1) CH3COO¯ (aq) + HCIO (aq) CH3COOH (aq) + CIO (aq) 2) NO2 (aq) + CH3COOH (aq)HNO2 (aq) + CH3COO¯ (aq) 3) HCIO (aq) + NO2 (aq)CIO (aq) + HNO2 (aq) Arrange the substances based on their relative acid strength. HCIO Clear All HNO 2 strongest acid CH3COO¯ intermediate acid CH3COOH weakest acid NO2 not a Bronsted-Lowry acid CIO-

1) CH3COO¯ (aq) + HCIO (aq) CH3COOH (aq) + CIO (aq) 2) NO2 (aq) + CH3COOH (aq)HNO2 (aq) + CH3COO¯ (aq) 3) HCIO (aq) + NO2 (aq)CIO (aq) + HNO2 (aq) Arrange the substances based on their relative acid strength. HCIO Clear All HNO 2 strongest acid CH3COO¯ intermediate acid CH3COOH weakest acid NO2 not a Bronsted-Lowry acid CIO-

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...

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Which of the following is a Bronsted-Lowery acid-base reaction? O Al(s) + 2 HNO3(aq) Al(NO3)2(aq) + H2l8) O soals) + H2O(U) H,SO,laq) O 2 KOH(aq) + H2CO3(aq) K2CO3(aq) + H2O() O CaBrylaq) + 2 HCI(aq) CaCl2{aq) + H2ls) + Brz3) O None of the above Methane, CH4, can be synthesized by reacting hydrogen with carbon monoxide: H2 + CO → CH4 + H2O Balance this equation and determine how many grams of CH4 are produced when 100.0 g of H2 react. O 16.54 g O 49.16 g O 148.8 g O 265.3 g O 795.8 g
Choose the answer that has the appropriate acid and base that would make this neutralization reaction: Acid + Base --> H2O(l) + KCl(aq) HK(aq) + ClOH(aq) HCl(aq) + KOH(aq) H2Cl(aq) + KOH(aq) H2O(l) + KCl(aq)
Identify the Bronsted-Lowry acid and base on the left side of the equation and the conjugate acid and conjugate base on the right side. HBr0 (aq) + H,0 (I) H30* (aq) + Bro (aq) HSO, (aq) + HCO, (aq) so, (aq) + H,CO3 (aq) 2- HSO; (aq) + H,0* (aq) H,SO; (aq) + H,0 (1)
Identify the conjugate acid-base pairs: (a) CH3COOH(aq) + H2O(l) CH3COO2(aq) + H3O1(aq) (b) H2O(l) + F 2(aq) OH2(aq) + HF(aq)
HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A−? Group of answer choices HA(aq) + H2O(l) ⇌ H2A+(aq) + OH− A−(aq) + H3O+(aq) ⇌ HA (aq) + H2O(l) HA(aq) + OH−(aq) ⇌ H2O(l) + H+(aq) A−(aq) + H2O(l) ⇌ HA(aq) + OH−(aq) A−(aq) + OH−(aq) ⇌ HOA2−
Which of the acid-base reactions below would be reactant-favoured? Select one or more: NH4*(aq) + CO²(aq) = NH3(aq) + HCO3(aq) HPO4² (aq) + NH4*(aq) = H₂PO4 (aq) + NH3(aq) CN-(aq) + H₂O(aq) = HCN(aq) + OH(aq) CN (aq) + H₂SO3(aq) = HCN(aq) + HSO3(aq) HCO3(aq) + H₂S(aq) = H₂CO3(aq) + HS (aq) Check
Consider the following reaction: HF(aq) + NH3(aq) 2 NH4*(aq) + F'(aq) In this reaction NH4*(aq) is: the conjugate acid of HF(aq) the conjugate acid of NH3(aq) the conjugate base of NH3(aq) the conjugate base of HF(aq)
Select the conjugate acid-base pairs for the reaction: CH3CO2H(aq) + H2O(l) ↔ CH3CO2-(aq) + H3O+(aq)
31. For each reaction, identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conju- gate base. (a) HBr(aq) + H₂O(l) →→→ H3O+ (aq) + Br¯(aq) (b) NH3(aq) + H₂O(l) — NH4+ (aq) + OH¯(aq) (c) HNO3(aq) + H₂O(1) H3O+ (aq) + NO3¯(aq) (d) C₂H5N(aq) + H₂O(l) — C₂H5NH+ (aq) + OH¯(aq)
What is the approximate K for the following acid/base reaction? H25 (aq) +F (aq) ++ HF (aq) +HS (aq) ACID BASE HCI C H2SO4 HNO3 H30 (aq) HSO H3PO4 HSO NO3 H2O so, H,PO, F HF CH3COOH H,CO3 H,S H,PO, NH, CH;COO HCO, HS HPO, NH, CO PO OH HCO HPO. 1,0 OH H, CH CH, OA unable to determine OB. K.<1 Base strength increasing Acid strength increasing
Select the reaction that depicts the ionization of a weak acid in water. Group of answer choices HNO3(aq) + H2O(l) ⇌ NO3‒(aq) + H3O+(aq) NH3(aq) + H2O(l) ⇌ NH2‒(aq) + H3O+(aq) NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH‒(aq) HF(aq) + H2O(l) ⇌ F‒(aq) + H3O+(aq)
In the reaction HPO 2 (aq) + H20(1) PO,3-(aq) + H30* (aq) HPO (aq) is the H20(1) is the PO43 (aq) is th and H30*(aq) is the Bronsted Lowry acid Bronsted Lowry base reactant product conjugate acid conjugate base