Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 15, Problem 37QAP
Interpretation Introduction
Interpretation:
The precipitate formed needs to be determined, if a solution is made up by mixing
Concept introduction:
To precipitate
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Chemistry: Principles and Reactions
Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Calculate K for the reactions in Question 1.Ch. 15 - Calculate K for the reactions in Question 2.Ch. 15 - Calculate K for the reactions in Question 3.Ch. 15 - Calculate K for the reactions in Question 4.Ch. 15 - Calculate [H+] and pH in a solution in which...Ch. 15 - Calculate [OH-] and pH in a solution in which the...
Ch. 15 - A buffer is prepared by dissolving 0.0250 mol of...Ch. 15 - Prob. 12QAPCh. 15 - A buffer solution is prepared by adding 15.00 g of...Ch. 15 - A buffer solution is prepared by adding 5.50 g of...Ch. 15 - A solution with a pH of 9.22 is prepared by adding...Ch. 15 - An aqueous solution of 0.057 M weak acid, HX, has...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Copper(l) chloride, CuCl, is the starting material...Ch. 15 - Prob. 22QAPCh. 15 - Prob. 23QAPCh. 15 - Ksp for CaSO4 at 100C is estimated to be1.6105. At...Ch. 15 - Prob. 25QAPCh. 15 - At 25C, 10.24 mg of Cr(OH)2 are dissolved in...Ch. 15 - Calcium nitrate is added to a sodium sulfate...Ch. 15 - Cadmium(ll) chloride is added to a solution of...Ch. 15 - Water from a well is found to contain 3.0 mg of...Ch. 15 - Silver(I) sulfate (Ksp=1.2105) is used in the...Ch. 15 - A solution is prepared by mixing 13.00 mL of...Ch. 15 - A solution is prepared by mixing 45.00 mL of 0.022...Ch. 15 - A solution is 0.047 M in both NaF and Na2CO3....Ch. 15 - Solid lead nitrate is added to a solution that is...Ch. 15 - A solution is made up by adding 0.632 g of barium...Ch. 15 - A solution is made up by adding 0.839 g of...Ch. 15 - Prob. 37QAPCh. 15 - To a beaker with 500 mL of water are added 95 mg...Ch. 15 - Write net ionic equations for the reaction of H+...Ch. 15 - Prob. 40QAPCh. 15 - Prob. 41QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 43QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 45QAPCh. 15 - Write an overall net ionic equation and calculate...Ch. 15 - Consider the reaction...Ch. 15 - Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2...Ch. 15 - Aluminum hydroxide reacts with an excess of...Ch. 15 - Prob. 50QAPCh. 15 - Calculate the molar solubility of gold(I) chloride...Ch. 15 - Calculate the molar solubility of PbCl2 in 0.2 M...Ch. 15 - For the reaction...Ch. 15 - For the reaction Zn(OH)2(s)+2OH(aq)Zn(OH)42(aq)...Ch. 15 - What are the concentrations of Cu2+, NH3, and...Ch. 15 - Prob. 56QAPCh. 15 - Calcium ions in blood trigger clotting. To prevent...Ch. 15 - Prob. 58QAPCh. 15 - A town adds 2.0 ppm of F- ion to fluoridate its...Ch. 15 - Consider the following hypothetical dissociation:...Ch. 15 - Prob. 61QAPCh. 15 - Consider a 2.0-L aqueous solution of 4.17 M NH3,...Ch. 15 - Marble is almost pure CaCO3. Acid rain has a...Ch. 15 - Prob. 64QAPCh. 15 - Prob. 65QAPCh. 15 - The box below represents one liter of a saturated...Ch. 15 - Consider a saturated solution of BaCO3 at 7.5C....Ch. 15 - Prob. 68QAPCh. 15 - Consider the insoluble salts JQ, K2R, L2S3, MT2,...Ch. 15 - Prob. 70QAPCh. 15 - Consider the equilibrium curve for AgCl shown...Ch. 15 - Dissolving CaCO3 is an endothermic reaction. The...Ch. 15 - Challenge Problems Insoluble hydroxides such as...Ch. 15 - What is the solubility of CaF2 in a buffer...Ch. 15 - What is [Br-] just as AgCl begins to precipitate...Ch. 15 - Prob. 76QAPCh. 15 - Prob. 77QAPCh. 15 - Prob. 78QAP
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- The Ksp for Q, a slightly soluble ionic compound composed of M22+ and X ions, is 4.5 1029. The electron configuration of M+ is [Xe]6s14f145d10. The X anion has 54 electrons. What is the molar solubility of Q in a solution of NaX prepared by dissolving 1.98 g NaX in 150. mL solution?arrow_forwardA solution is made up by adding 0.839 g of silver(I) nitrate and 1.024 g of lead(II) nitrate to enough water to make 492 mL of solution. Solid sodium chromate, Na2CrO4, is added without changing the volume of the solution. (a) Which salt will precipitate first, Ag2CrO4 or PbCrO4? (b) What is the concentration of the chromate ion when the first salt starts to precipitate?arrow_forwardA solution is made up by adding 0.632 g of barium nitrate and 0.920 g of lanthanum nitrate, to La(NO3)3 enough water to make 0.500 L of solution. Solid sodium iodate, NalO3, is added (without volume change) to the solution. (a) Which salt will precipitate first? La(IO3)3 (Ksp=7.501012) or BAIO3 (Ksp=4.0109)? (b) What is [IO3-] when the salt in (a) first begins to precipitate?arrow_forward
