Classes at: - Topic: Ionic Equilibrium
|
|
- Jared Taylor
- 5 years ago
- Views:
Transcription
1 01. Hydrogen ion concentration in mol/l in a solution of ph = 5.4 will be : [AIEEE 2005] (a) (b) (c) (d) If the dissociation constant of an acid HA is , the ph of a 0.1 M solution of the acid HA will be approximately : [MPCET 1999] (a) 3 (b) 5 (c) 1 (d) The ph of a solution is 5.0. To this solution sufficient acid is added to decrease the ph to 2.0. The increase in hydrogen ion concentration is:[pmt (MP) 90; CPMT 90] (a) 1000 times (b) 5/2 times (c) 100 times (d) 5 times 04. When the ph of a solution is 2 the hydrogen ion concentration is : [NCERT 1993] (a) M (b) M (c) M (d) M 05. The ph of 1/1000 N KOH solution is: [MLNR 1991; CET (Karnataka) 1992] (a) (b) 3 (c) 2 (d) At 90 C, pure water has [H 3 O + ] = 10 6 mol/ litre. The value of K w at 90 C is : [MLNR 1990; CBSE (PMT) 1993] (a) 10 6 (b) (c) (d) ph of a 10 8 M solution of HCl in water is: [MLNR 1990] (a) 8 (b) 8 (c) between 7 and 8 (d) between 6 and 7 PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna Topic: Ionic Equilibrium Meq. Approach 08. The ph of the solution is 4. The hydrogen ion concentration of the solution in mol/litre is : [CPMT 1991] (a) 10 2 (b) 10 4 (c) 10 4 (d) The ph of 0.1 N HCl solution is: (a) 1.0 (b) 7.0 (c) 14.0 (d) molar solution of formic acid is 3.2% ionized. Its ionization constant is: (a) (b) (c) (d) pk a values of four acids are given below at 25 C. The strongest acid is: [PMT (MP) 90] (a) 2.0 (b) 2.5 (c) 3.0 (d) The values of dissociation constant of some acids (at 25 C) are given below. The strongest acid in water is : (a) (b) (c) (d) The concentration of hydrogen ion [H + ] and ph in 10 M HCl is : [CBSE (PMT) 1995] (a) 10 1, zero (b) 10 1, 1 (c) 10 2, 1 (d) 10 1, The ph of solution, whose hydrogen ion concentration is one mol per litre, will be: (a) 1.0 (b) 0.1 (c) zero (d) 1.5 Page No.: 1
2 15. The ph of 0.1 M HCl is approximately 1. The approximate ph of 0.05 M H 2 SO 4 is : (a) 0.05 (b) 0.5 (c) 1 (d) The ph of a 0.01 M solution of acetic acid having degree of dissociation 12.5% is: (a) (b) (c) (d) The ph of water is 7 at 25 C. If water is heated to 50 C, which of the following should be true? (a) ph will decrease (b) ph will increase (c) ph will remain seven (d) [H + ] will increase but [OH ] will decrease 18. The [H 3 O + ] in the rain water of ph = 4.35 is: (a) M (b) M (c) M (d) M 19. The [OH ] in 100 ml of M HCl (aq.) is : (a) M (b) M (c) M (d) M 20. Which solution will have ph closer to 1.0? [IIT 1992] (a) 100 ml of (M/10) HCl ml of (M/10) NaOH (b) 55 ml of (M/10) HCl + 45 ml of (M/10) NaOH (c) 10 ml of (M/10) HCl + 90 ml of (M/10) NaOH (d) 75 ml of (M/5) HCl + 25 ml of (M/5) NaOH 21. Which of the following will occur if a 0.1 M solution of a weak acid is diluted to 0.01 M at constant temperature? [ MLNR 1992; AIIMS 1993] (a) [H + ] will decrease to 0.01 M (b) ph will decrease (c) percentage ionization will increase (d) K a will increase 22. A certain buffer solution contains equal concentration of X and HX. The K a for HX is The ph of the buffer is : [MLNR 1992] (a) 3 (b) 8 (c) 11 (d) The ph of a M NaOH solution is nearest to : [MLNR 1992] (a) 10 (b) 7 (c) 4 (d) The ph of a 0.02 M solution of hydrochloric acid is : [PMT (MP) 1993] (a) 2.0 (b) 1.7 (c) 0.3 (d) ph of 0.05 M Mg(OH) 2 is: [CBSE (PMT) 90] (a) 13 (b) 10 (c) 1 (d) zero 26. K a for HCN is at 25 C. For maintaining a constant ph of 9, the volume of 5 M KCN solution required to be added to 10 ml of 2 M HCN solution is: [CBSE (PMT) 93] (a) 4 ml (b) 7.95 ml (c) 2 ml (d) 9.3 ml 27. An aqueous solution of 0.1 M NH 4 Cl will have a ph closer to : [ AIIMS 1993] (a) 9.1 (b) 8.1 (c) 7.1 (d) The number of mole of hydroxide [OH ] ion in 0.3 litre of M solution of Ba(OH) 2 is : [CPMT 1991] (a) (b) (c) (d) A 0.01 M ammonia solution is 5% ionized. The concentration of [OH ] ion is : [CET (Karnataka) 1993] (a) M (b) M (c) M (d) 0.05 M g of pure NaOH is dissolved in 10 litre of distilled water. The ph of the solution is : [CET (Karnataka) 1991] (a) 9 (b) 10 (c) 11 (d) 12 Page No.: 2
