Organic Chemistry (8th Edition)
8th Edition
ISBN: 9780134042282
Author: Paula Yurkanis Bruice
Publisher: PEARSON
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Textbook Question
Chapter 2.11, Problem 49P
Write the equation that shows how a buffer made by dissolving CH3COOH and CH3COO–Na+ in water prevents the pH of a solution from changing appreciably when
- a. a small amount of H+ is added to the solution.
- b. a small amount of HO– is added to the solution.
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Chapter 2 Solutions
Organic Chemistry (8th Edition)
Ch. 2.1 - Which of the following are not acids? CH3COOH CO2...Ch. 2.1 - Consider the following reaction: a. What is the...Ch. 2.1 - Draw the products of the addbase renc1 ion when a....Ch. 2.1 - a. What is the conjugate acid of each or the...Ch. 2.2 - a. Which is a stronger acid: one with a pKa of 5.2...Ch. 2.2 - An acid has a Ka of 4.53 106 in water. What is...Ch. 2.2 - Prob. 7PCh. 2.2 - Antacids are compounds that neutralize stomach...Ch. 2.2 - Are the following body fluids acidic or basic? a....Ch. 2.3 - Draw the conjugate acid of each of the following:...
Ch. 2.3 - a. Write an equation showing CH3OH reacting as an...Ch. 2.3 - Estimate the pKa values of the following...Ch. 2.3 - a. Which is a stronger base: CH3COO or HCOO? (The...Ch. 2.3 - Using the pKa values in Section 2.3, rank the...Ch. 2.4 - Prob. 15PCh. 2.5 - a. For each of the acid-base reactions in Section...Ch. 2.5 - Ethyne has a pKa value of 25, water has a pKa...Ch. 2.5 - Which of the following bases can remove a proton...Ch. 2.5 - Calculate the equilibrium constant for the...Ch. 2.6 - Rank the ions (CH3, NH2, HO, and F) from most...Ch. 2.6 - Rank the carbanions shown in the margin from most...Ch. 2.6 - Which is the stronger acid?Ch. 2.6 - Prob. 23PCh. 2.6 - What reaction in Problem 23 has the smallest...Ch. 2.6 - Rank the halide ions (F, Cl, Br, and l) from...Ch. 2.6 - a. Which is more electronegative, oxygen or...Ch. 2.6 - Which is a stronger acid? a. HCl or HBr b....Ch. 2.6 - a. Which of the halide ions (F, Cl, Br, and l) is...Ch. 2.6 - Which is a stronger base? (The potential maps in...Ch. 2.7 - What is a stronger acid? a. CH3OCH2CH2OH or...Ch. 2.7 - Rank the following compounds from strongest add to...Ch. 2.7 - What is a stronger base?Ch. 2.8 - For each of the following compounds, indicate the...Ch. 2.8 - Prob. 35PCh. 2.8 - Which is a stronger acid? Why?Ch. 2.8 - Fosamax (shown on the previous page) has six...Ch. 2.9 - Using the table of pKa values given in Appendix I,...Ch. 2.10 - For each of the following compounds (here shown in...Ch. 2.10 - As long as the pH is not less than _______, at...Ch. 2.10 - a. Indicate whether a protonated amine (RN+H3)...Ch. 2.10 - A naturally occurring amino acid such as alanine...Ch. 2.10 - a. At what pH is the concentration of a compound,...Ch. 2.10 - For each of the following compounds, indicate the...Ch. 2.10 - Given the data in Problem 47: a. What pH would you...Ch. 2.11 - Write the equation that shows how a buffer made by...Ch. 2.12 - Draw the products of the following react ions. Use...Ch. 2.12 - What product are formed when each of the following...Ch. 2 - Which is a stronger base? a. HS or HO b. CH3O or...Ch. 2 - According to the explanations by Lewis, if a...Ch. 2 - a. Rank the following alcohols from strongest to...Ch. 2 - a. Rank the following carboxylic acids from...Ch. 2 - Prob. 57PCh. 2 - For the following compound. a. draw its conjugate...Ch. 2 - Rank the following compounds from strongest to...Ch. 2 - Prob. 60PCh. 2 - Prob. 61PCh. 2 - a. Rank the following alcohols from strongest to...Ch. 2 - A single bond between two carbons with different...Ch. 2 - For each compound, indicate the atom that is most...Ch. 2 - a. Given the Ka values, estimate the pKa value of...Ch. 2 - Tenormin, a member of the group of drugs known as...Ch. 2 - From which of the following compounds can HO...Ch. 2 - a. For each of the following pairs of reactions,...Ch. 2 - Prob. 69PCh. 2 - Which is a stronger acid? a. b. c. d.Ch. 2 - Prob. 71PCh. 2 - Prob. 72PCh. 2 - Given that pH+ pOH = 14 and that the concentration...Ch. 2 - How could you separate a mixture of the following...Ch. 2 - Prob. 75PCh. 2 - a. If an add with a pKa of 5.3 is in an aqueous...Ch. 2 - Calculate the pH values of the following...Ch. 2 - Prob. 1PCh. 2 - Prob. 2PCh. 2 - Prob. 3PCh. 2 - Which of the reactions in Problem 3 favor...Ch. 2 - Prob. 5PCh. 2 - Prob. 6PCh. 2 - Prob. 7PCh. 2 - Which is the stronger acid? a. ClCH2CH2OH or...Ch. 2 - Prob. 9PCh. 2 - Prob. 10PCh. 2 - Which is a more stable base? Remembering that the...Ch. 2 - Which is the Stronger acid?Ch. 2 - Prob. 13PCh. 2 - a. Draw the structure of (CH3COOH (pKa = 4.7) at...
