6. Draw two graphs for weak acid HA: (a) percent dissociation for HA versus the initial concentration of HA ([HA]o) (hint: assume [HA], as x and [H+]/[HA], as y). (b) the equilibrium concentration of H+ versus [HA]o. Explain both.

6. Draw two graphs for weak acid HA: (a) percent dissociation for HA versus the initial concentration of HA ([HA]o) (hint: assume [HA], as x and [H+]/[HA], as y). (b) the equilibrium concentration of H+ versus [HA]o. Explain both.

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 8RQ: For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in...

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(a) Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) calculate the Kb values for the CHCOO- and ClO- .
Consider the following acidic equilibrium: H₂CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + H₃O⁺(aq). If you add NaHCO₃ to this solution, which of the following will occur? A) The reaction quotient will decrease. B) The reaction will shift in the reverse direction. C) The equilibrium constant will increase. D) No changes to the equilibrium positions will take place.
Answer the following questions about acid-base equilibrium reactions. (a)Which is a stronger acid HX or HY in the reaction below? HX + Y –→X –+ HYK eq= 2.43 x 10 –3 (b)What is the difference between a strong acid and a weak acid in terms of equilibrium position? (c)If the Kaof H2CO3is 4.3 x 10 –7and the Kaof HF is 6.8 x 10 –4, then is the reaction below reactant favored or product favored?H2CO3+ F –→HCO3–+ HF
(b) What will happen if acetic acid (HC2H3O2) is added to water? O An equilibrium will form between its molecular form, HC2H3O2, and the species formed by removal of water, C2H2O. O An equilibrium will form between its molecular form, HC2H3O2, and the species formed by addition of water, H3C2H3O3. O Acetic acid is a strong acid and will ionize completely. O An equilibrium will form between its molecular form, HC2H3O2, and the ionized form, H* and C2H3O2. O Acetic acid is a weak acid and will not ionize completely. Hint Attempts: 1 of 15 used Submit Save for Later TIng I aI system, SOme of UIS energy Can De transieIICU To une su t ST國 ост 15 MacBook Air
For the following reaction, K< 1. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. C18H21O3N + C,H;OH=C,H;0" + C18H21O3NH* Clear All C18H2103NH* Stronger Bronsted-Lowry acid Weaker Bronsted-Lowry C,H;O¯ acid C18H21O3N Stronger Bronsted-Lowry base Weaker Bronsted-Lowry C,H;OH base
30. In the reaction HCl(aq) + H₂O(l) ⇒Cl¯(aq)+ H3O+ (aq) does water act as a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither, or both? (A) Neither as an acid nor as a base; water is neutral (B) Both an acid and a base. (C) An acid (D) A base (E) Depends temperature
H. | || The percent ionization of chloroacetic acid is less than that of fluoroacetic acid. :*-C-C-ö-H The percent ionizations cannot be compared without knowing the concentrations of the two acids. The structure of haloacetic acids, XCH,COOH (where X is The percent ionizations cannot be compared without knowing the pH of the solution. either F, Cl, Br, or 1), is shown above. The dissociation constants and molar masses of four haloacetic acids are listed in the table below. The percent ionization of chloroacetic acid is greater than that of fluoroacetic acid. Acid pK. K. Molar Mass(g/mol) CLEAR ALL Fluoroacetic acid 2.59 2.57 x 10–3 78.0 Chloroacetic acid 2.87 1.35 x 10–3 94.5 Bromoacetic acid 2.90 1.26 x 10-3 138.9 lodoacetic acid 3.18 6.61 × 10-4 185.9 An aqueous solution contains small but equal concentrations of both chloroacetic and fluoroacetic acids. Which statement comparing the percent ionizations of the two acids in the solution is true? エーO-
From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb for each of the weak bases.(a) CH3CO2H: [H3 O+] = 1.34 × 10−3 M;[CH3 CO2−] = 1.34 × 10−3 M;[CH3CO2H] = 9.866 × 10−2 M;(b) ClO−: [OH−] = 4.0 × 10−4 M;[HClO] = 2.38 × 10−5 M;[ClO−] = 0.273 M;(c) HCO2H: [HCO2H] = 0.524 M;[H3 O+] = 9.8 × 10−3 M;[HCO2−] = 9.8 × 10−3 M;(d) C6 H5 NH3+ : [C6 H5 NH3+] = 0.233 M;[C6H5NH2] = 2.3 × 10−3 M;[H3 O+] = 2.3 × 10−3 M
A solution is made by dissolving 44.1 g of Ba(NO₂)₂ in 500.0 mL of water. (a) Does Ba²⁺ have any acidic or basic properties? (b) Does NO₂⁻ have any acidic or basic properties? (c) As NO₂⁻ is a base, write the basic equilibrium equation that exists in solution (d) What is the value of Kb for NO₂⁻? The Ka of HNO₂ is 4.5 × 10⁻⁴. (e) Determine the pH of the solution
Can you provide an example and explanation?
2. Answer the questions for the acid below: a) Write the acid dissociation constant, Ka, expression for the reaction: b) If [A] = 0.030 M, [H3O+] = 0.010 M, and [HA] = 0.5 M, what is the value of Ka? c) If another acid, HB, has a Ka value of 1.0 x 10-10, which acid is stronger? HA or HB? Why? HA(aq) + H₂O(1)→ H30+ (aq) + A¯ (aq)
Sodium hypochlorite solution is also known as bleach. It contains the hypochlorite ion ClO-. (a) Write an equation for the reaction between hypochlorite ion and ammonium ion. Label the acids and bases in the forward and reverse reactions. Identify the two conjugate acid-base pairs. (b) This equilibrium favors the reactants. Which of the acids is stronger and donates protons more readily?