3 31. The ph of the solution produced when an aqueous solution of strong acid ph 5 is mixed with equal volume of an aqueous solution of strong acid of ph 3 is:[cet (Karnataka) 91] (a) 3.3 (b) 3.5 (c) 4.5 (d) An acid-base indicator has K a = The acid form of the indicator is red and the basic form is blue. the [H + ] required to change the indicator from 75% red to 75% blue is : [CET (Karnataka) 1993] (a) M (b) M (c) M (d) M 33. A certain weak acid has a dissociation constant The equilibrium constant for its reaction with a strong base is : [IIT 1994] (a) (b) (c) (d) If K a for a weak acid is pk b value of its conjugate base is : [NTSE 1991] (a) 5 (b) 6 (c) 7 (d) A solution of ph 9.0 is one thousand times as basic as a solution of ph :[EAMCET 1990] (a) 6 (b) 7 (c) 4 (d) In 100 ml of an aqueous HCl of ph 1.0, 900 ml of distilled water is added, the ph of the resultant solution becomes : [EAMCET 92] (a) 1.0 (b) 2.0 (c) 4.0 (d) The ph of a soft drink is Its H + ion concentration will be : [PMT (MP) 1990] (a) mol/litre (b) mol/litre (c) mol/litre (d) mol/litre 38. The heat of neutralization ( H) of a strong acid and strong base in dilute aqueous solutions at 25 C is : [BHU 1992,93] (a) kj (b) kj (c) kj (d) kj 39. The dissociation constant of HCN is The value of hydrolysis constant of KCN will be : [BHU 1992] (a) (b) (c) (d) If the solubility of lithium sodium hexafluoroaluminate, Li 3 Na 3 (AlF 6 ) 2 is a mol/litre, its solubility product is equal to : [CPMT 92] (a) a 2 (b) 12a 2 (c) 18a 3 (d) 2916a The solubility of AgCl in water at 10 C is mol/litre. The K sp of AgCl is : [BHU 1992] (a) [ ] 1/2 (b) 6.2 (10 6 ) 2 (c) (6.2) (d) [ ] K sp of AgCl at 18 C is If Ag + of solution is mol/litre the Cl that must exceed before AgCl is precipitated would be: [CPMT 1991] (a) mol/litre (b) mol/litre (c) mol/litre (d) mol/litre 43. In which of the following solutions the solubility of AgCl will be maximum? [CBSE (PMT) 1993] (a) 0.1 M AgNO 3 (b) Water (c) 0.1 M NaCl (d) 0.1 M KCl 44. The solubility of PbCl 2 in water is 0.01 M at 25 C. Its maximum concentration in 0.1 M NaCl will be : [CBSE (PMT) 1993] (a) M (b) M (c) M (d) M 45. If the solubility product of lead iodide (PbI 2 ) is , its solubility will be : [PMT (MP)90] (a) M (b) M (c) M (d) M 46. The solubility product of a salt AB 2 is at 373 K. The solubility of AB 2 in boiling water will be : [Roorkee 1990] (a) M (b) M (c) M (d) M Page No.: 3
4 47. The solubility of AgCl is g/litre. The solubility product of AgCl will be : (a) (b) (c) (d) Under the same conditions which mixture by volume of 1 M potassium hydroxide and 1 M nitric acid solution produces the highest temperature? [PMT (MP) 1990] (a) (b) (c) (d) If the concentration of CrO 4 ion in a saturated solution of silver chromate be M, solubility product of silver chromate will be : [CPMT 1993] (a) (b) (c) (d) At 30 C the solubility of Ag 2 CO 3 (K sp = ) would be greatest in one litre of [PMT (MP) 1990] (a) 0.05 M Na 2 CO 3 (b) 0.05 M AgNO 3 (c) pure water (d) 0.05 M K 2 CO Heat of neutralization for the reaction NaOH + HCl NaCl + H 2 O is 57.1 kj mol 1. What will be the heat released when 0.25 mole of NaOH is titrated against 0.25 mole of HCl? [CPMT 1990] (a) 22.5 kj (b) 57.1 kj (c) 14.3 kj (d) 28.6 kj 52. The solubility of AgCl (K sp = ) in a 0.10 M NaCl solution is : [PMT (MP) 1992; Roorkee 1995] (a) 0.1 M (b) M (c) M (d) M 53. Solubility product of MX 2 at 298 K is At this temperature concentration of M 2+ ion in mol per litre is : [AIEEE 2005] (a) M (b) M (c) M (d) M 54. The precipitate of CaF 2 (K sp = ) is obtained when equal volumes of the following are mixed : [PMT (MP) 