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- .
(i) What is the Arrhenius definition of an acid, give an example Why is NH3 considered a base according to Bronsted-Lowry theory?
Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO,H, pK = 5.0]. (a) Which acid has the larger K? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right? %3D The pKa values in Table 2.1 span a large range (-7 to 50). The pK, scale is logarithmic. small difference in pK, translates into a large numerical difference, For example, the diffe between the pK, of NH3 (38) and CH2=CH, (44) is six pKa units. This means that NH, is one million times more acidic than CH,=CH,.
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.
The pH scale for acidity is defined by pH log10 H* where H is the concentration of hydrogen ions measured in moles per liter (M). (A) The pH of egg whites is 8.3. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M (B) The pH of lemon juice is 2.0. Calculate the concentration of hydrogen ions in moles per liter (M). [H+] = M
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
3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.
3a) Write the hydrolysis reaction of a 0.050M solution of acetic acid. Clearly identify the acid, base, conjugate acid, and conjugate base in the reaction. b) is this acid a strong acid or weak acid? Why? c) calculate the [H3O+] for this reaction (hint: Use an ICEq box) d) calculate the pH of a 0.050M solution of this acid
Calculate the pH and the pOH of these solutions: (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH = pOH =
25) Consider 0.14 M monoprotic acid (HA) that is 12% ionized. (a) Show the reaction of dissociation (ionization) of HA (b) Calculate the [H+] in the solution. (c) Calculate the Ka of HA.
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-