CHEMISTRY:MOLECULAR..(LL)-PRINT..W/CODE
7th Edition
ISBN: 9781119457282
Author: JESPERSEN
Publisher: WILEY
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Chapter 17, Problem 131RQ
Marble is composed primarily of
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Which of the following pairs of solution would you use to prepare a buffer with pH = 7.45?
(A) Acetic acid + sodium acetate; (CH3CO2H has Ka = 1.8 x 10–5)
(B) Sodium dihydrogen phosphate + sodium hydrogen phosphate; (H2PO4– has Ka = 6.2 x 10–8)
(C) Ammonium chloride + ammonia; (NH3 has Kb = 1.8 x 10–5)
(D) Sodium hydrogen carbonate + sodium carbonate; (HCO3– has Ka = 5.6 x 10–11)
(a) (i) A tap water sample has a hardness of 285 mg/L as CaCO3. What is the predominant form of this hardness at a pH of 7.5?(ii) Provide a balanced chemical reaction showing how this hardness can be removed by the addition of lime (Ca(OH)2).(iii) How much lime is required to precipitate the hardness in 2.5 litres of this tap water? How much calcium carbonate will be precipitated? Assume the reaction is 100% efficient and the solubility of calcium carbonate under these conditions is 40 mg/LAtomic weights:Ca = 40H = 1C = 12 O = 16(b) Explain and discuss the concept of CT values to evaluate the performance of chemical oxidation processes as disinfectants during drinking water treatment.
What of the following is the expression for the solubility product of Ba3(AsO4)2?
Chapter 17 Solutions
CHEMISTRY:MOLECULAR..(LL)-PRINT..W/CODE
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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- The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)arrow_forwardAcrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?arrow_forwardWrite the net ionic equation in which the slightly soluble salt barium fluoride, BaF2, dissolves in dilute hydrochloric acid.arrow_forward
- Your answer is partially correct. Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer solution containing 46 g of NH4CI dissolved in 1.00 L of 0.920 M NH3? pH = 9.24 (b) How many moles of acid are required to change the pH of this solution by 0.07 pH units? i 5.5E-2 mol (c) Suppose 4.8 mL of 11.8 M HCI solution is added to 146 mL of the solution of Part (a). Calculate the new pH. pH = i 9.08 eTextbook and Media Save for Later Attempts: 1 of 3 used Submit Answerarrow_forward3. (6)What is the pH of a buffer that is 0.12M lactic acid (HC;H,O3) and 0.10M sodium lactate? Ka= 1.4 x 104. Write the acid dissociation reaction.arrow_forward5mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl) The Kb for ammonia is 1.75 x 10-5 1)Write a balanced chemical equation for the reaction of ammonia and hydrochloric acid and a balanced chemical equation for the equilibrium of ammonia in water. 2) What is the pH of the ammonia solution prior to the addition of any HCl?arrow_forward
- What is the solubility of NH3 if its partial pressure is reduced to 30,000 Pa?arrow_forwardChoose the acid below that would make the most effective buffer for a solution to maintain a pH of 5.00 (aq., 25 oC), given a 0.500 M concentration of it and its conjugate salt. a) propionic acid, Ka = 1.34 x 10–5 b) HN3, Ka = 1.90 x 10–5 c) butanoic acid, Ka = 1.52 x 10–5 d) NH4Cl, Ka = 5.56 x 10–10 e) benzoic acid, Ka = 6.30 x 10–5arrow_forward5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5arrow_forward
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