1990; MLNR 1992] (a) 10 4 M Ca M F (b) 10 2 M Ca M F (c) 10 5 M Ca M F (d) 10 3 M Ca M F 55. How many gram of CaC 2 O 4 will dissolve in one litre of saturated solution? K sp of CaC 2 O 4 is mol 2 and its molecular weight is 128 : [PMT (MP) 1993] (a) g (b) g (c) g (d) g 56. The ph of a M NaOH solution is nearest to : [MLNR 1992] (a) 10 (b) 7 (c) 4 (d) A physician wishes to prepare a buffer solution at ph = 3.58 that efficiently resists a change in ph yet contains only small conc. of the buffering agents. Which one of the following weak acid together with its sodium salt would be best to use?[cbse (PMT) 97] (a) m-chloro bezoic acid (pk a = 3.98) (b) p-chlorocinnamic acid (pk a = 4.41) (c) 2, 5-dihydroxy benzoic acid (pk a = 2.97) (d) Acetoacetic acid (pk a = 3.58) 58. K b for the hydrolysis reaction, B + + H 2 O BOH + H + is , the hydrolysis constant of the salt is : [Roorkee 1998] (a) 10 6 (b) 10 7 (c) 10 8 (d) The hydroxide with highest solubility product is : [Roorkee 1994] (a) Al(OH) 3 (b) CO(OH) 2 (c) Cr(OH) 3 (d) Fe(OH) The dissociation constant of NH 4 OH is The hydrolysis constant of NH 4 Cl would be : [Roorkee 1993] (a) (b) (c) (d) The ph of 1.0 M aqueous solution of a weak acid HA is 6.0. Its dissociation constant is : [Roorkee 1993] (a) 10 6 (b) (c) 1.0 (d) 6.0 Page No.: 4
5 62. A weak acid HX (K a = ) on reaction with NaOH gives NaX. For 0.1 M aqueous solution of NaX, the % hydrolysis is : [IIT 2004] (a) 0.001% (b) 0.01% (c) 0.15% (d) 1% 63. In a mixture of CH 3 COOH and CH 3 COONa, the ratio of salt to acid concentration is increased by ten folds. The ph of the solution will increase by: [Roorkee 1991] (a) Zero (b) 1 (c) 2 (d) If pk b for fluoride ion at 25 C is 10.83, the ionization constant of hydrofluoric acid in water at this temperature is: [IIT 1997] (a) (b) (c) (d) The solubility of a saturated solution of calcium fluoride is moles per litre. Its solubility product is: [CBSE (PMT) 1999] (a) (b) (c) (d) At infinite dilution, the percentage ionisation for both strong and weak electrolytes is : [CPMT 1999] (a) 1% (b) 20% (c) 50% (d) 100% 67. A buffer solution is prepared by mixing 10 ml of 1.0 M acetic and 20 ml of 0.5 M sodium acetate and then diluted to 100 ml with distilled water. If the pk a of CH 3 COOH is 4.76, what is the ph of the buffer solution prepared? [MPCET 1999] (a) 5.21 (b) 4.76 (c) 4.34 (d) To neutralise completely 20 ml of 0.1 M aqueous solution of phosphorous acid H 3 PO 3, the volume of 0.1 M KOH solution required is : [AIEEE 2004] (a) 60 ml (b) 20 ml (c) 40 ml (d) 10 ml 69. What is the correct representation for the solubility product of SnS 2? [MPCET 1999] (a) [Sn 2+ ] [S 2 ] 2 (b) [Sn 4+ ] [S 2 ] 2 (c) [Sn 2+ ] [2S 2 ] (d) [Sn 4+ ] [2S 2 ] The concentration of [H + ] and concentration of [OH ] of a 0.1 M aqueous solution of 2% ionised weak acid is [ionic product of water = ] : [CBSE (PMT) 1999] (a) M and M (b) M and M (c) M and M (d) M and M 71. The solubility product of a sparingly soluble salt AX 2 is Its solubility (in mol/ litre) is : [CBSE (PMT) 2004] (a) (b) (c) (d) The solubility in water off a sparingly soluble salt AB 2 is mol/litre. Its solubility product is : [AIEEE 2003] (a) (b) (c) (d) Solubility of an aqueous solution of Mg(OH) 2 is X mole litre 1, then its K sp is: [AIEEE 2002] (a) 4X 3 (b) 108X 5 (c) 27X 4 (d) 9X mole of CH 3 NH 2 (K b = ) is mixed with 0.08 mole of HCl and diluted to 1 litre. The [H + ] in solution is: [IIT 2005] (a) M (b) M (c) M (d) M 75. AT 25 C, K b for a base BOH is The [OH ] in 0.01 M aqueous solution of base is : [CBSE (PMT) 2005] (a) (b) (c) (d) The hydrogen ion concentration of a 10 8 M HCl aqueous solution at 298 K (K w = ) is : [CBSE (PMT) 2006] (a) M (b) M (c) M (d) M Page No.: 5
