ANSWER
Ka | pKa | Kb | pKb |
9.96 | 1.1 ![]() |
0.000092 | 4.04 |
1.3 ![]() |
12.87 | 0.074 | 1.13 |
0.00711 | 2.15 | 1.4 ![]() |
11.85 |
5.2 ![]() |
13.28 | 0.19 | 0.72 |
PART 1
Kb = 0.000092
We have relation, pKb = - log Kb
pKb = - log 0.000092
pKb = 4.036
ANSWER : pKb = 4.04
We have relation, pKa + pKb = 14
pKa = 14 - pKb
pKa = 14 - 4.04
pKa = 9.96
ANSWER : pKa = 9.96
We have relation, pKa = - log Ka
Ka = 10 - pKa = 10 - 9.96 = 1.096
10 -10
ANSWER : Ka = 1.1
10 -10
PART 2
We have relation, pKa + pKb = 14
pKa = 14 - pKb
pKa = 14 -1.13
pKa = 12.87
ANSWER : pKa = 12.87
We have relation, pKa = - log Ka
Ka = 10 - pKa = 10 - 12.87 = 1.348
10 -13
ANSWER : Ka = 1.3
10 -13
We have relation, pKb = - log Kb
Kb = 10 - pKb = 10 - 1.13 =0.074
ANSWER : Kb = 0.074
PART 3
We have relation, pKa = - log Ka
pKa = - log 0.00711
pKa = 2.15
ANSWER :pKa = 2.15
We have relation, pKa + pKb = 14
pKb = 14 - pKa
pKb = 14 - 2.15
pKb = 11.85
ANSWER : pKb = 11.85
We have relation, pKb = - log Kb
Kb = 10 - pKb = 10 - 11.85 =1.4125
10 -12
ANSWER : Kb = 1.4
10 -12
PART 4
We have relation, pKa = - log Ka
Ka = 10 - pKa = 10 - 13.28 = 5.2481
10 -14
ANSWER : Ka = 5.2
10 -14
We have relation, pKa + pKb = 14
pKb = 14 - pKa
pKb = 14 -13.28
pKb = 0.72
ANSWER : pKb = 0.72
We have relation, pKb = - log Kb
Kb = 10 - pKb = 10 - 0.72 =0.1905
ANSWER : Kb = 0.19
1. (4 points) Complete the table below at 25 °C. | Ka рка Кь pKb 0.000092...
4.(4 points) What is the value of equilibrium constant for the system shown below at 25°C in terms of Ka HNO2 and Kb C5H5N? No2 (ag) + C6H5NH*(ag) = C6H5N(ag) + HNO2(ag) (а) Ка+ Kb (b) Ka - Kb (c) Ka/ Kb (d) Kw / (Ka Kb) (e) -Ka Kb) ОООО
Match the question with the best answer:
A. 2x 10-14 В. -log Ka C. pH 7 D. hydrogen ion donor рн E. water F. hydrogen ion acceptor рКа G. H30 OH т рКw H. -log [OH Concentration of [OH] in pure water 1. Ка т Кw Bronsted acid J.1 x 107 M Bronsted base К. 14 L. pH 7 Can act as both an acid and a base М. Кь N. 1 x 1014 O. -log [H30*] Р. рн <7
(C) (25%) Complete the table and calculations below to calculate the moments of inertia of the shape about the x axis and y-axis 3 in. 3 in. 6 in. n. 4 in. Shape (in4) (in) yo (in) (in) in (in')
Cryptography and Codes
4. Complete the addition table below, where P = (2,4), and Q = (0,0) are points on the elliptic curve y-x3 + 4x. 0 -P
4. Complete the addition table below, where P = (2,4), and Q = (0,0) are points on the elliptic curve y-x3 + 4x. 0 -P
1) Ammonia, NH3, is a monoprotic base with pKb = 4.74 at 25 °C. For 0.121 mol L−1 NH3(aq) at 25 °C, calculate (a) the percent ionization of NH3; and (b) the pH of the solution. 2) Hydrazoic acid, HN3, is a monoprotic acid with pKa = 4.72 at 25 °C. For 0.121 mol L−1 HN3(aq) at 25 °C, calculate (a) the percent ionization of HN3; and (b) the pH of the solution.
4. (4 points) Complete each of the acid base reactions below and determine which direction the reaction will favor. Use the Ka table below. a. NH" + CO2 b. HCN + H2PO4 → c. CH,COOH + HS → d. H2S + HCO » КА 7.5 x 10 Acid H3PO4 CH,COOH H.CO, HS 1.8 x 10% 4.3 x 107 9.1 x 10% 6.2 x 10* 6.2 x 10-10 5.6 x 10-0 H PO. HCN NH.
Given that Ka for HF is 6.3 × 10-4 at 25 °C, what is the value of Kb for F– at 25 °C? Given that Kb for CH3NH2 is 5.0 × 10-4 at 25 °C, what is the value of Ka for CH3NH3 at 25 °C?
Given that Ka for HCOOH is 1.8 � 10-4 at 25 �C, what is the value of Kb for COOH� at 25 �C? Kb=5.56 x10^-11 Given that Kb for CH3CH2NH2 is 1.7 � 10-9 at 25 �C, what is the value of Ka for CH3CH2NH3 at 25 �C? Ka=
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF) 7.2x10-4; Ka ([Al(H20).]+)7.9x10-6; Ka (H3PO4)=7.5x10-2: Ka (HPO42-) =3.6x10-13; Ka (HCI)=Huge; Ka(Na+)=tiny; Ka(Cl-)tiny; Kb(NH3)=1.8x10-5; Kw=1x10-14 1) Calculate the pH of aqueous 0.25M HCl and 0.25M HF solutions. 2) Complete the following tables for aqueous solutions of conjugate acid-base pKa pKb Kb 1.3x10-4 35 3) Complete the following table for aqueous solutions DHL TH+) OH) pOH 1x102 4) Calculate the pH of aqueous 0.15M Ba(OH)2 and...
4. (14 pts) Using the values in the table below reported at 25°C, determine the table below reported at 25°C, determine AH at 400°C for the hydrogenation of acetylene to ethane, C2H2(g) + 2 H2(g) → CzHed) Assume that Cp.m is independent of temperature for all species in the reaction. mol AN mol 296.13 $1.68 CH, CH, H