The Ka for ch3co2h is 1.8 x10^-5 and the Ka for ch2chco2h is 1.4x10^-3. what is the Kb of the weaker of their two respective conjugate bases?
a. 2.1 x10^-8
b. 7.1 x10^2
c. 6.7 x 10^-10
d. 6.7 x 10^4
e. 7.1 x 10^-12
The Ka for ch3co2h is 1.8 x10^-5 and the Ka for ch2chco2h is 1.4x10^-3. what is the Kb of the wea...
The Ka for ch3co2h is 1.8 x10^-5 and the Ka for ch2chco2h is 1.4x10^-3. what is the Kb of the weaker of their two respective conjugate bases? a. 2.1 x10^-8 b. 7.1 x10^2 c. 6.7 x 10^-10 d. 6.7 x 10^4 e. 7.1 x 10^-12
What is the most likely identity of the species undergoing
titration?
a) hydrobromic acid (HBr); Ka = 1.08 x 109
b) acetic acid (CH3CO2H); Ka = 1.8 x 10-5
c) ammonia (NH3); Kb = 1.8 x 10-5
d) sodium acetate (NaC2H3O2); Kb = 5.6 x 10-10
13 12 10 8 pH 7- 4 2 10 30 50 70 90 110
Given that Ka for HCN is 6.2 x10-10 at 25 °C, what is the value of Kb for CN at 25 C? Number Given that Kb for NH3 is 1.8 x 10 at 25 °C, what is the value of Ka for NH4 at 25 C? Number
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=
QUESTION 4 The Ka of HCHO2 is Ka=1.8 x 10-4. What is the value of Kb for CHO2"? Please enter answer in format 1E-2
Question 39 Calculate the Kb of Hypochlorous acid, Ka=3.5 x10^-8. (1 point) 1.3 x 10^-4 2.9 x 10^-7 O 3.1 x 10^-6 O 8.6 x 10^-4 Question 40 Calculate the pka of Hypochlorous acid, Ka- 3.5 x10^-8. (1 point) 5.32 6.64 8.92 None of the above
The following shows a list of weak acids and bases with their Ka and Kb values. Substances Ka Substances Kb Cyanic acid (HCN) 4.9 x 10-10 Ammonia (NH3) 1.8 x 10-5 Nitrous acid (HNO2) 4.5 x 10-4 Aniline (C6H5NH2) 4.3 x 10-10 Hydrofluoric acid (HF) 6.8 x 10-4 Pyridine (C5H5N) 1.7 x 10-9 Acetic acid (CH3COOH) 1.8 x 10-5 Methylamine (CH3NH2) 4.4 x 10-4 If you want to make a pH 8.0 buffer solution, which of the following acids or...
Consider the following acids and bases: HCO2H Ka = 1.8 × 10-4 HOBr Ka = 2.0 × 10-9 (C2H5)2NH Kb = 1.3 × 10-3 HONH2 Kb = 1.1 × 10-8 Choose substances from the following list that would be the best choice to prepare a pH = 9.0 buffer solution. (Select all that apply.) HONH2 KHCO2 HCO2H (C2H5)2NH (C2H5)2NH2Cl HOBr NaOBr HONH3NO3
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...
please show all work neatly
5. (2 pts) Consider the following acids and their dissociation constants HPO4-2(aq) + H2O.. H3O"(aq) + PO4-3(aq) Ka-2.2x 10.13 HCOOH(aq) H20 H3O (a) HCOO (aq) Ka = 1.8x10-4 a. Which is the weaker acid, HPO42 or HCOOH? b. What is the conjugate base of, HPO42 or c. Which acid has the weaker conjugate base? d. Which acid produces more ions? 6. (2 pts) Write a balanced equation for the neutralization of H3PO4(aq) and NaOH(aq) (3...