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- 6. Find Ka and Kb of each of the following amphiprotic anions and determine if they act as an acid or a base in water solution. а) НРО- Ka = (С.А. 3D Kb = A or B b) HC,H;0, Ka = (C. A. = ) Kb = A or B c) HSO; Ka = : (C. A. = Kb = A or B15. An aqueous solution of HBr would contain which of the following? Br 1- and H3O+ HBr and H3O+ HBr, Br 1-, and H3O+ HBr, Br 1-, and OH–1. The following equilibrium exists when ammonium is dissolved in water: NH4+ (aq) + H2O (l) « H3O+ (aq) + NH3 (aq) The Ka of NH4 is 5.6 x 10-10. Find the pH of a 3.00 M solution of NH4Cl. (hint: since NH4Cl completely ionizes, the concentration of the ammonium ion is 3.00 M) NH4Cl (s)àNH4+ (aq) + Cl- (aq)
- Calculate the pH at 25 °C of a 0.85M solution of ethylammonium bromide (C,H,NH,Br). Note that ethylamine (C,H,NH,) is a weak base with a pK, of 3.19. Round your answer to 1 decimal place. pH = [| Eglanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibilt 12 MacBook AirFormic acid dissociates reversibly according to the following equation. [ /20] HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.ACTIVITY 2: “What's my Product" Direction: Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. I. 1. HC2H3O2 + CsH;N – 2. HSO4- + PO43- - 3. HC103 + (C2H5);N → 4. NH3 + C6H5O- → 5. CSH5NH* + C2042-
- 8. Which of the following equations shows that isoquinoline, C9H7N, behaves as a Brønsted-Lowry base in water?A. C9H7N(aq) + OH-(l) C9H6N-(aq) + H2O(aq)B. C9H7N(aq) + H2O(l) C9H6N-(aq) + H3O+(aq)C. C9H7N(aq) + H3O+(aq) C9H7NH+(aq) + H2O(l) D. C9H7NH+(aq) + OH-(aq) C9H7N(aq) + H2O(l)E. C9H7NH+(aq) + H2O(l) C9H7N(aq) + H3O+(aq)What is the equilibrium-constant expression of the basic dissociation of NaNO2? Kb = ([HNO2] [NO2])/[OH-] %3D Kb = ([NO2] [OH-])/[HNO2] %3D Kb = ([HNO2] [OH-])/[NO2] Kb = [OH-J/([HN02] [NO2])4. Calculate the pH you would expect for a 0.15 M aqueous solution of each substance. - nitric acid - ascorbic acid - lithium hydroxide - methylamine (see Table 15.4, p. 682) I 5. Consider your work on the ascorbic acid solution in the previous problem. What would the equilibrium concentration of the conjugate (ascorbate, C,H;O6) be in the solution?
- Yeni... O Ara Posta Gonderileri Gözden Geçir Görünüm Yardim 4- Write equations for the acid base reactions that would occur (if any) if ethanol were added to solutions of each of the following compounds In each reaction, label the stronger acid, the stronger base, and so forth.(Please consult the table given below) Ya) NaNH (c) (d) NaOH EGO 16 A 12 IA 17 & 5 8 KFor each of the following aqueous reactions, identify the acid, the base, the conjugate base, and the conjugate acid. а. Al(H2 O)63+ + H2O H30+ + Al(H2O)5 (OH)²+ b. + HONH3 HONH2 + H2O H3O+ + с. НОСI + C6H;NH2 — OCi- C6 H5 NH3+ +Identify the Lewis acid and the Lewis base in each the following reactions. (Omit states of matter.) а. В (ОН),(aq) + H,0() — в(он). (аq) + н (aд) Acid: Base: b. НаО() + CN (ад) — HCN(aq) + он (ад) Acid: Base: Hgl, (8) + 21 (aq) → HgI, ² (ag) с. Acid: Base: