CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
7th Edition
ISBN: 9781119497325
Author: JESPERSEN
Publisher: WILEY
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Chapter 17, Problem 113RQ
(Calculate the molar solubility of
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A chemistry graduate student is given 450. mL of a 0.50M methylamine (CH, NH,) solution. Methylamine is a weak base with K,=4.4 × 10 *. What mass of
CH,NH,Br should the student dissolve in the CH,NH, solution to turn it into a buffer with pH = 10.96?
You may assume that the volume of the solution doesn't change when the CH,NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to
2 significant digits.
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A chemistry graduate student is given 125. mL of a 0.90M dimethylamine ((CH3)2NH) solution. Dimethylamine is a weak base with K = 5.4 × 10. What
(CH),NH,CI should the student dissolve in the (CH), NH solution to turn it into a buffer with pH = 11.23?
You may assume that the volume of the solution doesn't change when the (CH,),NH,CI is dissolved in it. Be sure your answer has a unit symbol, and round it
to 2 significant digits.
A chemistry graduate student is given 125. mL of a 1.00 M methylamine (CH ,NH,) solution. Methylamine is a weak base with K,=4.4× 10 *. What mass of
CH,NH,Br should the student dissolve in the CH,NH, solution to turn it into a buffer with pH =11.05?
You may assume that the volume of the solution doesn't change when the CH,NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to
2 significant digits.
Chapter 17 Solutions
CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
Ch. 17 - What are the ion product expressions for the...Ch. 17 - What are the ion product expressions for the...Ch. 17 - The solubility of thallium(I) iodide, TlI, in...Ch. 17 - One liter of water will dissolve mol of ....Ch. 17 - Prob. 5PECh. 17 - Calculate the molar solubility of
Ch. 17 - Calculate the molar solubility of AgI in a...Ch. 17 - Prob. 8PECh. 17 - Calculate the ion product for the solution in...Ch. 17 - Calculate the ion product for a solution...
Ch. 17 - What precipitate might be expected if we mix ?...Ch. 17 - 50.0 mL of 0.10 M Pb(NO3)2 and 20.0 mL of 0.040 M...Ch. 17 - Determine whether adding an acid will increase the...Ch. 17 - Determine the molar solubility of Ag2CrO4in1.0MH+...Ch. 17 - What pH is needed to achieve a concentration of...Ch. 17 - What pH is needed to dissolve 2.00 g PbS in...Ch. 17 - If a solution contains calcium ions (0.25 M) and...Ch. 17 - Prob. 18PECh. 17 - Suppose a solution contains and is saturated with ...Ch. 17 - Consider a solution containing , both at...Ch. 17 - The Ksp for barium oxalate,...Ch. 17 - A solution contains calcium nitrate and nickel...Ch. 17 - Calculate the solubility of silver chloride in ...Ch. 17 - How many moles of have to be added to 1.0 L of...Ch. 17 - Equilibria in Solutions of Slightly Soluble Salts...Ch. 17 - Equilibria in Solutions of Slightly Soluble Salts...Ch. 17 - Equilibria in Solutions of Slightly Soluble Salts...Ch. 17 - Equilibria in Solutions of Slightly Soluble...Ch. 17 - Prob. 5RQCh. 17 - Prob. 6RQCh. 17 - Equilibria in Solutions of Slightly Soluble Salts...Ch. 17 - Solubility of Basic Salts Is Influenced by...Ch. 17 - Prob. 9RQCh. 17 - Solubility of Basic Salts Is Influenced by...Ch. 17 - Solubility of Basic Salts Is Influenced by Acids...Ch. 17 - Solubility of Basic Salts Is Influenced by Acids A...Ch. 17 - Solubility of Basic Salts Is Influenced by Acids...Ch. 17 - Solubility of Basic Salts Is Influenced by Acids...Ch. 17 - Equilibria in Solutions of Metal Oxides and...Ch. 17 - Equilibria in Solutions of Metal Oxides and...Ch. 17 - Equilibria in Solutions of Metal Oxides and...Ch. 17 - Selective Precipitation Use Le Chatelier's...Ch. 17 - Prob. 19RQCh. 17 - Selective Precipitation If you had a solution with...Ch. 17 - Equilibria Involving Complex Ions Explain the...Ch. 17 - Equilibria Involving Complex Ions What is a...Ch. 17 - Complexation and Solubility
17.23 Using Le...Ch. 17 - Complexation and Solubility For...Ch. 17 - Prob. 25RQCh. 17 - Equilibria in Solutions of Slightly Soluble...Ch. 17 - Prob. 27RQCh. 17 - Prob. 28RQCh. 17 - Prob. 29RQCh. 17 - Prob. 30RQCh. 17 - Prob. 31RQCh. 17 - Which compound is more soluble in water,...Ch. 17 - 17.33 In water, the solubility of lead(II)...Ch. 17 - The solubility of zinc oxalate is 7.9103M....Ch. 17 - 17.35 Barium sulfate is so insoluble that it can...Ch. 17 - A student found that a maximum of 0.800 g silver...Ch. 17 - Prob. 37RQCh. 17 - A student prepared a saturated solution of CaCrO4...Ch. 17 - At 25C, the molar solubility of silver phosphate...Ch. 17 - 17.40 The molar solubility of barium phosphate in...Ch. 17 - What is the molar solubility of PbBr2 in water?Ch. 17 - 17.42 What is the molar solubility of in water?
