A chemist prepared aqueous solutions of two weak acids: solution A is hydrazoic acid (HN3), and solution B is propanoicacid (HC2H5CO2). At 25°C, the acid-dissociation constant (Ka) for hydrazoic acid is 2.5x 10-5 and the base-dissociationconstant (Kb) for the propanoate ion (C2H5CO2) is 7.8 x 10-10, Determine the following.(a) the Ka value for propanoic acid (HC2H5CO₂)(b) the Kы value for the azide ion (N3)(c) the stronger acid between hydrazoic acid and propanoic acidhydrazoic acidpropanoic acid(d) the stronger base between the azide ion and the propanoate ionazide ionTutorialpropanoate ion

A. Ka = 1.3x10-5B. Kb = 4.0x10-10C. hydrazoic acidD. propanoate ion Explanation:Given:…

Answered: A chemist prepared aqueous solutions of…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.30QE

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Similar questions

What is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?
Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2
Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
Which of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?
Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion
Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
Malic acid is a weak diprotic organic acid with Ka1 = 4.0 104 and Ka2 = 9.0 105. a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about one molar in malic acid. c Calculate the pH of a 0.0175 M malic acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentrationin in solutions b and c?
CH3CH2CO2H , Ką = 1.3 x 105 CH3CH2CO2 , Kp = 7.7 x 10-10 F, Kp = 1.4 x 10-11 HF , Ką = 7.2 x 10-4 For the reaction between propanoic acid (CH3CH2CO2H) and a solution containing fluoride ions (F"): (a) The name of the conjugate base produced is (b) The name of the conjugate acid produced is (c) The reaction is favoured (write 'reactant' or 'product'), because the reactants are the (write 'weaker' or 'stronger') set of acid and base.
The polyprotic acid, H3X, has acid dissociation constants Kaj = 5.6×10-1, Ka2 = 2.8×10-3, and Kaz = 1.4x10-4. What is the K, value of the following reaction at 25°C? НаX (ад) + ОН (ад) — нх?-(ад) + Нә0(1) Report your answer to two significant figures using E notation.
Calculate the degree of dissociation (%) for a 0.10 M aqueous solution of hydrogen cyanide (HCN) at a temperature, where its acid constant value is pKHCN = 9.2.
1.) Use the following acid or base dissociation constants to calculate the pH of the listed aqueous solutions. Acid Ка Base Kb hypochlorous acid, HCIO 4.0 x 10 8 methylamine, CH3NH2 5.0 x 104 hydrofluoric acid, HF 6.3х 104 pyridine, CSH5N 1.7 x 109 formic acid, HCOOH 1.8 x 104 ammonia, NH3 1.8 x 105 a.) pH of 0.155 M Ba(OH)2 b.) pH of 0.750 M hypochlorous acid, HCIO c.) pH of 0.215 M CH3NH3CI(aq)

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