ALEKS 360 AC INTRD CHEM >I<
5th Edition
ISBN: 9781260977585
Author: BAUER
Publisher: MCG
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Chapter 13, Problem 101QP
Interpretation Introduction
Interpretation:
The change on titrating an acid of
Concept Introduction:
Indicators are brightly coloured organic dyes and are weak acids and bases. They give different colours in different
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Chapter 13 Solutions
ALEKS 360 AC INTRD CHEM >I<
Ch. 13 - How do acids and bases differ from other...Ch. 13 - Prob. 2QCCh. 13 - Prob. 3QCCh. 13 - Prob. 4QCCh. 13 - Prob. 5QCCh. 13 - Prob. 6QCCh. 13 - Prob. 1PPCh. 13 - Prob. 2PPCh. 13 - Prob. 3PPCh. 13 - Prob. 4PP
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- For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forwardWhich of the acid-base indicators discussed in this chapter would be suitable for the titration of (a) HNO3 with KOH. (b) KOH with acetic acid. (c) HCl with NH3. (d) KOH with HNO2. Explain your answers.arrow_forward8-58 What is the connection between buffer action and Le Chatelier's principle?arrow_forward
- In Part A, a 15.00 mL aliquot of a 0.155 mol L-1 3-methylbutanoic acid solution was titrated to its equivalence point with 11.7 mL of 0.198 molL-1 NaOH solution. At the equivalence point, all of the weak acid, 3-methylbutanoic acid, is converted to its weak conjugate base, 3-methylbutanoate. What is the pH at this equivalence point? 6.957 4.770 8.855 5.145 O 9.230arrow_forwarda) Calculate the molar ratio of formic acid/sodium formate to prepare a pH-4.00 buffer solution. b) If you have 1.000 g of formic acid dissolved in 1 L of water, how many grams of sodium formate do you need to add to this solution to prepare the pH-4.00 buffer?arrow_forwardWhich one of the buffer solutions (pH 4.20 or pH 4.90) demonstrated the least change in pH, and hence the best buffering ability, upon the addition of the 2 ml NaOH? Explain why.arrow_forward
- a) Why can you not prepare a solution of pH = 8 by diluting sufficiently a 0.01 M solution of HCl with water? b) You could determine Ka for benzoic acid by measuring the pH of a 0.010 M solution of benzoic acid. Why is the graphical method used in this experiment a better way of determining Ka? c) List the measurements along with their uncertainties made in the determination of the molar mass of benzoic acid. Calculate the uncertainty in the mola r mass of benzoic acid determined by the titration.arrow_forwardCreate a titration curve when 13 mL of 0.12 M HCl is titrated with 0.09 M NaOH. Generate a titration curve when 23.0 mL of 0.15 M NaOH is titrated with a 0.61 M HCl.arrow_forward8-39. (a) Write the chemical reactions whose equilibrium constants are K and K for imidazole and imidazole hydrochloride, respectively. (b) Calculate the pH of a solution prepared by mixing 1.00 g of imida- zole with 1.00 g of imidazole hydrochloride and diluting to 100.0 mL. (c) Calculate the pH of the solution if 2.30 mL of 1.07 M HC1O4 are added.arrow_forward
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