Ch. 17 - Calculate the molar solubility of Zn(CN)2 in...Ch. 17 - Calculate the molar solubility of PbF2 in water....Ch. 17 - 17.45 At , the value of for , and that for ....Ch. 17 - At 25C, the value of Ksp for AgCNis6.010-17 and...Ch. 17 - A salt whose formula is MX has a Ksp equal to...Ch. 17 - 17.48 A salt having a formula of the type has ....Ch. 17 - Calcium sulfate is found in plaster. At 25C the...Ch. 17 - Chalk is CaCO3, and at 25CitsKsp=3.410 What is the...Ch. 17 - It was found that the molar solubility of BaSO3 in...Ch. 17 - 17.52 The molar solubility of . What is the value...Ch. 17 - Prob. 53RQCh. 17 - Mercury(I) chloride has Ksp=1.41018. Calculate the...Ch. 17 - Calculate the molar solubility of Mg(OH)2 in a...Ch. 17 - 17.56 Calculate the molar solubility of in a...Ch. 17 - 17.57 What is the highest concentration of that...Ch. 17 - 17.58 Will lead (II) bromide be less soluble in...Ch. 17 - Calculate the molar solubility of...Ch. 17 - 17.60 What is the molar solubility of in (a) 0.20...Ch. 17 - 17.61 What is the molar solubility of in a buffer...Ch. 17 - What is the molar solubility of Ca(OH)2 in (a)...Ch. 17 - In an experiment, 2.20gofNaOH(s) is added to 250...Ch. 17 - Suppose that 1.75 g of NaOH(s) is added to 250 mL...Ch. 17 - 17.65 Docs a precipitate of form when are...Ch. 17 - Prob. 66RQCh. 17 - 17.67 Docs a precipitate of form if 50.0 ml. of ...Ch. 17 - Prob. 68RQCh. 17 - 17.69 Suppose that 50.0 mL each of 0.0100 M...Ch. 17 - If a solution of 0.10 M Mn2+ and 0.10 M Cd2+ is...Ch. 17 - In an aqueous suspension of Ca(OH)2, the only...Ch. 17 - Suppose that 25.0 mL of 0.10MHCl is added to 1.000...Ch. 17 - *17.73 When solid is added to a suspension of ...Ch. 17 - *17.74 After solid was added to a slightly basic...Ch. 17 - *17.75 Will a precipitate form in a solution made...Ch. 17 - 17.76 What is the molar solubility of in water?...Ch. 17 - Solubility of Basic Salts Is Influenced by...Ch. 17 - Solubility of Basic Salts Is Influenced by...Ch. 17 - *17.79 What is the molar solubility of in pure...Ch. 17 - 17.80 What is the molar solubility of in pure...Ch. 17 - How many grams of solid sodium acetate must be...Ch. 17 - How many grams of solid potassium fluoride must be...Ch. 17 - What is the molar solubility of Mg(OH)2 in 0.1MNH3...Ch. 17 - *17.84 If 100 mL of is added to 0.400 L of a...Ch. 17 - Equilibria in Solutions of Metal Oxides and...Ch. 17 - Prob. 86RQCh. 17 - *17.87 Does nickel(II) sulfide dissolve in 4 M...Ch. 17 - Does iron(II) sulfide dissolve in 8 M HCl? Perform...Ch. 17 - Selective Precipitation Both AgCl and AgI are very...Ch. 17 - Prob. 90RQCh. 17 - 17.91 What value of and what pH permit the...Ch. 17 - What pH would yield the maximum separation of Mn2+...Ch. 17 - Prob. 93RQCh. 17 - Kidney stones often contain insoluble calcium...Ch. 17 - 17.95 Solid is added to a solution of . After...Ch. 17 - What value of [ H+ ] and what pH would allow the...Ch. 17 - Prob. 97RQCh. 17 - *17.98 In the metal plating industry, the waste is...Ch. 17 - Equilibria Involving Complex Ions
17.99 Write the...Ch. 17 - Equilibria Involving Complex Ions
17.100 Write the...Ch. 17 - Prob. 101RQCh. 17 - Prob. 102RQCh. 17 - Prob. 103RQCh. 17 - Prob. 104RQCh. 17 - For PbCl3, Kform=2.510 . Use this information plus...Ch. 17 - The overall formation constant for Ag(CN)2 equals...Ch. 17 - How many grams of solid NaCN have to be added to...Ch. 17 - Prob. 108RQCh. 17 - Silver iodide is very insoluble and can be...Ch. 17 - 17.110 Silver forms a sparingly soluble iodide...Ch. 17 - The formation constant for Ag(CN)2-equals5.341018....Ch. 17 - 17.112 Suppose that some dipositive cation, , is...Ch. 17 - (Calculate the molar solubility of...Ch. 17 - The molar solubility of Zn(OH)2in1.0MNH3 is...Ch. 17 - What ratio of Ksp values will allow for the use of...Ch. 17 - A student had a solution that contained...Ch. 17 - Suppose that 50.0 mL of 0.12 M AgNO3 is added to...Ch. 17 - Prob. 118RQCh. 17 - Prob. 