Organic Chemistry (8th Edition)
8th Edition
ISBN: 9780134042282
Author: Paula Yurkanis Bruice
Publisher: PEARSON
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Textbook Question
Chapter 2, Problem 76P
a. If an add with a pKa of 5.3 is in an aqueous solutions of solution of pH 5.7, what percentage of the acid is present in its acidic form?
b. At what pH does 80% of the acid exist in its acidic form?
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3.
Calculate the pH of the following solutions. Hint: some parts should
require very little math!
a. A 0.010 M solution of an acid that completely dissociates in solution.
b. A 0.010 M solution of an acid that's conjugate base has a pk of 8.2.
c. A solution that's comprised of 75% acid and 25% conjugate base with a Ka
= 1.4 x 10-4
d. A 0.100 M solution of sodium hydroxide.
In my slide, there is a table summarizing the pKa values for different acids.
(1) when ranking the acidity level (how strong the acids are), a low pKa means high acidity. Why is that?
(2) Calculate the phosphoric acid solution pH when the ratio of [H2PO4-]/[H3PO4] is 0.8.
1. Calculate the pH of a 1 L solution containing 6 mL of 1.5 M acetic acid and 5 mL of
0.4 M sodium acetate. The pKa of acetic acid is 4.76.
2. What is the ratio of conjugate base to acid of buffer (pKa=4.8) with pH=4.8?
Show your work.
3. Phosphate buffers are common in biochemistry lab. They can be made from
phosphoric acid (H;PO4):
pКа-2.15
pKa=7.20
pKa=12.35
H,PO,
H,PO,
HPO, 2 PO,*
Which acid/conjugate base would you use to prepare a buffer at pH=8.11?
Which acid/conjugate base would you use to prepare a buffer at pH=11.11?
Which acid/conjugate base would you use to prepare a buffer at pH=3.11?
4. Sulfhydryl groups are capable of ionizing (losing a proton). The pka of the side
chain of Cys is 8.18. Explain why Cys is drawn as -SH and not -S at physiological
pH.
5. Which of the amino acids below would most likely be found on the surface of a
protein? Which would be found on the inside of a globular protein? Explain your
answer.
Asp, Phe, Ser, Leu, Arg
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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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 5. The pKa of acetic acid (HA) is approximately 4.8. If a solution of acetic acid is brought to pH= 4.8, what can we say about the concentrations of HA and its conjugate base A? a) The solution is acidic so there is more HA than A. b) HA is a weak acid so it dissociates easily and [A'] is higher than [HA]. c) Their concentrations are the same. d) We can't say, it depends on the initial concentration of HA. e) We can't say, it depends on temperature.arrow_forwardSome weak acids and their pKa values are given below. Which one of these acids will have the STRONGEST conjugate base? Select one: a. Phenol; pKa = 10.00 b. Methanoic acid; pKa = 3.75 c. Bromoethanoic acid; pKa = 2.9 d. Methanol; pKa = 15.54arrow_forward7. Determine the K₁ of each of the following. a. A 0.00475 M solution of acid HY has a pH of 2.68. What is the Ka of HY? b. CICH₂COOH has a pKa of 2.87, what is the Ka of the acid? c. A base has a pKb of 5.14, what is the Ka of the conjugate acid? d. A 0.25 M solution of a weak acid is 3% dissociated, what is the Ka of the acid?arrow_forward
- Ajja what is the ph of a 0.10m solution of an acid with a pKa of 8.4?arrow_forward4. Compounds might have more than pKa. 5. We usually prefer to prepare buffers from alkaline origin compounds. 6. The pH of a buffer solution containing .1 M acetic acid and 0.1 M sodium acetate? (Ka for acetic acid = 1.75 ×10-5) is 3.9. 7. The pH of a solution containing ephedrine 0.1 M and ephedrine HCI 0.01 M? (Kb for ephedrine = 2.3 x 10-5) is 7.99. 8. The maximum buffer capacity for solutions can be achieved when the required pH double than pKa of the acid.. 9. When one of the buffer components is depleted completely the solution lose its buffering capacity and can no longer resist the change in pH. 10. At a hydrogen ion concentration of 1.75 x 10-5, what is the capacity of a buffer containing 0.10 mole each of acetic acid and sodium acetate per liter of solution? (Ka = 1.75 x 10-5 ) is 9.11.arrow_forward17. What is the pH of the solution produced when 50 mL of 0.25 M HCl is added to 250.0 mL of 0.1 M ammonia? [Given pKa of NH4 is 9.245] a. 4.755 b. 8.944 C. 9.245 d. 9.546arrow_forward
- If the concentration of an acid in solution is 2.2 times larger than the concentration of its conjugate base, and the pH of the solution is 3.5, what is the pKa of the acid? Include the answer to 3 significant figuresarrow_forwardThe pKa value is ammonia is 9.3. You are allergic to the odor of ammonia. You smelled an ammonia solution with the pH 9.3 yesterday and it was OK. Now you tried to smell the same solution but with the pH of 8.3. What will happen to your allergy symptom? How much better or worse it will be compared to yesterday? (e.g., ~5 times better or worse).arrow_forward1. What is the pH of a 0.2 M acetic acid solution where the Ka for acetic acid is 1.33 x 10-5 M. 2. What is the pH of a 0.1 M formic acid solution where the pka for formic acid is 3.77.arrow_forward
- Which statements about acid-base equilibria is/are Wrong? I. The pKa = log Ka. II. A strong acid has a negative pKa value. II. A stronger acid has a pKa with a larger value than a weaker acid. IV. The stronger the base, the smaller the pKa of its conjugate acid. Select one: O I, II, IV O II O , IV O II, IVarrow_forwardConsider a set of 0.100 M weak acid solutions with various pK values. Which one is the least acidic? pKa=7.3 pKa=4.4 OpKa=3.2 pKa=6.8 pKa=8.5arrow_forward3. The pH of the given solution of lactic acid and lactate is 4.30. Calculate the pKa of lactic acid, when the concentration of lactic acid and lactate are 0.020 M and 0.073 M respectively.arrow_forward
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