6 A N S W E R 01. d 02. a 03. a 04. b 05. d 06. b 07. d 08. c 09. a 10. b 11. a 12. a 13. a 14. c 15. c 16. c 17. a 18. a 19. c 20. d 21. c 22. b 23. b 24. b 25. a 26. c 27. d 28. c 29. c 30. b 31. a 32. c 33. c 34. d 35. a 36. b 37. c 38. b 39. d 40. d 41. d 42. a 43. b 44. d 45. a 46. d 47. b 48. c 49. c 50. c 51. c 52. c 53. b 54. b 55. a 56. b 57. d 58. c 59. b 60. d 61. b 62. b 63. b 64. c 65. d 66. d 67. b 68. c 69. b 70. c 71. c 72. c 73. a 74. b 75. a 76. d Page No.: 6
Classes at: - Topic: Ionic Equilibrium
PHYSICAL CHEMISTRY by: SHAILENDRA KR Classes at: - SCIENCE TUTORIALS; Opp Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No 5A/65, Opp Mahual Kothi, Alpana Market, Patna Topic:
More informationPHYSICAL CHEMISTRY. by: SHAILENDRA KR. Meq. Approach. Classes at: - Topic: Mole Concept
PHYSICAL CHEMISTRY by: SHAILENDRA KR. asses at: - SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna Topic:
More informationClasses at: - Confidence building Problems
PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna Confidence
More informationAP Chemistry. CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect Buffered Solutions. Composition and Action of Buffered Solutions
AP Chemistry CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak electrolyte.
More informationChem 103 Exam #1. Identify the letter of the choice that best completes the statement or answers the question. Multiple Choice
Chem 103 Exam #1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which of the following can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry
More informationAcids, Bases, & Neutralization Chapter 20 & 21 Assignment & Problem Set
Acids, Bases, & Neutralization Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Acids, Bases, & Neutralization 2 Study Guide: Things You Must Know
More informationChap 17 Additional Aspects of Aqueous Equilibria. Hsu Fu Yin
Chap 17 Additional Aspects of Aqueous Equilibria Hsu Fu Yin 1 17.1 The Common-Ion Effect Acetic acid is a weak acid: CH 3 COOH(aq) H + (aq) + CH 3 COO (aq) Sodium acetate is a strong electrolyte: NaCH
More information7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M
Solubility, Ksp Worksheet 1 1. How many milliliters of 0.20 M AlCl 3 solution would be necessary to precipitate all of the Ag + from 45ml of a 0.20 M AgNO 3 solution? AlCl 3(aq) + 3AgNO 3(aq) Al(NO 3)
More informationCHAPTER 7.0: IONIC EQUILIBRIA
Acids and Bases 1 CHAPTER 7.0: IONIC EQUILIBRIA 7.1: Acids and bases Learning outcomes: At the end of this lesson, students should be able to: Define acid and base according to Arrhenius, Bronsted- Lowry
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium Sample Exercise 17.1 (p. 726) What is the ph of a 0.30 M solution of acetic acid? Be sure to use a RICE table, even though you may not need it. (2.63) What
More informationChapter 19. Solubility and Simultaneous Equilibria p
Chapter 19 Solubility and Simultaneous Equilibria p. 832 857 Solubility Product ) The product of molar concentrations of the constituent ions, each raised ot the power of its stoichiometric coefficients
More informationTopic: Units of Solubility Product Constant 1. The units of the solubility product of Cu 2. are : a) M 2 b) M 5 c) M d) M 3 ) 4
PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - Meq. Approach SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market,
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak
More informationFunsheet 9.1 [VSEPR] Gu 2015
Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NI 3 CF 4 OCl 2 C 2 F 2 HOF Funsheet 9.1 [VSEPR] Gu 2015
More informationTopic: Chemical Kinetics SO HCI 2 + 2I
PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - Meq. Approach SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market,
More informationEquilibri acido-base ed equilibri di solubilità. Capitolo 16
Equilibri acido-base ed equilibri di solubilità Capitolo 16 The common ion effect is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance.
