B. What is the major anionic (negatively charged) species present at equilibrium in solutions made up of the following species: example: NH3 + HCl (gas) 1. OH + CH₂CO₂H (in water) 2. CH3O+ 3. CHO + 4. CH3O+ H₂C CH3 H₂C (in water) 6. NaH (in water) OH CH3 (in water) (in water) 5. CHO + CH3NO₂ (in water) Cr

B. What is the major anionic (negatively charged) species present at equilibrium in solutions made up of the following species: example: NH3 + HCl (gas) 1. OH + CH₂CO₂H (in water) 2. CH3O+ 3. CHO + 4. CH3O+ H₂C CH3 H₂C (in water) 6. NaH (in water) OH CH3 (in water) (in water) 5. CHO + CH3NO₂ (in water) Cr

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 95SCQ: Most naturally occurring acids are weak acids. Lactic acid is one example....

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Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
1. Nitrogen in an industrial wastewater is primarily in the form of ammonia (NH3) and ammonium (NH4+) ions. The acid/base equilibrium reaction for ammonia and ammonium is given as: NH4+ → H+ + NH3 Ką = 10-9.26 The total nitrogen concentration in wastewater is given as 2 x 10-3 moles/L (or 28 mg N/L), a. Calculate the concentration of ammonia (NH3) and ammonium (NH4*) ions at pH 10. NH3: moles/L NH4*: moles/L Check b. In ammonia stripping, nitrogen is removed from wastewater by volatilization of NH3. Would ammonia stripping be more effective above or below pH 9? Briefly explain your reasoning.
Which of the following is TRUE about the RbCl salt? I. RbCl ions do not participate in hydrolysis with water. II. RbCl are derived from weak base and weak acid respectively. III. RbCl has a value of Ka = Kb. IV. RbCl solution is acidic. Consider the reaction: 2 SO2 (g) + O2(g) ⇄ 2 SO3(g); ΔHo = -198.2 kJ/mole Predict the shift of the chemical reaction in the given system if the pressure of the gas system was increased. The equilibrium shifts in the forward direction. The equilibrium shifts in the reverse direction. Equilibrium is not changed or affected.
In the reaction NH4*(aq) + H₂O(l) → NH3(aq) + H₂O*(aq) the conjugate acid-base pairs are... O A. NH4*/H₂O and NH3/H3O* O B. NH4*/NH3 and H3O*/H₂O O C. NH4+/H3O* and H₂O/NH3 OD. NHÀ/H2O
3. The sour taste of lemons is attributed to citric acid. The dissociation of citric acid in water occurs in three steps. H&CO, 5 H*+ H;C,O, Kal= 7.4x104 H-CO, 5 H* + H,C,O,2- K= 1.7x10-5 H,C.O2- H* + H;C,O, K= 4.0x10-7 HO HO OH OH %3D Draw the ladder diagram for citric acid. nnt terthook section: 7.10
What is the concentration of each ion in each of the following solutions? (assume complete dissociation)a. a 0.550 M water solution of K2CO3b. a 0.345 M water solution of HClO4
Which of the following salts produces a neutral solution when dissolved in water? a. NaClO 4 b. KF c. All of these salts produce a neutral solution when dissolved in water. d. Mg(NO 2 ) 2 e. CaCO 3
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3. What is the pH of a 0.0075 mol L·' HCl solution? What is [OH]in this solution? 4. Each of the following salts were dissolved in water to give a 0.10 mol.L·' solution. Rank the solutions from lowest to highest pH. Their respective pKb values are indicated in brackets. Na2S (-5), Na3PO4 (1.68), NaF (10.86), NaCH3CO0 (9.26), AIC13
3. Quinine, C2H2,N2O2(aq), is responsible for saving thousands of lives during the construction of the Panama Canal. Quinine is a weak base. a) Write the products for the reaction below AND write the equilibrium constant expression for the reaction. C20H2,N,O2(aq) + H,O(1) K, =. b) Given the value of K, for the above reaction is 8.1 x 10°, a saturated solution of quinine has a pH of 10.04. Determine the mass of quinine that would be dissolved in a 150 mL saturated solution of quinine.
8. Calculate the equilibrium concentration of each aqueous species (H2A, HA– A2–, H3O+, and OH–) in the solution. Assume a temperature of 25°C. H2A: pKa1 = 2.05 and pKa2 = 6.22a. 0.10 M H2A b. 0.10 M Na2A
Calculate the concentrations of all species in a 0.940 M Na, SO, (sodium sulfite) solution. The ionization constants for sulfurous acid are Kal = 1.4 × 10-2 and K42 = 6.3 × 10–8. [Na*] = 1.88 [so}] = 0.94 M M [HSO;] = 3.8 x10 -4 1.65 x10-8 M [H,SO,] M Incorrect [OH] = 3.8 x10¬4 [H*] = 2.6 x10-11 M M