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All Textbook Solutions for Chemistry: Matter and Change
Use the symbols ,, and = to express the relationship between the concentrations of H+ ions and OH ions in acidic, neutral, and basic solutions.Explain how the definition of a Lewis acid differs from the definition of a Bronsted-Lowry acid.64AExplain the difference between a strong acid and a weak acid.Explain why equilibrium arrows are used in the ionization equations for some acids.Which of the beakers shown in Figure 18.29 might contain a solution of 0.1M hypochlorous acid? Explain your answer.How would you compare the strengths of two weak acids experimentally? By looking up information in a table or a handbook?Identify the conjugate acid-base pairs in the reaction of H3PO4 with water.70A71A72A73A74AWhat is the relationship between the pOH and the OH ion concentration of a solution?Solution A has a pH of 2.0. Solution B has a pH of 5.0 Which solution is more acidic? Based on the H+ ion concentrations in the two solutions, how many times more acidic?\If the concentration of H+ ions in an aqueous solution decreases, what must happen to the concentration of OH ions? Why?Use Le Chátelier's principle to explain what happens to the equilibrium H2O(l)H+(aq)+OH(aq) when a few drops of HCl are added to pure water.Common Acids and Bases Use the data in Table 18.8 to answer the following questions. Which substance is the most basic? Which substance is closest to neutral? Which has a concentration of H+=4.01010M ? Which has a pOH of 11.0? How many times more basic is antacid than blood?80A81A82A83A84AWhat acid and base must react to produce an aqueous sodium iodide solution?What acid-base indicators, shown in Figure 18.24 would be suitable for the neutralization reaction whose titration curve is shown in Figure 18.30?Why?When might a pH meter be better than an indicator to determine the end point of an acid-base titration?sWhat happens when an acid is added to a solution containing the HF/F buffer system?When methyl red is added to an aqueous solution, a pink color results. When methyl orange is added to the same solution, a yellow color is produced. What is the approximate pH range of the solution? Use Figure 18.24Give the name and formula of the acid and the base from which each salt was formed NaCl KHCO3 NH4NO2 Cas91A92AIn an acid-base titration, 45.78 mL of a sulfuric acid solution is titrated to the end point by 74.30mL of 0.4388M sodium hydroxide solution. What is the molarity of the H2SO4 solution?94A95A96A97A98A99A100A101A102A103A104A105A106A107A108A109A110A111A112A113A114A115A116A117A118A119A120A121A122A123A124A125A1STP2STP3STP4STP5STP6STP7STP8STP9STP10STP11STP12STP13STP14STP15STP16STP17STP18STP1PP2PP3PP4PP5SSC6SSC7SSC8SSC9SSC10SSC11SSC12PP13PP14PP15PP16PP17SSC18SSC19SSC20SSC21SSC22PP23PP24PP25PP26PP27PP28PP29PP30PP31PP32PP33PP34PP35SSC36SSC37SSC38SSC39SSC40SSC41SSC42SSC43SSC44PP45PP46PP47PP48PP49SSC50SSC51SSC52SSC53SSC54SSC33A34A35A36A37A38A39A40A41A42A43A44A45A46A47A48A49A50A51A52A53A54A55A56A57A58A59A60A61A62A63A64A65A66A67A68A69A70A71A72A73A74A75A76A77A78A79A80A81A82A83A84A85A86A87A88A89A90A91A92A93A94A95A96A1STP2STP3STP4STP5STP6STP7STP8STP9STP10STP11STP12STP13STP14STP15STP16STP17STP18STP1PP2PP3PP4PP5PP6PP7PP8PP9SSC10SSC11SSC12SSC13SSC14SSC15PP16PP17PP18PP19PP20PP21PP22PP23PP24PP25PP26SSC27SSC28SSC29SSC30SSC31SSC32SSC30A31A32A33A34A35A36A37A38A39A40A41A42A43A44A45A46A47A48A49A50A51A52A53A54A55A56A57A58A59A60A61A62A63A64A65A66A67A68A69A70A71A72A73A74A75A76A77A78A79A