Use the References to access important values if needed for this questionIn the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base.(C,H3)3N(aq) + H,0(1)→ (C,H3)3NH*(aq) + OH(aq)B-LB-LThe formula of the reactant that acts as a proton donor isThe formula of the reactant that acts as a proton acceptor isSubmit AnswerRetry Entire Group8 more group attempts remainingCengage Learning Cengage Technical Suppoet98 F Rain coming

a Bronsted Lowry acid is a species that donates protons and a Bronsted Lowry base is a species that…

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Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter17: Acid-base(proton Transfer) Reactions

Section: Chapter Questions

Problem 12E

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In the following net ionic reaction, identify each species as either a Brnsted-Lowry acid or a Brnsted -Lowry base: CH3COO(aq)+HS(aq)CH3COOH(aq)+S2(aq). Identify the conjugate of each reactant and state whether it is a conjugate acid or a conjugate base.
Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 103 and Ka2 = 4.6 105. a Letting the symbol H2A represent tartaric 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 0.5 M in tartaric acid. c Calculate the pH of a 0 0250 M tartaric acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentration in solutions b and c?
Note whether hydrolysis occurs for each of the following ions. If hydrolysis doe occur, write the chemical equation for it. Then write the equilibrium expression for the acid or base ionization (whichever occurs). a CH3NH3+ b Cl c ClO2 d CO32+
The following illustration displays the relative number of species when an acid, HA, is added to water. a. Is HA a weak or strong acid? How can you tell? b. Using the relative numbers given in the illustration, determine the value for Ka and the percent dissociation of the acid. Assume the initial acid concentration is 0.20 M.
Boron trifluoride, BF3, and diethyl ether, (C2H5)2O, react to produce a compound with the formula BF3 : (C2H5)2O. A coordinate covalent bond is formed between the boron atom on BF3 and the oxygen atom on (C2H5)2O. Write the equation for this reaction, using Lewis electron-dot formulas. Label the Lewis acid and the Lewis base. Determine how many grams of BF3: (C2H5)2O are formed when 9.10 g BF3 and 23.3 g (C2H5)2O are placed in a reaction vessel, assuming that the reaction goes to completion.
A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein
12.63 For each of the following reactions, indicate the Bronsted-Lowrv acids and bases. What are the conjugate acid-base pairs? CN’(aq) + H2O(€) «=* HCN(aq) + OH’(aq) HCO}-(aq) + H,o+(aq) +* H2CO,(aq) + H,O(€) (C) CH,CtX)H(aq) + HS~(aq)i=i CH}COO"(aq) + H2S(aq)
Which of the following concentrations would be practically equal in a calculation of the equilibrium concentrations in a 0.134-M solution of H2CO3, a diprotic acid: [H3O+], [OH-], [H2CO3], [HCO3], [CO32-]? N0 calculations are needed to answer this question.
At 25 C, a 0.10% aqueous solution of adipic acid, C5H9O2COOH, has a pH of 3.2. A saturated solution of the acid, which contains 1.44 g acid per 100. mL of solution, has a pH = 2.7. Calculate the percent dissociation of adipic acid in each solution.
Strong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.
Note whether hydrolysis occurs for each of the following ions. If hydrolysis docs occur, write the chemical equation for it. Then write the equilibrium expression for the acid or base ionization (whichever occurs). a NO3 b OCl c NH2NH3+ d Br
Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the electronegative chlorine atom pulls electrons away from the OH bond and thus weakens it. Calculate the hydronium-ion concentration and the pH of a 0.0020 M solution of chloroacetic acid, Ka is 1.3 103.

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