3. B.LA clonale Which of the following species can be both Bronsted-Lowry acids and ((f) Bronsted-Lowry bases? P B.L.B H₂O NH₂ CH3-C-CH3 H3O A accept H+ N III, IV b) II, IV (c) III d) I, IV 9" Consider the equilibrium PO4 + Н20 Which are the Bronsted-Lowry bases? HPO4 + он- Not a bronsted base PO4 PO4 C) PO4 and НРО4 -- and он- and H₂O 10- For the equilibrium CH3NH3 + + Aad H2O base B) CH3NH3+ H3O+ and H₂O D) H₂O E) H2O and and он- HPO4 the two substances which are both acids are: A) H₂O and C) CH3NH3+ and CH3NH2 сна инвесьм H30 HzO+H+ +H+ CH3NH2 + H3O+ C.B/ C.A/Acid base CH3NH3+ and H3O+ E) CH3NH2 and H₂O CH3NH3 gives 1 H' to H₂D, thus CH3NH3+ acts as an acid || For the following reaction, choose the set that represents the correct order (left to right) of species 1-4 in the following reaction and predict the direction of the equilibrium. (pKa =-9 for 1, pKa = -7 for 4) H2SO4 + CH3COOH- + OH the position of 1 2 pKa=476 HSO 3 + CH-C-OH 4 A. acid + base base + acid B. acid+base base + acid C. acid + base base + acid D. acid + base E. acid + base acid + base acid + base an equilibrium favors a weaker acid and a weaker base Stronger acid + Stronger base + weaker acid = weaker base 4

3. B.LA clonale Which of the following species can be both Bronsted-Lowry acids and ((f) Bronsted-Lowry bases? P B.L.B H₂O NH₂ CH3-C-CH3 H3O A accept H+ N III, IV b) II, IV (c) III d) I, IV 9" Consider the equilibrium PO4 + Н20 Which are the Bronsted-Lowry bases? HPO4 + он- Not a bronsted base PO4 PO4 C) PO4 and НРО4 -- and он- and H₂O 10- For the equilibrium CH3NH3 + + Aad H2O base B) CH3NH3+ H3O+ and H₂O D) H₂O E) H2O and and он- HPO4 the two substances which are both acids are: A) H₂O and C) CH3NH3+ and CH3NH2 сна инвесьм H30 HzO+H+ +H+ CH3NH2 + H3O+ C.B/ C.A/Acid base CH3NH3+ and H3O+ E) CH3NH2 and H₂O CH3NH3 gives 1 H' to H₂D, thus CH3NH3+ acts as an acid || For the following reaction, choose the set that represents the correct order (left to right) of species 1-4 in the following reaction and predict the direction of the equilibrium. (pKa =-9 for 1, pKa = -7 for 4) H2SO4 + CH3COOH- + OH the position of 1 2 pKa=476 HSO 3 + CH-C-OH 4 A. acid + base base + acid B. acid+base base + acid C. acid + base base + acid D. acid + base E. acid + base acid + base acid + base an equilibrium favors a weaker acid and a weaker base Stronger acid + Stronger base + weaker acid = weaker base 4

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 2CR

See similar textbooks

Similar questions

Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3
For each of the following reactions, indicate the BrĂ¸nsted-Lowry acids and bases. What are the conjugate acid/base pairs? (a) H3 O+(aq)+CN(aq)HCN(aq)+H2O (b) HNO2(aq)+OH(aq)NO2(aq)+H2O (c) HCHO2(aq)+H2OCHO2(aq)+H3 O+(aq)
Consider citric acid, H3C6H5O7, added to many soft drinks. The equilibrium constants for its step-wise ionization areKa1=7.5104 ,Ka2=1.7105, andKa3=4.0107. Write the overall net ionic equation and calculate K for the complete ionization of citric acid.
a. Write the conjugate base for each of the following Brensted- Lowry acids. Oj, H2SOj. HC1O4. NH/. H2CO, Write the conjugate acid for each of the following Bronsted- Lowry bases. ~. hso4- nh2- nh3, co32-
Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
8-112 Consider an initial 0.040 M hypobromous acid (HOBr) solution at a certain temperature. At equilibrium after partial dissociation, its pH is found to be 5.05. What is the acid ionization constant, Ka, for hypobromous acid at this temperature?
Consider a 0.60-M solution of HC3H5O3, lactic acid (Ka = 1.4 104). a. Which of the following are major species in the solution? i. HC3H5O3 ii. C3H5O3 iii. H+ iv. H2O v. OH b. Complete the following ICE table in terms of x, the amount (mol/L) of lactic acid that dissociates to reach equilibrium. c. What is the equilibrium concentration for C3H3O3? d. Calculate the pH of the solution.
Consider the following statements. Write out an example reaction and K expression that is associated with each statement. a. The autoionization of water. b. An acid reacts with water to produce the conjugate base of the acid and the hydronium ion. c. A base reacts with water to produce the conjugate acid of the base and the hydroxide ion.
Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?
Determine Ka for hydrogen sulfate ion, HSO4-. In a 0.10-M solution the acid is 29% ionized.