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OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
11th Edition
ISBN: 9781305673939
Author: Darrell Ebbing; Steven D. Gammon
Publisher: Cengage Learning US
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Chapter 17, Problem 17.70QP
Describe how you could separate the following mixture of metal ions: Na+, Hg2+, and Ca2+.
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To simulate the pH of blood, which is 7.4, an undergraduate researcher in a biology lab produced a buffer solution by dissolving sodium dihydrogen phosphate (NaH2PO4, Ka = 6.2 × 10–8) and sodium hydrogen phosphate (Na2HPO4) together in an aqueous solution. What mole ratio of Na2HPO4/NaH2PO4 did she need to use?
You prepare a standard NaOH solution for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC₆H₇O₆, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 17.54 mL of the NaOH to titrate (react exactly with) the ascorbic acid found in one 500.0 mg tablet. What is the percent vitamin C by mass in the tablet?
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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.
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☐ x10
Chapter 17 Solutions
OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
Ch. 17.1 - Give solubility product expressions for the...Ch. 17.1 - Silver ion may be recovered from used photographic...Ch. 17.1 - Lead(II) arsenate, Pb3(AsO4)2, has been used as an...Ch. 17.1 - Prob. 17.4ECh. 17.1 - Prob. 17.1CCCh. 17.2 - a. Calculate the molar solubility of barium...Ch. 17.2 - Suppose you have equal volumes of saturated...Ch. 17.2 - Prob. 17.3CCCh. 17.3 - Anhydrite is a mineral composed of CaSO4 (calcium...Ch. 17.3 - A solution of 0.00016 M lead(II) nitrate,...
Ch. 17.4 - Which salt would have its solubility more affected...Ch. 17.4 - If you add a dilute acidic solution to a mixture...Ch. 17.5 - What is the concentration of Cu2+(aq) in a...Ch. 17.6 - Will silver iodide precipitate from a solution...Ch. 17.6 - What is the molar solubility of AgBr in 1.0 M...Ch. 17 - Suppose the molar solubility of nickel hydroxide....Ch. 17 - Explain why calcium sulfate is less soluble in...Ch. 17 - What must be the concentration of silver ion in a...Ch. 17 - Prob. 17.4QPCh. 17 - Explain why barium fluoride dissolves in dilute...Ch. 17 - Prob. 17.6QPCh. 17 - Prob. 17.7QPCh. 17 - Prob. 17.8QPCh. 17 - Prob. 17.9QPCh. 17 - Prob. 17.10QPCh. 17 - Prob. 17.11QPCh. 17 - Write the solubility product expression for the...Ch. 17 - What is the molar solubility of calcium oxalate,...Ch. 17 - Prob. 17.14QPCh. 17 - Solubility and Solubility Product You put 0.10-mol...Ch. 17 - Solubility Equilibria Consider three hypothetical...Ch. 17 - Which compound in each of the following pairs of...Ch. 17 - Prob. 17.18QPCh. 17 - You are given a saturated solution of lead(II)...Ch. 17 - Which of the following pictures best represents a...Ch. 17 - Which of the following pictures best represents an...Ch. 17 - Prob. 17.22QPCh. 17 - Prob. 17.23QPCh. 17 - Prob. 17.24QPCh. 17 - Use the solubility rules (Table 4.1) to decide...Ch. 17 - Use the solubility rules (Table 4.1) to decide...Ch. 17 - Write solubility product expressions for the...Ch. 17 - Write solubility product expressions for the...Ch. 17 - Prob. 17.29QPCh. 17 - The solubility of magnesium oxalate, MgC2O4, in...Ch. 17 - The solubility of cobalt(II) iodate in water is...Ch. 17 - Prob. 17.32QPCh. 17 - The pH of a saturated solution of copper(II)...Ch. 17 - A solution saturated in calcium hydroxide...Ch. 17 - Strontianite (strontium carbonate) is an important...Ch. 17 - Magnesite (magnesium carbonate, MgCO3) is a common...Ch. 17 - What is the solubility of PbF2 in water? The Ksp...Ch. 17 - What is the solubility of strontium iodate,...Ch. 17 - What is the solubility (in grams per liter) of...Ch. 17 - What is the solubility (in grams per liter) of...Ch. 17 - The solubility of magnesium fluoride, MgF2, in...Ch. 17 - The solubility of silver sulfate, Ag2SO4, in water...Ch. 17 - What is the solubility (in grams per liter) of...Ch. 17 - Calculate the molar solubility of strontium...Ch. 17 - From each of the following