More informationClasses at: - Topic: Mole Concept, Volumetric & Redox Titration
01) To prepare a solution that is 0.0 KCl starting with 100 ml of 0.0 KCl (a) Add 0.7 g KCl (b) Add 0 ml of water Add 0.10 mole KCl (d) Evaporate 10 ml water 0) 10.78 g of H PO in 0 ml solution is 0.0
More informationTopic: Mole Concept. (At. mass, Ba= 137) will be
PHYSICAL CHEMISTRY by: SHAILENDRA KR. Meq. Approach Classes at: - SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market,
More informationTopic 9: Acids & Bases
Topic 9: Acids & Bases Regents Chemistry Mr. Mancuso Electrolytes Substances that conduct electricity when Include Ability to conduct electricity is due to the presence of Dissociation: ~ 1 ~ Acids and
More informationSecondary Topics in Equilibrium
Secondary Topics in Equilibrium Outline 1. Common Ions 2. Buffers 3. Titrations Review 1. Common Ions Include the common ion into the equilibrium expression Calculate the molar solubility in mol L -1 when
More informationCh 8 Practice Problems
Ch 8 Practice Problems 1. What combination of substances will give a buffered solution that has a ph of 5.05? Assume each pair of substances is dissolved in 5.0 L of water. (K a for NH 4 = 5.6 10 10 ;
More informationAcid-Base Equilibria and Solubility Equilibria Chapter 17
PowerPoint Lecture Presentation by J. David Robertson University of Missouri Acid-Base Equilibria and Solubility Equilibria Chapter 17 The common ion effect is the shift in equilibrium caused by the addition
More informationReview of Chemistry 11
Review of Chemistry 11 HCl C 3 H 8 SO 2 NH 4 Cl KOH H 2 SO 4 H 2 O AgNO 3 PbSO 4 H 3 PO 4 Ca(OH) 2 Al(OH) 3 P 2 O 5 Ba(OH) 2 CH 3 COOH 1. Classify the above as ionic or covalent by making two lists. Describe
More informationAP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section
Slide 1 / 91 Slide 2 / 91 AP Chemistry Aqueous Equilibria II: Ksp & Solubility Products Table of Contents: K sp & Solubility Products Slide 3 / 91 Click on the topic to go to that section Introduction
More informationTopic: Balancing Equations. 1. Balance the following equation. What is the sum of the coefficients of the reactants and products?
PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - Meq. Approach SCIENCE TUTRIALS; pp. Khuda Baksh Library, Ashok Rajpath, Patna PIN PINT STUDY CIRCLE; House No. 5A/65, pp. Mahual Kothi, Alpana Market,
More informationName Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
More informationCHM 1046 Test #4 April 24, 2001
CHM 1046 Test #4 April 24, 2001 1. Which one of the following is a strong acid? a. H 2 CO 3 b. H 2 SO 3 c. H 2 SO 4 d. H 3 PO 4 e. CH 3 COOH 2. The substance (CH 3 CH 2 ) 2 NH is considered a. a weak acid
More informationChemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten; Catherine J. Murphy.
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten; Catherine J. Murphy Chapter 17 Additional Aspects of Aqueous Equilibria Ahmad Aqel Ifseisi Assistant
More informationReview 7: Solubility Equilibria
Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both
More informationOperational Skills. Operational Skills. The Common Ion Effect. A Problem To Consider. A Problem To Consider APPLICATIONS OF AQUEOUS EQUILIBRIA
APPLICATIONS OF AQUEOUS EQUILIBRIA Operational Skills Calculating the common-ion effect on acid ionization Calculating the ph of a buffer from given volumes of solution Calculating the ph of a solution
More informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9) ( F - 32) F = ( 9 / 5)( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More informationCh. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2
Ch. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution
More informationChapter 17. Additional Aspects of Aqueous Equilibria 蘇正寬 Pearson Education, Inc.
Chapter 17 Additional Aspects of Aqueous Equilibria 蘇正寬 chengkuan@mail.ntou.edu.tw Additional Aspects of Aqueous Equilibria 17.1 The Common-Ion Effect 17.2 Buffers 17.3 Acid Base Titrations 17.4 Solubility
More informationAqueous Equilibria, Part 2 AP Chemistry Lecture Outline
Aqueous Equilibria, Part 2 AP Chemistry Lecture Outline Name: The Common-Ion Effect Suppose we have a weak acid and a soluble salt of that acid. CH 3 COOH NaCH 3 COO CH 3 COOH CH 3 COO + H + Since NaCH
More informationph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor
ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate
More informationUnit-8 Equilibrium. Rate of reaction: Consider the following chemical reactions:
Unit-8 Equilibrium Rate of reaction: Consider the following chemical reactions: 1. The solution of sodium chloride and silver nitrate when mixed, there is an instantaneous formation of a precipitate of
More informationCreate assignment, 48975, Exam 2, Apr 05 at 9:07 am 1
Create assignment, 48975, Exam 2, Apr 05 at 9:07 am 1 This print-out should have 30 questions. Multiple-choice questions may continue on the next column or page find all choices before making your selection.
