You are given a 0.250 M NO21 solution. a. Write the balanced chemical reaction of NO21 with water, including phase labels and correct charges. b. Using an ICE table, calculate the pH of this weak base solution. The Kb of NO21 is 2.16 · 1011.
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- Consider the following data on some weak acids and weak bases: name K₂ formula HNO₂ 4.5 x 104 acetic acid HCH,CO₂ 1.8x105 acid nitrous acid solution 0.1 M HONHYBT 0.1 M KBr Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 0.1 M KCH₂CO₂ 0.1 M C₂H₂NHCI PH choose one choose one choose one base choose one K name formula hydroxylamine HONH₂ 1.1 x 107 pyridine CH₂N 1.7×10The following assertions apply to acid A and base B. • When acid A interacts with a strong base and base B reacts with a strong acid, neutral salts are generated.• The Ka of Acid A is greater than that of HClO2.• The pH of a 2.13 x 10–3 M solution of base B is 11.6. Which among the choices below is most likely? a. Acid A is HClO and base B is NaOH. b. Acid A is HBrO4 and base B is KOH. c. Acid A is HClO4 and base B is Ba(OH)2. d. Acid A is HBrO2 and base B is Sr(OH)2.1. A 0.0250 M Ca(X)₂ has a pH of 8.049. Ca(X)2 is composed of a Ca²+ cation and an unknown anion X, which undergoes hydrolysis. A. Write the balanced dissociation reaction of Ca(X)2 into its ions. Write your answer on your solution sheet B. Write the balanced hydrolysis reaction of the unknown anion, X. Write your answer on your solution sheet C. Calculate the K₁ or K, of X¹. D. Given the following K, values of different weak acids, determine the identity of X. Weak acids Ka HIO 2.00 x 10-11 HCN 6.17 x 10-10 CH3COOH 1.80 x 105 HNO 2 4.00 x 10-4 27
- 7. Write a Bronsted-Lowry acid-base equation for the reaction between each pair of species. Assume each species is aqueous. Show your workings. a.nitric acid and potassium hydroxide b.phosphoric acid and sodium bicarbonate c. ammonia and hydrofluoric acidThe pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = − log [H+] where [+] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 4.92 × 10-³ mol/L, the pH is b. If the pH of a solution is 3.078, the hydrogen ion concentration is mol/L.1. A 0.0250 M Ca(X)₂ has a pH of 8.049. Ca(X)₂ is composed of a Ca²+ cation and an unknown anion X, which undergoes hydrolysis. A. Write the balanced dissociation reaction of Ca(X)2 into its ions. Write your answer on your solution sheet B. Write the balanced hydrolysis reaction of the unknown anion, X. Write your answer on your solution sheet C. Calculate the K₁, or K, of X. D. Given the following K, values of different weak acids, determine the identity of X. Weak acids Ka HIO 2.00 x 10-11 HCN 6.17 x 10-10 CH₂COOH 1.80 x 105 HNO2 4.00 x 104
- 1. A 0.0250 M Ca(X)2 has a pH of 8.049. Ca(X)2 is composed of a Ca²+ cation and an unknown anion X, which undergoes hydrolysis. A. Write the balanced dissociation reaction of Ca(X)2 into its ions. Write your answer on your solution sheet B. Write the balanced hydrolysis reaction of the unknown anion, X. Write your answer on your solution sheet C. Calculate the K₁, or Kp of X. D. Given the following Ką values of different weak acids, determine the identity of X". Weak acids Ka HIO 2.00 x 10-11 HCN 6.17 x 10-10 CH3COOH 1.80 x 10-5 HNO₂ 4.00 x 10-4The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = - log[H*] where [H*] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 7.26 x 10 mol L, the pH is b. If the pH of a solution is 3.607, the hydrogen ion concentration is mol L.Calculate the pH of a 0.10 M solution of sodium hypochlorite (NaClO; Ka 2.90 x 10$). Also, calculate the pH after diluting the solution by 10 times.
- 5. A typical aspirin tablet contains 325mg of acetylsalicylic acid (HC9H704) which is a weak acid. The Ka of this acid is 3.69 x 10-4. a. Give the equation for dissociation of the weak acid HC9H7O4. b. What is the initial concentration, in units of molarity, of acetylsalicylic acid if 2 tablets are dissolved in 500. mL of water? c. What is the equilibrium concentration of all species of this solution of acetylsalicylic acid? d. What is the pH, pOH, and % ionization of this solution?4. Suppose you had a sample of Hydrobromic acid that had a molarity of 0.1 and you had 42 ml of it. If you added 20 ml of 0.15 M NaOH, what is the pH of the resulting solution? NaOH + HBr -> NaBr H2OThe pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H¹] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.171, the hydrogen ion concentration is mol/L.