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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
Write the hydrolysis reaction for ethylamine, CH3CH2NH2 (aq). Below the reaction, label the Bronsted Lowry acid, Bronsted Lowry Base, conjugate acid, and conjugate base.
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- In which reaction does bicarbonate act as a Bronsted-Lowry base? O HCO (aq) + H₂O (1)→ H₂CO3 (aq) + OH- (aq) O H₂CO3 (aq) → CO2 (9) + H₂O (1) O HCO (aq) + NaOH (aq) → Nat (aq) + CO² (aq) + H₂O(l) O HCO3(aq) + H₂O (1)→ CO2 (aq) + H3O+ (aq)arrow_forward1) Complete the following reactions and identify the acid, base, conjugate acid and conjugate base. CH;CH,NH2 (aq) + H2O (1) a) CH;COOH (aq) + H,O (I) b) c) Identify the conjugate base and conjugate acid of each of the following. Conjugate Base Molecule Conjugate Acid HCO3 H20 HSO4- H2PO4arrow_forwardArrange the definitions of an acid in order of increasing specificity: Lewis acid Bronsted-Lowry acid Arrhenius acidarrow_forward
- Enter the formula for the conjugate base of HPO42− .Express your answer as a chemical formula.arrow_forwardUsing tne Brønstea-Lowry concept of acias ana bases, identiry the Brønsted-Lowry acid and base in eacn of the following reactions: HS (aq) + H20(1)→H2S(aq) + OH (aq) CH3NH2(g) + BBr3 (g)→CH3NH2BB13 (s) Drag the appropriate items to their respective bins. • View Available Hint(s) Brønsted-Lowry acid Brønsted-Lowry base Neitherarrow_forwardGive any three examples of soft base ?arrow_forward
- Ethylamine, C2H5NH2, is a weak base. A 0.65 M aqueous solution of ethylamine has a pH of 12.20. What is K₁ for ethylamine? Calculate the pH of a 0.63 M aqueous solution of ethylamine. Kb = pH =arrow_forwardA molecule that behaves as a Lewis acid will donate a hydrogen ion. may also behave as a Br∅nsted-Lowry base. cannot also behave as a Br∅nsted-Lowry acid. may also behave as a Br∅nsted-Lowry acid.arrow_forwardDetermine the pH of each of the following solutions. 0.19 M CH3NH3I(Kb(CH3NH2)=4.4×10^−4) Express your answer to two decimal places.arrow_forward
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