More informationEquilibrium principles in aqueous systems are limited to qualitative descriptions and/or calculations involving:
NCEA Chemistry 3.6 Aqueous Systems AS 91392 Demonstrate understanding of equilibrium principles in aqueous systems Aqueous systems are limited to those involving sparingly soluble ionic solids Equilibrium
More informationREVIEW QUESTIONS Chapter 17
Chemistry 102 REVIEW QUESTIONS Chapter 17 1. A buffer is prepared by adding 20.0 g of acetic acid (HC 2 H 3 O 2 ) and 20.0 g of sodium acetate (NaC 2 H 3 O 2 ) in enough water to prepare 2.00 L of solution.
More informationAcid-Base Equilibria and Solubility Equilibria
ACIDS-BASES COMMON ION EFFECT SOLUBILITY OF SALTS Acid-Base Equilibria and Solubility Equilibria Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 2 The common
More informationChapter 17 Additional Aspects of
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 17 Additional Aspects of John D. Bookstaver St. Charles Community College Cottleville,
More informationDougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria
Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria This is a PRACTICE TEST. Complete ALL questions. Answers will be provided so that you may check your work. I strongly
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationChemistry 102 Chapter 17 COMMON ION EFFECT
COMMON ION EFFECT Common ion effect is the shift in equilibrium caused by the addition of an ion that takes part in the equilibrium. For example, consider the effect of adding HCl to a solution of acetic
More informationThe solubility of insoluble substances can be decreased by the presence of a common ion. AgCl will be our example.
COMMON ION EFFECT WORKED PROBLEMS The solubility of insoluble substances can be decreased by the presence of a common ion. AgCl will be our example. Present in silver chloride are silver ions (Ag + ) and
More informationChapter 15 Additional Aspects of
Chemistry, The Central Science Chapter 15 Additional Aspects of Buffers: Solution that resists change in ph when a small amount of acid or base is added or when the solution is diluted. A buffer solution
More informationConsider a normal weak acid equilibrium: Which direction will the reaction shift if more A is added? What happens to the % ionization of HA?
ch16blank Page 1 Chapter 16: Aqueous ionic equilibrium Topics in this chapter: 1. Buffers 2. Titrations and ph curves 3. Solubility equilibria Buffersresist changes to the ph of a solution. Consider a
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More information5. What is the percent ionization of a 1.4 M HC 2 H 3 O 2 solution (K a = ) at 25 C? A) 0.50% B) 0.36% C) 0.30% D) 0.18% E) 2.
Name: Date: 1. For which of the following equilibria does K c correspond to an acid-ionization constant, K a? A) NH 3 (aq) + H 3 O + (aq) NH 4 + (aq) + H 2 O(l) B) NH 4 + (aq) + H 2 O(l) NH 3 (aq) + H
More informationCHAPTER 16 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA
CHAPTER 16 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA 16.3 (a) This is a weak acid problem. Setting up the standard equilibrium table: CH 3 COOH(aq) H + (aq) + CH 3 COO (aq) Initial (M): 0.40 0.00
More informationChemical Equilibrium Chapter 6
Chemical Equilibrium Chapter 6 "When a system is in chemical equilibrium, a change in one of the parameters of the equilibrium produces a shift in such a direction that, were no other factors involved
More informationChemistry Lab Equilibrium Practice Test
Chemistry Lab Equilibrium Practice Test Basic Concepts of Equilibrium and Le Chatelier s Principle 1. Which statement is correct about a system at equilibrium? (A) The forward and reverse reactions occur
More information(i) Purification of common salt
(i) Purification of common salt Natural common salt consists of many insoluble and soluble impurities. Saturated solution of common salt is prepared and insoluble impurities are filtered off. Hydrogen
More informationName Date. 9. Which substance shows the least change in solubility (grams of solute) from 0 C to 100 C?
Solubility Curve Practice Problems Directions: Use the graph to answer the questions below. Assume you will be using 100g of water unless otherwise stated. 1. How many grams of potassium chloride (KCl)
More information(for tutoring, homework help, or help with online classes)
www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. chem10b 17.2-5 Of the following solutions, which has the greatest buffering capacity? A. 0.821 M HF and 0.909 M NaF
More informationAcid and Bases. Physical Properties. Chemical Properties. Indicators. Corrosive when concentrated. Corrosive when concentrated.
Physical Properties Acid and Bases Chemistry 30 Acids Corrosive when concentrated Have a sour taste Bases Corrosive when concentrated Have a bitter taste Often have a sharp odour Chemical Properties Indicators
More informationAP Chapter 15 & 16: Acid-Base Equilibria Name
AP Chapter 15 & 16: Acid-Base Equilibria Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 15 & 16: Acid-Base Equilibria 2 Warm-Ups (Show
More informationTry this one Calculate the ph of a solution containing M nitrous acid (Ka = 4.5 E -4) and 0.10 M potassium nitrite.
