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Chapter 15 Solutions
Chemistry: An Atoms First Approach
- You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.arrow_forwardA solution contains Ca2+ and Pb2+ ions, both at a concentration of 0.010 M. You wish to separate the two ions from each other as completely as possible by precipitating one but not the other using aqueous Na2SO4 as the precipitating agent. (a) Which will precipitate first as sodium sulfate is added, CaSO4 or PbSO4? (b) What will be the concentration of the first ion that precipitates (Ca2+ or Pb2+) when the second, more soluble salt begins to precipitate?arrow_forwardA chemistry graduate student is given 450. mL of a 1.00M chlorous acid (HClO₂) solution. Chlorous acid is a weak acid -2 with K = 1.1 × 10 . What mass of NaClO₂ should the student dissolve in the HClO2 solution to turn it into a buffer with a pH = 1.52? You may assume that the volume of the solution doesn't change when the NaClO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. [] x10 Xarrow_forward
- 5 A chemistry graduate student is given 450. mL of a 0.10M ammonia (NH3) solution. Ammonia is a weak base with K, = 1.8 × 10. What mass of NH4Cl should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.11? You may assume that the volume of the solution doesn't change when the NH4Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ☐ ☐ x10arrow_forwardFor the titration of an aqueous nitrous acid solution, HNO,(aq), with an aqueous strontium hydroxide solution, Sr(OH)2{aq), what do you expect the pH of the solution to be at the equivalence point? O Basic (pH > 7.00) O Unable to determine the pH of the solution at the equivalence point without additional information O Acidic (pH < 7.00) O Neutral (pH = 7.00)arrow_forwardAn aqueous solution contains 0.28 M hydrofluoric acid. One Liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) O 0.139 mol NaOH 0.28 mol NaNO, 0.14 mol HNO, 0.29 mol HNO3 O 0.29 mol NaFarrow_forward
- A chemistry graduate student is given 100. mL of a 0.90M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 10 What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.97? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.arrow_forwardA solution is formed by adding 3.20 grams of solid sodium hypochlorite, NaClO, to 500.0 ml of 0.0750M calcium hypochlorite, Ca(ClO)₂. Calculate the pH of the resulting solution. You may assume that the sodium hypochlorite dissolve completely and that the change in volume is negligible with the addition of the solid.arrow_forwardWhen some sodium hydroxide is gradually added to a solution of lead nitrate Pb(NO3)2 at 0.01 mol.L-¹, lead hydroxide Pb(OH)2 starts to precipitate at pH of 7.5; Calculate the solubility product of Pb(OH)2. What is the solubility of lead hydroxide in water? What would be the concentration of Pb²+ if the pH of the initial solution was fixed to 9? The answer : 1) Ks 10-¹5 ;2) 6.3×10-6 mol.L-¹; 3) [Pb²+] = 10–5 mol.L-¹arrow_forward
- The solubility product for calcium phosphate is Ksp= 1.3 × 10–26. What is the molar solubility of calcium phosphate?arrow_forwardThe solubility of an ionic compound in water can be expressed in terms of the mass that will dissolve in a given volume of water, or in terms of the solubility product, Ksp. If only 0.303 g of Ca(OH)2 dissolves in enough water to give 0.243 L of aqueous solution at a given temperature, what is the Ksp value for calcium hydroxide at this temperature?arrow_forwardThe solubility of an ionic compound in water can be expressed in terms of the mass that will dissolve in a given volume of water, or in terms of the solubility product, Ksp.If only 0.264 g of Ca(OH)2 dissolves in enough water to give 0.165 L of aqueous solution at a given temperature, what is the Ksp value for calcium hydroxide at this temperature?arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning