Calculate the pH of a saturated solution of Mg(OH)2. Ksp [Mg(OH)2] = 1.8 × 10-¹1.Express your answer to two decimal places.View Available Hint(s)pH =SubmitIVE ΑΣΦ?

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Answered: Calculate the pH of a saturated…

Calculate the pH of a saturated solution of Mg(OH)2. Ksp [Mg(OH)2] = 1.8 x 10-¹1. Express your answer to two decimal places. View Available Hint(s) pH = Submit [5] ΑΣΦ ?

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter8: Acids And Bases

Section: Chapter Questions

Problem 8.44P: 8-44 What is the molarity of a solution made by dissolving 3.4 g of Ba(OH)2 in enough water to make...

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For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
8-44 What is the molarity of a solution made by dissolving 3.4 g of Ba(OH)2 in enough water to make 450 mL of solution? Assume that Ba(OH)2 ionizes completely in water to Ba2+ and OH- ions. What is the pH of the solution?
Please answer these questions on your Page 8 (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 7.7 x 10-¹2. What is the pH of a 0.011 M solution of A-(aq)? The temperature is 25°C. (b) For the reaction A(g) A(1), the equilibrium constant is 0.666 at 25.0°C and 0.111 at 75.0°C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?
8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? 9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)
3. H̟CO, 2Ħ+HCO,¯ K, = 4.3 × 10-7 HCO, H* + Co, K, = 5.6 × 10-" The acid dissociation constants for the reactions above are given at 25°C. (a) What is the pH of a 0.050-molar solution of H,CO, at 25°C? (b) What is the concentration of CO,- ions in the solution in (a)? (c) How would the addition of each of the following substances affect the pH of the solution in (a)? (i) HCl (ii) NaHCO, (iii) NaOH (iv) NaCl
Like any equilibrium constant, Kw changes with temperature. (a) Given that autoionization is endothermic, how does Kw change with rising T ? Explain with a reaction that includes heat as reactant or product. (b) In many medical applications, the value of Kw at 37°C (body temperature) may be more appropriate than the value at 25°C, 1.0 x 10-14. The pH of pure water at 37°C is 6.80. Calculate Kw, pOH, and [OH-] at this temperature.
5) Hydroxylamine, HONH2, readily forms salts such as hydroxylamine hydrochloride which are used as antioxidants in soaps. Hydroxylamine has K₁ of 9.1 x 10-2. What is the pH of a 0.025 HONH3 tags MHONH₂ solution? A) 2.90 но HỌ = (af) RI 1.92 x = 1.5 × 10 ³ = [OH-] x HONH2 0.025
Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.
COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…
(a) Calculate the percent ionization of a 0.20 M solution of monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10^-4. (b) The pH of gastric acid juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20 M. Calculate the percent ionization of the acid under these conditions.
(c) Calculate the pH of 0.5 mol/L sodium hydrogen carbonate, NaHCO3. The Ka,1 of carbonic acid, H₂CO3, is 4.3 x 10-7. Нансез END
For the diprotic weak acid H₁A, Kal = 3.2 × 10-6 and Ka2 = 6.3 × 10-9. What is the pH of a 0.0800 M solution of H,A? What are the equilibrium concentrations of H2A and A2 in this solution? Step 1: Make an equilibrium table for the molar concentrations at equilibrium after the first dissociation step. Concentration (M) H,A(aq) H+(aq) + HA (aq) initial 0.0800 0 0 change -I +x +x equilibrium Express Kal in terms of the initial concentration of H,A and x, and then show the simplified expression when x is assumed to be negligible compared to to the initial concentration. complete: Kal= = 3.89 Incorrect Determine the numerical value of x. x = 6.3 ×10 9 M simplified: Kal≈ 3.9 Incorrect