Chapter 17 Applying equilibrium 17.1 The Common Ion Effect When the salt with the anion of a is added to that acid, it reverses the dissociation of the acid. Lowers the of the acid. The same principle
More informationChapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill
Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component
More informationSOLUBILITY REVIEW QUESTIONS
Solubility Problem Set 1 SOLUBILITY REVIEW QUESTIONS 1. What is the solubility of calcium sulphate in M, g/l, and g/100 ml? 2. What is the solubility of silver chromate? In a saturated solution of silver
More informationAcid-Base Equilibria and Solubility Equilibria
Acid-Base Equilibria and Solubility Equilibria Acid-Base Equilibria and Solubility Equilibria Homogeneous versus Heterogeneous Solution Equilibria (17.1) Buffer Solutions (17.2) A Closer Look at Acid-Base
More informationX212F Which of the following is a weak base in aqueous solution? A) H 2 CO 3 B) B(OH) 3 C) N 2 H 4 D) LiOH E) Ba(OH) 2
PX212SP14 Practice Exam II / Spring 2014 1. Which of the following statements are characteristic of acids? 1. They are proton donors. 2. They react with bases to produce a salt and water. 3. They taste
More informationMr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases
Acids and Bases 1 UNIT 4: ACIDS & BASES OUTCOMES All important vocabulary is in Italics and bold. Outline the historical development of acid base theories. Include: Arrhenius, BronstedLowry, Lewis. Write
More informationI. Multiple Choice Questions (Type-I) is K p
Unit 7 EQUILIBRIUM I. Multiple Choice Questions (Type-I) 1. We know that the relationship between K c and K p is K p K c (RT) n What would be the value of n for the reaction NH 4 Cl (s) NH 3 (g) + HCl
More informationSOLUBILITY PRODUCT (K sp ) Slightly Soluble Salts & ph AND BUFFERS (Part Two)
SOLUBILITY PRODUCT (K sp ) Slightly Soluble Salts & ph AND BUFFERS (Part Two) ADEng. PRGORAMME Chemistry for Engineers Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore
More informationAP CHEMISTRY NOTES 10-1 AQUEOUS EQUILIBRIA: BUFFER SYSTEMS
AP CHEMISTRY NOTES 10-1 AQUEOUS EQUILIBRIA: BUFFER SYSTEMS THE COMMON ION EFFECT The common ion effect occurs when the addition of an ion already present in the system causes the equilibrium to shift away
More informationAdditional Aspects of Aqueous Equilibria David A. Katz Department of Chemistry Pima Community College
Additional Aspects of Aqueous Equilibria David A. Katz Department of Chemistry Pima Community College The Common Ion Effect Consider a solution of acetic acid: HC 2 H 3 O 2(aq) + H 2 O (l) H 3 O + (aq)
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationCHEMISTRY - BURDGE-ATOMS FIRST 3E CH.17 - ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA
!! www.clutchprep.com CONCEPT: CLASSIFICATION AND IDENTIFICATION OF BUFFERS Solutions which contain a acid and its base are called buffer solutions because they resist drastic changes in ph. They resist
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak
More informationChem 112, Fall 05 Exam 3A
Before you begin, make sure that your exam has all 10 pages. There are 32 required problems (3 points each, unless noted otherwise) and two extra credit problems (3 points each). Stay focused on your exam.
More informationNo Brain Too Small CHEMISTRY AS90700 Describe properties of aqueous systems. ph of weak acids, weak bases and salt solutions
ph of weak acids, weak bases and salt solutions 2010: 1 An aqueous solution of ammonium chloride (NH 4 Cl) has a ph of 4.66. (a) (i) Write the equation for solid ammonium chloride dissolving in water.