ion concentrations in a...Ch. 17 - From each of the following ion concentrations in a...Ch. 17 - Lead(II) chromate, PbCrO4, was used as a yellow...Ch. 17 - Lead sulfate PbSO4, was used as a white paint...Ch. 17 - The following solutions are mixed: 1.0 L of...Ch. 17 - A 45-mL sample of 0.015 M calcium chloride, CaCl2,...Ch. 17 - A 45.0-mL sample of 0.0015 M BaCl2 was added to a...Ch. 17 - A 65.0-mL sample of 0.010 M Pb(NO3)2 was added to...Ch. 17 - How many moles of calcium chloride, CaCl2, can be...Ch. 17 - Magnesium sulfate, MgSO4, is added to 456 mL of...Ch. 17 - What is the I concentration just as AgCl begins to...Ch. 17 - What is the Cl concentration just as Ag2CrO4...Ch. 17 - Write the net ionic equation in which the slightly...Ch. 17 - Write the net ionic equation in which the slightly...Ch. 17 - Which salt would you expect to dissolve more...Ch. 17 - Which salt would you expect to dissolve more...Ch. 17 - Write the chemical equation for the formation of...Ch. 17 - Write the chemical equation for the formation of...Ch. 17 - Sufficient sodium cyanide, NaCN, was added to...Ch. 17 - The formation constant Kf for the complex ion...Ch. 17 - Prob. 17.65QPCh. 17 - Predict whether nickel(II) hydroxide, Ni(OH)2,...Ch. 17 - What is the molar solubility of CdC2O4 in 0.10 M...Ch. 17 - What is the molar solubility of ZnS in 0.10 M NH3?Ch. 17 - Prob. 17.69QPCh. 17 - Describe how you could separate the following...Ch. 17 - A student dissolved a compound in water and added...Ch. 17 - A student was asked to identify a compound. In an...Ch. 17 - Prob. 17.73QPCh. 17 - Prob. 17.74QPCh. 17 - Prob. 17.75QPCh. 17 - Prob. 17.76QPCh. 17 - For cerium(III) hydroxide, Ce(OH)3, Ksp equals 2.0...Ch. 17 - Copper(II) ferrocyanide, Cu2Fe(CN)6, dissolves to...Ch. 17 - What is the solubility of magnesium hydroxide in a...Ch. 17 - What is the solubility of silver oxide, Ag2O, in a...Ch. 17 - What is the molar solubility of Mg(OH)2 in a...Ch. 17 - What is the molar solubility of Al(OH)3 in a...Ch. 17 - Prob. 17.83QPCh. 17 - What must be the concentration of chromate ion in...Ch. 17 - A 3.20-L solution of 1.25 103 M Pb(NO3)2 is mixed...Ch. 17 - Prob. 17.86QPCh. 17 - How many grams of sodium chloride can be added to...Ch. 17 - Prob. 17.88QPCh. 17 - Prob. 17.89QPCh. 17 - Prob. 17.90QPCh. 17 - Calculate the molar solubility of silver bromide,...Ch. 17 - Prob. 17.92QPCh. 17 - The solubility of zinc oxalate, ZnC2O4, in 0.0150...Ch. 17 - The solubility of cadmium oxalate. CdC2O4, in...Ch. 17 - Prob. 17.95QPCh. 17 - Prob. 17.96QPCh. 17 - A saturated solution of copper(II) iodate in pure...Ch. 17 - A saturated solution of lead iodate in pure water...Ch. 17 - A solution contains 0.0150 M lead(II) ion. A...Ch. 17 - A solution contains 0.00740 M calcium ion. A...Ch. 17 - a If the molar solubility of cobalt(II) hydroxide...Ch. 17 - a If the molar solubility of beryllium(II)...Ch. 17 - Although silver chloride is insoluble in water, it...Ch. 17 - Crystals of AgBr can be removed from...Ch. 17 - A 1.0-L solution that is 4.2 M in ammonia is mixed...Ch. 17 - Prob. 17.106QPCh. 17 - Prob. 17.107QPCh. 17 - Prob. 17.108QPCh. 17 - Prob. 17.109QPCh. 17 - A chemist mixes 1.00 L each of 0.100 M Na2CO3 and...Ch. 17 - Prob. 17.111QPCh. 17 - Prob. 17.112QPCh. 17 - An analytical chemist has a solution containing...Ch. 17 - How would the solubility of calcium fluoride be...Ch. 17 - A scientist was interested in how soluble rust is...Ch. 17 - Prob. 17.116QPCh. 17 - Prob. 17.117QPCh. 17 - Prob. 17.118QPCh. 17 - Prob. 17.119QPCh. 17 - Suppose you add 35.6 mL of 0.578 M H2SO4 to 55.6...Ch. 17 - Prob. 17.121QPCh. 17 - Prob. 17.122QPCh. 17 - Prob. 17.123QPCh. 17 - Suppose you have a water solution that is 0.0010 M...Ch. 17 - Prob. 17.125QPCh. 17 - Suppose that an aqueous solution is in equilibrium...Ch. 17 - Prob. 17.127QPCh. 17 - The text describes zinc hydroxide as an amphoteric...Ch. 17 - A solution is 1.5 104 M Zn2 and 0.20 M HSO4. The...Ch. 17 - Prob. 17.130QPCh. 17 - What is the solubility of calcium fluoride in a...Ch. 17 - What is the solubility of magnesium fluoride in a...Ch. 17 - Prob. 17.133QPCh. 17 - Prob. 17.134QP
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