a. What is the base ionization constant for CH,BrCOO-?Kb: CH-7-5ニフ7.14 x 10"CH zBV CoOlH Ś CHZBV C00b. What is the standard free energy of formation of CH2BRCOO ?CHz Br c O0c. What is the pH of a 0.027 M NACH;B1COO? Note: More space on next page.

The conjugate base of the CH2BrCOOH is CH2BrCOO-. Thus we can find the Ka of the weak acid from the…

a. What is the base ionization constant for CH2BrCOO ? Kp: CH -5 r ל ל- Ź CH2B CO0 – "CH 2BV COOlH b. What is the standard free energy of formation of CH2BrCOO ? c. What is the pH of a 0.027 M NaCH2BrCOO? Note: More space on next page.

a. What is the base ionization constant for CH2BrCOO ? Kp: CH -5 r ל ל- Ź CH2B CO0 – "CH 2BV COOlH b. What is the standard free energy of formation of CH2BrCOO ? c. What is the pH of a 0.027 M NaCH2BrCOO? Note: More space on next page.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 70QAP: A 0.250 M solution of a weak base R2NH has a pH of 10.60 at 25C. What is G for the dissociation of...

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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
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.)
A 0.250 M solution of a weak base R2NH has a pH of 10.60 at 25C. What is G for the dissociation of the weak base in water at 25C? R2NH(aq)+H2OR2NH2+(aq)+OH(aq)
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
Final Volume V₂ = 341 mL al Volume V₁ =? 10. What is the molecular geometry and molecular polarity for CH₂Cl, and SO, ²? 11. What do catalysts do and how do they affect reaction rates? 12. 2 Atoms are side by side. Their chemical reactivity is dependent on the electrons which hold serve fe 13. Identify the acid, base, conj. Acid, conj. Base: H₂CO, + HPO4 H₂PO4 + HCO, 14. True or False? Chemistry looks at the microscopic view of matter. 15. Identify the 4 biological buffer mechanisms 16. Calculate the density of silver metal if 930 cm³ block has a mass of 2.21 x 104 g. Express the answer with the correct number of significant figures. 17. Kinetic molecular theory describes the behavior of which state of matter? 18. The pH scale operates on a logarithm scale which means an increase or decrease fold in the of pH is by 10s. So, a change in pH from 5 to 3 is a hydrogen ion concentration. And in other words, a pH of 3 has and less OH- than a pH of 5 19. A precipitate occurs in the reaction…
24. Methylamine, CH3NH4 is a weak base that ionizes in solution as shown by the following equation. CH3NH2 + H20 5 CH;NH;* + OH- (a) At 25 °C, the percentage ionization in a 0.160 molar solution of CH3NH2 is 4.7%. Calculate JOH], [CH3NH3'], [CH3NH2], [H3O*], and the pH of a 0.160-molar solution of CH3NH2 at 25 °C.
1. Complete the reaction NaOH → Na+¹ + i 2. What is the pH of a 0.001000 M NaOH solution ? first, find the [H3O+¹] using Kw Kw [ [H3O+¹] = [ |] [ pH = -log( a. acetic c. phosphoric g. sulfurous n. HPO3-2 u. 0.2500 aa. 2.6990 gg. 5.000 x 10-12 mm. conjugate acid b. hydrochloric [] d. perchloric e. hydrofluoric 1. Mg+2 S. HS-1 t. S-2 z. 1x 10-14 x. 1.000 x 10-3 y. 3.0000 CC. 11.0000 dd. 2 ee. 1 ff. 2.000 x 10-³ ii. 0.01250 jj. 0.22100 kk. 0.05656 II. acid pp. conjugate base -2 i. OH-1 j. H30+1 k. SO4² there is complete ionization f. sulfuric h. hydrosulfuric -2 0. H₂PO3-1 p. CO3-² q. HCO3-1 r. H₂S v. 0.1000 w. 0.02500 bb. 1.000 x 10-11 hh. 11.3010 oo. base m. Cl-1
H. | || The percent ionization of chloroacetic acid is less than that of fluoroacetic acid. :*-C-C-ö-H The percent ionizations cannot be compared without knowing the concentrations of the two acids. The structure of haloacetic acids, XCH,COOH (where X is The percent ionizations cannot be compared without knowing the pH of the solution. either F, Cl, Br, or 1), is shown above. The dissociation constants and molar masses of four haloacetic acids are listed in the table below. The percent ionization of chloroacetic acid is greater than that of fluoroacetic acid. Acid pK. K. Molar Mass(g/mol) CLEAR ALL Fluoroacetic acid 2.59 2.57 x 10–3 78.0 Chloroacetic acid 2.87 1.35 x 10–3 94.5 Bromoacetic acid 2.90 1.26 x 10-3 138.9 lodoacetic acid 3.18 6.61 × 10-4 185.9 An aqueous solution contains small but equal concentrations of both chloroacetic and fluoroacetic acids. Which statement comparing the percent ionizations of the two acids in the solution is true? エーO-
Activity 2. Self-ionization of water and pH, pOH, pKw »1. Write the law of mass action for the reaction of self-ionization of water and calculate the concentrations of [H;O*] and [OH]. H,0(1) + H20(1)= H30*(aq) + OH-(aq) Kw = 1.0x10-14 %3D 2 Since working with yery small powers of 10 can be inconvenient, we commonly use the mathematical
Delermine the (H*]. pH, and pOH of a solution with an JOH-| of 7.9 x 10-" Mal 25 °C. |#*| = M pli = pOH =
Calculate the pH at 25 °C of a 0.13M solution of trimethylammonium chloride ((CH;) NHCI 3 CH;),NHC!) Note that trimethylamine ((CH3),N) i is a weak base with a pK, of 4.19. b. Round your answer to 1 decimal place.
B E 1. CH₂MgBr 2.HO 1. Na(CN)BH, pH 4-5 2.H₂O CHÍNH, NAOH 1. CH CH2NH2, Na(CN)BH, pH 4-5 2. Neutralizing work-up Done