- To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be • no precipitate? • a precipitate of BaCO3 only? • a precipitate of CaCO3 only? • a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.arrow_forwardAn analytical chemist has a solution containing chloride ion, Cl. She decides to determine the amount of chloride ion in the solution by titrating 50.0 mL of this solution by 0.100 M AgNO3. As a way to indicate the endpoint of the titration, she added 1.00 g of potassium chromate, K2CrO4 (see Figure 17.5). As she slowly added the silver nitrate to the solution, a white precipitate formed. She continued the titration, with more white precipitate forming. Finally, the solution turned red, from another precipitate. The volume of the solution at this point was 60.3 mL. How many moles of chloride ion were there in the original solution? How many moles of chloride ion were there in the final solution? You may make any reasonable approximations.arrow_forwardWhen 1.55 g of solid thallium(I) bromide is added to 1.00 L of water, the salt dissolves to a small extent. TlBr(s)Tl+(aq)+Br(aq) The thallium(I) and bromide ions in equilibrium with TlBr each have a concentration of 1.9 103 M. What is the value of Ksp for TlBr?arrow_forward
- You have a solution that has a lead(II) ion concentration of 0.0012 M. If enough soluble chloride-containing salt is added so that the Cl concentration is 0.010 M, will PbCl2 precipitate?arrow_forwardSome barium chloride is added to a solution that contains both K2SO4 (0.050 M) and Na3PO4 (0.020 M). (a) Which begins to precipitate first: the barium sulfate or the barium phosphate? (b) The concentration of the first anion species to precipitate, either the sulfate or phosphate, decreases as the precipitate forms. What is the concentration of the first species when the second begins to precipitate?arrow_forwardLead(II) chromate, PbCrO4, was used as a yellow paint pigment (chrome yellow). When a solution is prepared that is 5.0 104 M in lead ion, Pb2, and 5.0 105 M in chromate ion, CrO42, would you expect some of the lead(II) chromate to precipitate?arrow_forward
- Solubility Equilibria Consider three hypothetical ionic solids: AX, AX2, and AX3 (each X forms X). Each of these solids has the same Ksp value, 5.5 10 7. You place 0.25 mol of each compound in a separate container and add enough water to bring the volume to 1.0 L in each case. a Write the chemical equation for each of the solids dissolving in water. b Would you expect the concentration of each solution to be 0.25 M in the compound? Explain, in some detail, why or why not. c Would you expect the concentrations of the A cations (A+, A2+, and A3+) in the three solutions to be the same? Does just knowing the stoichiometry of each reaction help you determine the answer, or do you need something else? Explain your answer in detail, but without doing any arithmetic calculations. d Of the three solids, which one would you expect to have the greatest molar solubility? Explain in detail, but without doing any arithmetic calculations. e Calculate the molar solubility of each compound.arrow_forwardA saturated solution of copper(II) iodate in pure water has a copper-ion concentration of 2.7 103 M. a What is the molar solubility of copper iodate in a 0.35 M potassium iodate solution? b What is the molar solubility of copper iodate in a 0.35 M copper nitrate solution? c Should there be a difference in the answers to parts a and b? Why?arrow_forwardThe weak base ethanolamine. HOCH2CH2NH2, can be titrated with HCl. HOCH2CH2NH2(aq)+H3O+(aq)HOCH2CH2NH3+(aq)+H2O(l) Assume you have 25.0 mL of a 0.010 M solution of ethanolamine and titrate it with 0.0095 M HCl. (Kb for ethanolamine is 3.2 107.) (a) What is the pH of the ethanolamine solution before the titration begins? (b) What is the pH at the equivalence point? (c) What is the pH at the halfway point of the titration? (d) Which indicator in Figure 17.11 would be the best choice to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 10.0, 20.0, and 30.0 mL of the acid. (f) Combine the information in parts (a), (b), (c), and (e), and plot an approximate titration curve.arrow_forward
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