G.98. The following reactions all have K > 1.1) CN (aq) + HF (aq)2) CN (aq) + HC₂H₂O4 (aq)3) HF (aq) + C₂H704 (aq)Arrange the substances based on their relative base strength.C9H704F™CNC9H704FCNHC₂H704HFF (aq) + HCN (aq)HCN (aq) + C9H704 (aq)HC₂H₂O4 (aq) + F (aq)HCNClear Allstrongest baseintermediate baseces based on their relative base strength.[Review Topics]Clear Allstrongest baseintermediate baseweakest basenot a Bronsted-Lowrybase

According to conjugate acid base principle, a strong acid has a weak conjugate base and a weak acid…

The following reactions all have K > 1. 1) CN (aq) + HF (aq) 2) CN (aq) + HC₂H₂O4 (aq) 3) HF (aq) + C₂H704 (aq) Arrange the substances based on their relative base strength. C9H704 F" F (aq) + HCN (aq) HCN (aq) + C9H704 (aq) HC₂H₂O4 (aq) + F (aq) CN Clear All strongest base intermediate base

The following reactions all have K > 1. 1) CN (aq) + HF (aq) 2) CN (aq) + HC₂H₂O4 (aq) 3) HF (aq) + C₂H704 (aq) Arrange the substances based on their relative base strength. C9H704 F" F (aq) + HCN (aq) HCN (aq) + C9H704 (aq) HC₂H₂O4 (aq) + F (aq) CN Clear All strongest base intermediate base

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the pH of a solution made by adding 0.65 m of acetic acid (H3CO2H) and 0.30 mol of sodium acetate (H3CO2Na) to enough water to make a 1.0 L solution? (K, = 1.8 x 105) %3D CH3CO2H (aq) + H2O (1) CH3CO2° (aq) + H3O* (aq) 4.74 O 5.08 04.40 8.92
Write the dissociation equation for ammonium hydroxide in solution? Ammonium hydroxide does not dissociate. NH4OH(aq) ⟷ NH4(aq) + OH(aq) NH4OH(aq) ⟶ NH4+1(aq) + OH-1(aq) NH4OH(aq) ⟷ NH4+1(aq) + OH-1(aq) NH4OH(aq) ⟶ NH4(aq) + OH(aq)
Water can act as either an acid or a base. Which equation represents water reacting as an acid? Group of answer choices H2O(l) + NH3(g) ⟶ OH–(aq) + NH4+(aq) H2O(l) + HCl(aq) ⟶ H3O+ + Cl–(aq) H2O(l) ⟶ H2(g) + ½O2(g) H2O(l) + C(s) ⟶ CO(g) + H2(g)
please explain each and solve The following reactions all have K>1. 1) CH3CO0 (aq) + HF (aq) F (aq) + CH3COOH (aq) 2) CH3CO0 (aq) + HC9H704 (aq) CH3COOH (aq) + C9H704 (aq) 3) HF (aq) + C9H704 (aq) HC9H704 (ag) + F (aq) Arrange the substances based on their relative acid strength. Clear All HF strongest acid HC9H704 intermediate acid weakest acid CH3CO0 not a Bronsted-Lowry acid CH3COOH C9H704 F
Consider the following chemical equilibrium for the weak base CN in water: CN (aq) + H₂O(1) HCN(aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d H pH will go up; [OH-]will go up; net amount of OH will go up pH will go down; [OH-] will go up; net amount of OH will go down pH will go down: [OH-] will go down; net amount of OH will go down pH will go up; [OH will go up; net amount of OH will go down X Your answer
The following three equations represent equilibria that lie far to the right.HNO3(aq) + CN–(aq) HCN(aq) + NO3–(aq)HCN(aq) + OH–(aq) H2O(l) + CN–(aq)H2O(l) + CH3O–(aq) CH3OH(aq) + OH–(aq) Identify the strongest base. Question 20 options: A) CH3OH B) CH3O– C) H2O D) NO3– E) CN–
Question 6 CH;COOH(ag) + H2O(1) 2 H30t (aq) + CH3COO (ag) CH3COO (ag) + H2O(1) 2 CH3COOH(aq) + OH- (ag) 2 H2O(1) 2 H3O*(aq) + OH¯(aq) A buffer solution is made up of acetic acid (CH3COOH) and sodium acetate (NaCH3COO). The major equilibria in the buffer system are represented above. Which of the following equilibria could be used to support the claim that the addition of a small amount of NaOH to the buffer will result in only a very small change in pH? А CH3COOH(ag) + CH3COO (aq) 2 CH;COO (ag) + CH;COOH(aq) B CH;COOH(aq) + OH (aq) 2 CH3COO (ag) + H,O(1) H3O* (ag) + OH (ag) 2 2 H20(1) CH;COOH (ag) + H2O(1) 2 H;0* (ag) + CH3COO (ag)
Benzoic acid (C6H5COOH) and aniline (C6H5NH2) areboth derivatives of benzene. Benzoic acid is an acid withKa = 6.3 x10-5 and aniline is a base with Ka = 4.3 x10-10. (a) What are the conjugate base of benzoic acid andthe conjugate acid of aniline? (b) Anilinium chloride(C6H5NH3Cl) is a strong electrolyte that dissociates intoanilinium ions (C6H5NH3+) and chloride ions. Which willbe more acidic, a 0.10 M solution of benzoic acid or a 0.10M solution of anilinium chloride? (c) What is the value ofthe equilibrium constant for the following equilibrium?C6H5COOH(aq) + C6H5NH2(aq) ⇌ C6H5COO-(aq) + C6H5NH3+(aq)
One way to determine the predominant species at equilibrium for an acid-base reaction is to say that the reaction arrow points to the acid with the higher value of pK. For example, NH, + H,0 NH, + H,O+ pK. pk, 9.24 pK-1.74 NH,+ + OH--→ NH, + H,0 рк, 9.24 pK, 15.7 Explain why this rule works.
43. Which one of the following equations represents the ionization of a weak monoprotic acid in water? O CN (aq) + H 20(aq) HCN(aq) + OH (ag) O HCN(aq) + OH (aq) H20(1) + CN (aq) O HCN(aq) + H 20(1) H30*(aq) + CN (aq) O HCN(aq) + NH 3(aq) NH4CN(aq) O HCN(aq) + CH (aq) H2O(1) + CN (aq)
Indicate the acid and its conjugate base, and the base and its conjugate acid. HC1O4 (aq) + H₂O(l) → H3O+ (aq) + C1O4 (aq) HC1O4 (aq): H₂O(l): H3O+ (aq): C1O4 (aq): Drag and drop your selection from the following list to complete the answer: conjugate base acid base conjugate acid
10) When reaction (1) and (2) below are added together, the result is reaction (3). 1) H200) +HNO2aq) = H3O+aq) + NO2-aq) 2) H3O+aq) + OH-(aq) = 2 H204) 3) HNO2(ag) +OH-(aq) = NO2-(aq) + H2O() If K1 = 4.50 × 10-4, and K2 = 1.00 x 1014, find the equilibrium constant, K3.