General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN: 9781305580343
Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher: Cengage Learning
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Textbook Question
Chapter 17, Problem 17.2QP
Explain why calcium sulfate is less soluble in sodium sulfate solution than in pure water.
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Chapter 17 Solutions
General Chemistry - Standalone book (MindTap Course List)
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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- A 0.250-M sodium sulfate solution is added to a 0.200-M barium nitrate solution and 0.700 g barium sulfate precipitates. Write the balanced equation for this reaction. Calculate the minimum volume of barium nitrate solution that was used. Calculate the minimum volume of sodium sulfate needed to precipitate 0.700 g barium sulfate. Assume 100% yield.arrow_forward12.111 You have three white solids. What experiment could you carry out to rank them in order of increasing solubility?arrow_forward12.49 The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mg of solute/L of solution.)arrow_forward
- In Exercise 12.49, what is the allowed concentration of AgCl in g per 100 g of water? The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mgofsolute/L of solution.)arrow_forwardFigure 16.3 shows the solubility of AgNO3 in water inunits of moles of AgNO3 per kilogram of H2O. If 255 g of AgNO3 is added to 100 g of water at 95°C and cooledslowly, at what temperature will the solution becomesaturated?arrow_forward
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY