In the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HClO2(aq) + H2O(l) = H3O+(aq) + ClO2 (aq) H2CO3(aq) + H2O(l) → H3O+(aq) + HCO3(aq) Answer Bank H2O(l) + CH3NH3(aq) = CH3NH2(aq) + H3O+ (aq) CA B CB A CH3COOH(aq) + H2O(1) = CH3COO¯(aq) + H3O+ (aq)

In the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HClO2(aq) + H2O(l) = H3O+(aq) + ClO2 (aq) H2CO3(aq) + H2O(l) → H3O+(aq) + HCO3(aq) Answer Bank H2O(l) + CH3NH3(aq) = CH3NH2(aq) + H3O+ (aq) CA B CB A CH3COOH(aq) + H2O(1) = CH3COO¯(aq) + H3O+ (aq)

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

Identify the reactant that is a Brønsted-Lowry acid and the reactant that is a Brønsted-Lowry base in each of the following: Part C 2- CO3² (aq) + H₂O = HCO3(aq) + OH-(aq) H₂O is the acid (proton donor); CO3² is the base (proton acceptor). H₂O is the acid (proton acceptor); CO² is the base (proton donor). O CO3²- is the acid (proton acceptor); H₂O is the base (proton donor). O CO² is the acid (proton donor); H₂O is the base (proton acceptor). Submit Part B Request Answer H₂SO4 (aq) + H₂O(1)→ H3O+ (aq) + HSO4 (aq) O H₂O is the acid (proton donor); H₂SO4 is the base (proton acceptor). O H₂SO4 is the acid (proton acceptor); H₂O is the base (proton donor). O H₂SO4 is the acid (proton donor); H₂O is the base (proton acceptor). O H₂O is the acid (proton acceptor); H₂SO4 is the base (proton donor). CH3-COO (aq) + H3O+ (aq) = H₂O(1) + CH3-COOH(aq) CH3-COO is the acid (proton acceptor); H3O+ is the base (proton donor). O H3O+ is the acid (proton donor); CH3-COO is the base (proton acceptor). O…
Match the acid to the correct chemical equation showing its reaction with water. hydrochloric acid hypochlorous acid chlorous acid chloric acid perchloric acid A. HClO2(aq) + H2O(l) ⇌ ClO2−(aq) + H3O+(aq) B. HCl(aq) + H2O(l) ⇌ Cl−(aq) + H3O+(aq) C. HClO2(aq) + H2O(l) → ClO2−(aq) + H3O+(aq) D. HClO3(aq) + H2O(l) ⇌ ClO3−(aq) + H3O+(aq) E. HClO(aq) + H2O(l) → ClO−(aq) + H3O+(aq) F. HClO(aq) + H2O(l) ⇌ ClO−(aq) + H3O+(aq) G. HClO4(aq) + H2O(l) → ClO4−(aq) + H3O+(aq) H. HClO3(aq) + H2O(l) → ClO3−(aq) + H3O+(aq) I. HClO4(aq) + H2O(l) ⇌ ClO4−(aq) + H3O+(aq) J. HCl(aq) + H2O(l) → Cl−(aq) + H3O+(aq)
For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. reaction HCl(aq) + H₂O(1) → CI¯ (aq) + H₂O* (aq) NH (aq) + H,O →+ NH,(aq) + HạO (aq) Cl(aq) + H₂O(1) → HCl(aq) + OH (aq) NH3(aq) + H₂O(1)→ NH(aq) + OH(aq) highlighted reactant Bronsted-Lowry Bronsted-Lowry neither acid base O O O
What is the general equation given when examining a titration? O A (aq) + H20 (1) = HA + OH (aq) (aq) H*e (aq) + ОН (aq) + OH' = H2O (1) О НА (aq) + H20 () =A (aq) + H3O*(aq) O HA (ag) + NaOH (ag) = NaA (aq) + H2O (1)
Write the equilibrium constant expression for this reaction: H,CO3(aq) 2H (aq)+CO (aq) →
For the reaction below, Kc = 1.10 × 10⁻⁸. What is the equilibrium concentration of OH⁻ if the reaction begins with 0.610 M HONH₂? HONH₂ (aq) + H₂O (l) ⇌ HONH₃⁺ (aq) + OH⁻ (aq)
Coral structures found in the Great Barrier Reef are composed of calcium carbonate, CaCO3, and are under threat of dissolution due to ocean acidification. Consider the following equilibrium reaction equation. CaCO3(s) + CO2(aq) + H2O(l) ⇌ Ca2+(aq) + 2HCO3–(aq) Write the expression for the equilibrium constant, Kc for this reaction. Predict whether the pH of the ocean will increase or decrease as a result of a decrease in the partial pressure of carbon dioxide in the atmosphere (circle your answer). Calculate the molar solubility (s) of calcium carbonate in water at 25 °C when Ksp = 4.5 ´ 10–9.
Part A Water ionizes by the equation =H+(aq) + OH (ag) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H*] and [OH ]: What is the H† concentration for an aqueous solution with pOH = 2.73 at 25 °C? Express your answer to two significant figures and include the appropriate units. Kw = [H*][OH¯] • View Available Hint(s) Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature. ? [H*] = Value Units
Consider the reaction below. Co(H,O),* (aq) + 4 Cl¯ (aq) = COC1," (aq) + 6 H,O (1I) The equilibrium constant expression (K) of the reaction does not include the concentration of H,O even though the reaction produces six moles of water. Explain.
Which of the following is a complete balanced reaction for an Arrhenius base in water? NaOH (s) 2 NaH (s) + O2 (g) →> ○ Mg(OH) 2 (s) → Mg2+ (aq) + OH (aq) ○ HNO2 (aq) → H+ (aq) + NO₂ (aq) KOH (s) →> K+ (aq) + OH¯ (aq)
A 0.043 M solution of an unknown acid, HA, has a pH of 2.56. What is the hydrogen ion concentration? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex: 4.5 x 105 = 4.5E5) HA(aq) + H" (aq) + A (aq) Answer:
What is the pH of 0.1510 M selenious acid solution, H2SeO3? H2SeO3(aq) + H2O(l) → HSeO3−(aq) + H3O+(aq) Ka1 = 3.5000e-2 HSeO3−(aq) + H2O(l) → SeO32−(aq) + H3O+(aq) Ka2 = 5.0000e-8