More informationExample 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates
Example 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates For Practice 15.1 In each reaction, identify the Brønsted Lowry acid, the Brønsted Lowry base, the conjugate acid, and the conjugate
More informationNet Ionic Reactions. The reaction between strong acids and strong bases is one example:
Net Ionic Reactions Model 1 Net Ionic Reactions. Net ionic reactions are frequently used when strong electrolytes react in solution to form nonelectrolytes or weak electrolytes. These equations let you
More informationAcid-Base Equilibria
Acid-Base Equilibria 1. Classify each of the following species as an acid, a base, or amphoteric in aqueous solution: (a) H 2 O; (b) CH 3 CH 2 ; (c) PO 4 3 ; (d) C 6 H 5 NH 3 2. Write the proton transfer
More informationChapter 17. Additional Aspects of Aqueous Equilibria. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 17 Additional Aspects of James F. Kirby Quinnipiac University Hamden, CT Effect of Acetate on the Acetic Acid Equilibrium Acetic acid is a weak acid: CH 3 COOH(aq) H + (aq)
More informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationAqueous Equilibria: Part II- Solubility Product
Aqueous Equilibria: Part II- Solubility Product PSI AP Chemistry Name-------------------------- I Solubility Product, K sp MC #63-103 a) Writing K sp expression b) Solving for K sp c) Solving for (molar)
More informationAqueous Equilibria Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry
2012 Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry The Common-Ion Effect Consider a solution of acetic acid: HC 2 H 3 O 2 (aq) + H 2 O(l) H 3 O + (aq) + C 2 H 3 O 2 (aq) If
More informationAP Chemistry. 4. Which atom in its ground state has the most unpaired electrons? a. Ge b. As c. Se d. Br e. Ga
Name AP Chemistry Take Home Quiz Due Thursday, 1/9/2014 Bubble the correct answer on your scantron for each of the following. 1. Barium sulfate is LEAST soluble in a 0.01-molar solution of which of the
More informationTopic: Colligative Property O 3
PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - Meq. Approach SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market,
More informationAP Study Questions
ID: A AP 16.4-16.7 Study Questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1 What is the ph of an aqueous solution at 25.0 C in which [H + ] is 0.0025
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationAcids & Bases. Tuesday, April 23, MHR Chemistry 11, ch. 10
Acids & Bases 1 MHR Chemistry 11, ch. 10 Acid or base? 2 Make a chart like this: Strong v. Weak oncentrated v. Diluted 3 Acid Strength Acid strength depends on how much an acid dissociates. The more it
More informationProblems -- Chapter Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following.
Problems -- Chapter 1 1. Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following. (a) NaNO and HNO answers: see end of problem set (b)
More informationChapter 8: Applications of Aqueous Equilibria
Chapter 8: Applications of Aqueous Equilibria 8.1 Solutions of Acids or Bases Containing a Common Ion 8.2 Buffered Solutions 8.3 Exact Treatment of Buffered Solutions 8.4 Buffer Capacity 8.5 Titrations
More informationPHYSICAL CHEMISTRY By:- Shailendra kumar
PHYSICAL CHEMISTRY By:- Shailendra kumar H :- PP KHUDA BAKSH LIBRARY, ASHK RAJPATH, PATNA - 4 B: House No 5A/65, pp Mahual Kothi, Alpana Market, Patna CNFIDENCE BUILDING TEST - 1 1 Convert 05 M KMn 4 in
More informationChemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances
Chemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances 1. Identify each of the following as ionic or molecular substances: a) NaCl (aq)... b) CH 3 COOH (aq)... c) CCl 4(l)... d) HNO 3(aq)...
More informationChem 128, Exam III April 23, 2004
I. (35 points) A. (10 points) Consider an aqueous solution of PbI 2 with solid lead(ii) iodide present. K sp =8.4x10 9. 1. Write a balanced net ionic equation for the equilibrium established between the
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationAcids and Bases. Unit 10
Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts
More informationChem Practice Exam Two (Chapters 19, 20 and 21)
Chem 203 - Practice Exam Two (Chapters 19, 20 and 21) 1. Consider the dissolution of MnS in water (K sp = 3.0 10 14 ). MnS(s) + H 2O(l) Mn 2+ (aq) + HS (aq) + OH (aq) How is the solubility of manganese(ii)
More informationReaction Classes. Precipitation Reactions
Reaction Classes Precipitation: synthesis of an ionic solid a solid precipitate forms when aqueous solutions of certain ions are mixed AcidBase: proton transfer reactions acid donates a proton to a base,
More informationProblem Solving. ] Substitute this value into the equation for poh.
Skills Worksheet Problem Solving In 1909, Danish biochemist S. P. L Sørensen introduced a system in which acidity was expressed as the negative logarithm of the H concentration. In this way, the acidity
More informationChemistry. Approximate Timeline. Students are expected to keep up with class work when absent.
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 15 SOLUTIONS Day Plans for the day Assignment(s) for the day 1 Begin Chapter 15
More information2018 Version. Chemistry AS C3.6 Aqueous Systems
2018 Version Chemistry AS 91392 C3.6 Aqueous Systems Achievement Criteria - Solubility Demonstrate understanding of equilibrium principles in aqueous systems Aqueous systems are limited to those involving
More informationChapter 10. Acids, Bases, and Salts
Chapter 10 Acids, Bases, and Salts Topics we ll be looking at in this chapter Arrhenius theory of acids and bases Bronsted-Lowry acid-base theory Mono-, di- and tri-protic acids Strengths of acids and
More informationLecture 5. Percent Composition. etc. Professor Hicks General Chemistry II (CHE132) Percent Composition. (aka percent by mass) 100 g.
Lecture 5 Professor Hicks General Chemistry II (CHE132) Percent Composition (aka percent by mass) % by mass component 1 = mass component 1 mass sample 100% sample component 1 100 g sample component 1 component
More informationSolution Stoichiometry
Chapter 8 Solution Stoichiometry Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the
More information