentration and pKb, determine the pH of a solution of the base. Show all work A student dissolves 0.750 moles ofNaA (where A is the anion/conjugate base of a generic weak monoprotic acid, HA) in 1 liter of water. What is the resulting pH of the solution if the generic acid (HA) has a pka of 3.26?
Calculate the pH at 25 °C of a 0.15M solution of lidocaine HC1 (C4H2,NONH,CI). Note that lidocaine (C14H2,NONH) is a weak base with a p K, of 7.94. Round your answer to 1 decimal place. pH = | olo Ar
ess impor The pH of an aqueous solution of 0.124 M sodium nitrite, NaNO2, is K₂ (HNO₂) = 4.50 × 10−4.) This solution is Submit Answe acidic basic neutral eferences to a Entire Group values if needed for this questio 9 more group attempts remaining (Assume that
Determine the principal species at the following pH levels for Nitrilotriacetic acid. The most protonated form is C6H10NO6+. pH= 1,2,3,4,10. pK1 = 1.0, pK2 = 1.81, pK3 = 2.52, pK4 = 9.46.

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