ül11. For the weak base piperidine, CSH10NH, K, = 1,30 x 10-3. What is the equilibriumconcentration of all species, the pH, % ionization, and pOH of a O.545 M solution ofpiperidine?108CらHioNI4 +H20 cg Itio NH2 t OH[coHiO NH2 ]•COH] = •0260 m[ cgHIO NH] =*Sしらーメ+ x tx* Sしら -入メPOH= 1.5851.30X10sPIt12,4115%3D•SIS - X4.lon= - 0260XIC0 = い、7%。※+1.30×1 -703×IG"ニ0×ニ,026012. What is the pH of a 0.459 M solution of NaCIO. Ka = 2.87 x 10-8(e) TH Skb=CHClot3 COHT kb= \xlo4NacIONat+ CIO%3DNeutralbasic2.87x10

11) Reaction- C5H10NH + H2O → C5H10NH2+ + OH-

11. For the weak base piperidine, CsHioNH, K. = 1.30 x 10-3. What is the equilibrium concentration of all species, the pH, % ionization, and pOH of a 0.545 M solution of piperidine? Cg HIONIH + H20 = CSItio NH2+ OH- 10 エSし1ら [COHIO NH2 I•COH] [ CgHIO NH] = = •0260 m ーメ + x tx • SLIS - X POH= I.S8らメ 1.30 X10s PIt %3D • SIS - X -6260 = いい17%。入IO0 文+1.30x10ー0るX10 ×ニ0260 ーい 12. What is the pH of a 0.459 M solution of NaCIO. Ka = 2.87 x 10-8

11. For the weak base piperidine, CsHioNH, K. = 1.30 x 10-3. What is the equilibrium concentration of all species, the pH, % ionization, and pOH of a 0.545 M solution of piperidine? Cg HIONIH + H20 = CSItio NH2+ OH- 10 エSし1ら [COHIO NH2 I•COH] [ CgHIO NH] = = •0260 m ーメ + x tx • SLIS - X POH= I.S8らメ 1.30 X10s PIt %3D • SIS - X -6260 = いい17%。入IO0 文+1.30x10ー0るX10 ×ニ0260 ーい 12. What is the pH of a 0.459 M solution of NaCIO. Ka = 2.87 x 10-8

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 3RQ

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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?
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?
8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?
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.)
Composition diagrams, commonly known as alpha plots, are often used to visualize the species in a solution of an acid or base as the pH is varied. The diagram for 0.100 M acetic acid is shown here. The plot shows how the fraction [alpha ()] of acetic acid in solution, =[CH3CO2H][CH3CO2H]+[CH3CO2] changes as the pH increases (blue curve). (The red curve shows how the fraction of acetate ion, CH3CO2, changes as the pH increases.) Alpha plots are another way of viewing the relative concentrations of acetic acid and acetate ion as a strong base is added to a solution of acetic acid in the course of a titration. (a) Explain why the fraction of acetic acid declines and that of acetate ion increases as the pH increases. (b) Which species predominates at a pH of 4, acetic acid or acetate ion? What is the situation at a pH of 6? (c) Consider the point where the two lines cross. The fraction of acetic acid in the solution is 0.5, and so is that of acetate ion. That is, the solution is half acid and half conjugate base; their concentrations are equal. At this point, the graph shows the pH is 4.74. Explain why the pH at this point is 4 74.
The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107
What is the ionization constant at 25 C for the weak acid CH3 NH3+, the conjugate acid of the weak base CH3NH2, Kb=4.4104.
A.) What is the pH of a 0.25 M solution of sodium propionate, NaC3H5O2, at 25°C? (For propionic acid, HC3H5O2, Ka = 1.3 x 10-5 at 25°C.) B.) What is the pH of a 0.79 M solution of methylamine (CH3NH2, Kb = 4.4 x 10–4) at 25oC?
An organic acid (HA) has a molecular weight of 100g/mol, a Kow = 5.6 and a K, = 2.7 x 10-2. If originally 2.0 g of the acid is dissolved in 100 mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100 mL of water, what will be the pH of the water? (Consider the equilibrium processes to be sequential and unrelated chemically) Possible answers: 1.89, 1.48, 2.01, 1.74, 1.61
The Ka for a weak acid is 1.2*10^-8. a. What is the equilibrium concentration of OH- in a 0.0020 M solution of the conjugate base? b. What is the equilibrium concentration of the undissociated conjugate base in a 0.0020 M solution of the conjugate base? c. What is the equilibrium pH of a 0.0020 M solution of the conjugate base?
Given that log Kso for Zr(OH)4(s) is 10-54.1, at what pH would the maximum concentration of Zr4+(aq) be 10-3 M?
Calculate the pH of an aqueous solution that is 3.24 x 10-1 M oxopropanoic acid and 0.101 M sodium oxoproanoate? [HINT: MW sodium oxopropanoate = 110.05 g/mol; Kaoxopropanoic acid = 3.30 x 10-3]