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- A solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a Write the net ionic equation that represents the reaction of this solution with a strong acid. b Write the net ionic equation that represents the reaction of this solution with a strong base. c To 100. mL of this solution, 10.0 mL of 1.00 M HCl is added. How many moles of NH3 and NH4+ are present in the reaction system before and after the addition of the HCl? What is the pH of the resulting solution? d Why did the pH change only slightly upon the addition of HCl?arrow_forwardUse the same symbols as in Question 61 ( = anion, =OH) for the box below. (a) Fill in a similar box (representing one liter of the same solution) after 2 mol of H+ (2) have been added. Indicate whether the resulting solution is an acid, base, or buffer. (b) Follow the directions of part (a) for the resulting solution after 2 mol of OH- (2 ) have been added. (c) Follow the directions of part (a) for the resulting solution after 5 mol of OH- (5 ) have been added. (Hint: Write the equation for the reaction before you draw the results.)arrow_forwardSodium benzoate, NaC7H5O2, is used as a preservative in foods. Consider a 50.0-mL sample of 0.250 M NaC7H5O2 being titrated by 0.200 M HBr. Calculate the pH of the solution: a when no HBr has been added; b after the addition of 50.0 mL of the HBr solution; c at the equivalence point; d after the addition of 75.00 mL of the HBr solution. The Kb value for the benzoate ion is 1.6 1010.arrow_forward
- . A buffered solution is prepared containing acetic acid, HC2H3O2, and sodium acetate, NaC2H3O2, both at 0.5 M. Write a chemical equation showing how this buffered solution would resist a decrease in its pH if a few drops of aqueous strong acid HCI solution were added to it. Write a chemical equation showing how this buffered solution would resist an increase in its pH if a few drops of aqueous strong base NaOH solution were added to it.arrow_forwardIdentify each pair that could form a buffer. (a) HCl and CH3COOH (b) NaH2PO4 and Na2HPO4 (c) H2CO3 and NaHCO3arrow_forwardWrite an equation for each of the following buffering actions. a. the response of a HPO42/PO43 buffer to the addition of OH ions b. the response of a HF/F buffer to the addition of OH ions c. the response of a HCN/CN buffer to the addition of H3O+ ions d. the response of a H3PO4/H2PO4 buffer to the addition of H3O+ ionsarrow_forward
- A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the following statements is most likely to be correct? a The pH of the solution at the equivalence point is 7.0. b The pH of the solution is greater than 13.0. c The pH of the solution is less than 2.0. d The pH of the solution is between 2.0 and 7.0. e The pH of the solution is between 7.0 and 13.0. The reason that best supports my choosing the answer above is a Whenever a solution is titrated with a strong acid, the solution will be very acidic. b Because the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. c Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidic.arrow_forwardAn important component of blood is the buffer combination of bicarbonate ion and carbonic acid. Consider blood with a pH of 7.42. a What is the ratio of [H2CO3] to [HCO3]? b What does the pH become if 15% of the bicarbonate ions are converted to carbonic acid? c What does the pH become if 25% of the carbonic acid molecules are converted to bicarbonate ions?arrow_forwardTwo samples of 1.00 M HCl of equivalent volumes are prepared. One sample is titrated to the equivalence point with a 1.00 M solution of sodium hydroxide, while the other sample is titrated to the equivalence point with a 1.00 M solution of calcium hydroxide. a Compare the volumes of sodium hydroxide and calcium hydroxide required to reach the equivalence point for each titration. b Determine the pH of each solution halfway to the equivalence point. c Determine the pH of each solution at the equivalence point.arrow_forward
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