For the following reaction, the products are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted- Lowry acids or bases. CN+NH₂OHHCN+NH₂OH NH,OH HCN CN NH₂OH Clear All Stronger Bronsted-Lowry acid Weaker Bronsted-Lowry acid Stronger Bronsted-Lowry base Weaker Bronsted-Lowry base Previous Next

For the following reaction, the products are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted- Lowry acids or bases. CN+NH₂OHHCN+NH₂OH NH,OH HCN CN NH₂OH Clear All Stronger Bronsted-Lowry acid Weaker Bronsted-Lowry acid Stronger Bronsted-Lowry base Weaker Bronsted-Lowry base Previous Next

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter4: Polar Bonds, Polar Reactions

Section: Chapter Questions

Problem 15E: Mark each of the following statements True or False: a. The conjugate base of a strong acid is...

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Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
Write two BrnstedLowry acid-base reactions and show how they represent proton-transfer reactions.
Explain why equilibrium arrows are used in the ionization equations for some acids.
. a. Write the conjugate acid for each of the following Brønsted-Lowry bases. NO3.HSO4,ClO4,NH3,HCO3b. Write the conjugate base for each of the following Brønsted- Lowry acids. HCI,H2SO4,NH3,NH4,HCO3
In the following net ionic reaction, identify each species as either a Brnsted-Lowry acid or a Brnsted -Lowry base: CH3COO(aq)+HS(aq)CH3COOH(aq)+S2(aq). Identify the conjugate of each reactant and state whether it is a conjugate acid or a conjugate base.
Write equations to illustrate the acid-base reaction when each of the following pairs of Brnsted acids and bases are combined: Acid Base a.HOCl H2O b.HClO4 NH3 c.H2O NH2 d.H2O OCl e.HC2O4 H2O
Calculate the pH and the pOH of each of the following solutions at 25 C for which the substances ionize completely: (a) 0.200 M HCl. (b) 0.0143 M NaOH. (c) 3.0 M HNO3. (d) 0.0031 M Ca(OH)2
Explain the difference between a strong acid and a weak acid.
For each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) NH4+(aq) + Br(aq) NH3(aq) + HBr(aq) (b) HPO42(aq) + CH3CO2(aq) PO43(aq) + CH3CO2H(aq) (c)[Fe(H2O)6]3+(aq) + HCO3(aq) [Fe(H2O)5(OH)]2+(aq) + H2CO3(aq)
. In each of the following chemical equations, identify the conjugate acid-base pairs. a. NH3(aq)+H2O(l)NH4+(aq)+OH(aq) b. PO43(aq)+H2O(1)HPO42(aq)+OH(aq) c. C2H3O2(aq)+H2O(l)HC2H3O2(aq)+OH(aq)
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()
Predict which of these acid-base reactions are product-favored and which are reactant-favored. In each case write a balanced equation for any reaction that might occur, even if the reaction is reactant-favored. Consult Table 14.2 if necessary. H2O(ℓ) + HNO3(aq) H3PO4(aq) + H2O(ℓ) CN−(aq) + HCl(aq)