119RQCh. 17 - In Example 17.11 we say, there are relatively few...Ch. 17 - *17.121 What is the molar solubility of ? What is...Ch. 17 - *17.122 An old method for mining gold was to wash...Ch. 17 - What is the molar concentration of Cu2+ ion in a...Ch. 17 - On the basis of the KspofAl(OH)3, what would be...Ch. 17 - The compound EDTA is used to remove soap scum, as...Ch. 17 - A chemist has a solution that contains a mixture...Ch. 17 - You are given a sample containing , both with...Ch. 17 - Prob. 128RQCh. 17 - In modern construction, walls and ceilings are...Ch. 17 - *17.130 How many milliliters of would have to be...Ch. 17 - Marble is composed primarily of CaCO3, a slightly...Ch. 17 - *17.132 The pH of a saturated solution of is 9.8....Ch. 17 - The osmotic pressure of a saturated solution of...Ch. 17 - A saturated solution of PbCl2 has a freezing point...Ch. 17 - 17.135 Consider mercury(II) sulfide, , which has a...Ch. 17 - If aqueous ammonia is added gradually to a...Ch. 17 - From a practical standpoint, can you effectively...Ch. 17 - 17.139 In older textbooks, the solubility...Ch. 17 - Suppose two silver wires, one coated with silver...
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- Consider the nanoscale-level representations for Question 110 of the titration of the aqueous weak acid HX with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: After a very small volume of titrant has been added to the initial HX solution? When enough titrant has been added to take the solution just past the equivalence point? Halfway to the equivalence point? At the equivalence point? Nanoscale representations for Question 110.arrow_forwardYou want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?arrow_forwardA 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume that volumes are additive.) (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of nitric acid is required to reach the equivalence point? (d) What is the pH of the solution before any HNO3 is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?arrow_forward
- When a diprotic acid, H2A, is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If the pH at 50.0 mL NaOH added is 4.0, and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka1, and Ka2 for the diprotic acid.arrow_forwardA chemistry graduate student is given 450. mL of a 1.10M methylamine (CH,NH,) solution. Methylamine is a weak base 4 with K- :4.4 × 10 What mass of CH,NH,Cl should the student dissolve in the CH,NH, solution to turn it into a buffer with pH = 10.14? You may assume that the volume of the solution doesn't change when the CH,NH,Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10arrow_forwardA chemistry graduate student is given 100. mL of a 0.90M trimethylamine ((CH3)N) solution. Trimethylamine is a weak base with K₁=7.4 × 104. f (CH3)2NHCl should the student dissolve in the (CH3)2N solution to turn it into a buffer with pH = 10.66? mass of You may assume that the volume of the solution doesn't change when the (CH3)2NHC1 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0x12 What X S ? EFET ol Ararrow_forward
- 4 A chemistry graduate student is given 100. mL of a 0.50M methylamine (CH,NH,) solution. Methylamine is a weak base with K,=4.4 × 10 *. What mass of CH,NH,Cl should the student dissolve in the CH, NH, solution to turn it into a buffer with pH = 10.93? You may assume that the volume of the solution doesn't change when the CH,NH, Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. olo Ar x10arrow_forwardTo fill a 500 mL volumetric flask, 40 g of ammonium chloride (NH4Cl) and 3.2 g of ammonia (NH3) are added along with water. Given the Kb of NH3 is 1.8 × 10−5, the pH of this buffer is...arrow_forwardCalculate the minimum pH needed to precipitate Mn(OH)2 so completely that the concentration of Mn2+ is less than 1 microgram per liter (1 part per billion (ppb)).arrow_forward
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