R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 1 / 7 Chemistry 1 Provincial Exam Workbook Unit 0: Solubility Equilibrium Multiple Choice Questions 1. Which of the following would be true when equal volumes of 0. M NaBr and 0. M AgNO are combined? A. No precipitate forms B. A precipitate of AgBr forms C. A precipitate of NaNO forms D. Precipitates of both NaNO and AgBr form. Using the solubility table, determine which of the following ions could not be used to separate S from SO by precipitation? A. Be B. Ca C. Ba D. Sr. Which of the following is true when solid NaS is added to a saturated solution of CuS and equilibrium is re-established? A. B. C. D. S increases Cu increases S does not change Cu does not change
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P / 7. Which of the following describes the relationship between the solubility product constant K and the solubility s of PbI? A. B. C. K =s K =s K s= D. s= K 5. Which of the following saturated solutions will have the lowest S? A. BaS B. CaS C. CuS D. ZnS 6. What is the solubility of SrF? 5 A..x10 M 17 B. 1.8x10 M 9 C..x10 M D. 1.0x10 M 7. Which of the following is a suitable term for representing solubility? A. grams B. moles C. molarity D. millilitres per second
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P / 7 8. A saturated solution is prepared by dissolving a salt in water. Which of the following graphs could represent the ion concentrations as the temperature is changed? 9. What is the concentration of OH ions in 50 ml of 0.0 M Sr OH? A. 0.050 M B. 0.10 M C. 0.0 M D. 0.0 M 10. What happens when 10.0 ml of 0. M KOH is added to 10.0 ml of 0. M CuSO? A. No precipitate forms B. A precipitate of KSO forms C. A precipitate of CuOH forms D. Precipitates of KSO and CuOH form
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P / 7 11. Consider the following equilibrium CaSO (s) Ca (aq) SO (aq) A. adding CaSO (s) B. adding MgSO (s) C. removing some Ca D. removing some Which of the following would shift the above equilibrium to the left? SO (aq) (aq) 1. Calculate the solubility of CaCO. 9 A..x10 M 5 B. 1.x10 M 5 C..8x10 M D. 8.x10 M 1. How many moles of dissolved solute are present in 100.0 ml of a saturated SrCO solution? A. B. C. D. 11 5.6x10 mol 6.x10 mol 5.x10 mol.x10 mol 1. What happens when equal volumes of 0. M AgNO and 0. M NaCl are combined? A. A precipitate forms because the trial ion product > K B. A precipitate forms because the trial ion product < K C. No precipitate forms because the trial ion product > K D. No precipitate forms because the trial ion product < K 15. Determine the maximum NaCO that can exist in 1.0 L of 0.0010M BaNO without forming a precipitate. A. B. C. D. 1.6x10 M 9.6x10 M 6.6x10 M 5.6x10 M
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 5 / 7 16. Solid BaOH is added to water to prepare a saturated solution. Which of the following is true for this equilibrium system? A. anion cation B. trial K is less than K C. blue litmus paper would turn red D. the rate of dissolving = the rate of crystallization 17. A saturated solution of PbI was subjected to a stress and the following graph was obtained. A. the addition of PbI B. a temperature change C. an increase in volume D. the evaporation of water Which stress was applied at time t 1? 18. A solution is prepared containing both 0. M OH and 0. M A. 0. M Cs B. 0. M Zn C. 0. M Pb D. 0. M Sr PO ions. An equal volume of a second solution is added in order to precipitate only one of these two anions. The second solution must contain which of the following?
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 6 / 7 19. Consider the following equilibrium A. left and B. left and C. right and D. right and When CaNO S S S S increases decreases increases decreases 0. How many moles of CaS(s) Ca (aq) S (aq) (aq) is added to this solution, the equilibrium shifts to the Pb are there in 500.0 ml of a saturated solution of PbSO? A. B. C. D..x10 16 9.0x10 9 6.7x10 5 1.x10 1. Which of the following compounds is least soluble in water? A. CuI B. BeS C. CsOH D. AgBrO. Which of the following will dissolve to form a molecular solution? A. HSO B. AgNO C. CaOH D. C6H1 O 6
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 7 / 7. Consider the following equilibrium A. heat B. HCl C. AgNO D. a catalyst energy AgCl(s) Ag (aq) Cl (aq) Addition of which of the following will increase the solubility of AgCl?. What is the Cl ml of solution? when 15.0 g of NaCl is dissolved in enough water to make 100.0 A. 0.150 M B. 0.90 M C..56 M D..90 M 5. An equal number of moles of NaCO is added to four different 10.0 ml samples. A precipitate forms in only one of the samples. Identify the cation which is present in the precipitate. A. Ba B. Ca C. Mg D. Sr 6. What is the net ionic equation for the reaction between BaS(aq) and Sr OH (aq)? A. Sr (aq) S (aq) SrS(s) B. Ba (aq) OH (aq) BaOH (s) C. D. Ba (aq) S (aq) Sr (aq) OH (aq) Ba OH (s) SrS(s) - Ba (aq) S (aq) Sr (aq) OH (aq) Ba OH (s) Sr (aq) S (aq)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 8 / 7 7. In which of the following would PbCl (s) be least soluble? A. 1 M HCl B. 1 M BaCl C. 1 M KSO D. 1 M PbNO 8. The solubility of ZnCO is 9 6.x10 M. What is the value of K for ZnCO? A. B. C. D..1x10 17 6.x10 9 1.x10 8 8.0x10 5 9. What is the A. 5.0x10 B. 1.x10 C..5x10 D. 5.0x10-1 -1-9 -5 K for the salt Pb IO if its solubility is -5 5.0x10 M? 0. What is the maximum IO 6.9x10 M - that can exist in a - + Cu solution? -6 A..0x10 M -6 B. 1.0x10 M - C. 1.0x10 M - D. 6.9x10 M 1. Which of the following will form a saturated solution? A. 0.10 mol CaSO added to 1.0 L of water B. 0.10 mol CsSO added to 1.0 L of water C. 0.0 mol MgSO added to.0 L of water D. 0.50 mol PbNO added to.0 L of water
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 9 / 7. Which of the following would be an appropriate measure of solubility? A. moles of solute per volume of solute B. mass of solute per volume of solution C. volume of solvent per mass of solvent D. moles of solute at a ecific temperature. What is the complete ionic equation for the precipitation reaction between MgS(aq) and Sr OH (aq)? + A. Mg (aq)+oh(aq) MgOH (s) B. MgS(aq)+Sr OH (aq) SrS(aq)+Mg OH (s) + - + + - C. Mg (aq)+s (aq)+sr (aq)+oh (aq) SrS(s)+Mg (aq)+oh (aq) + - + + - D. Mg (aq)+s (aq)+sr (aq)+oh (aq) Sr (aq)+s (aq)+mg OH (s). What is the K expression for the low solubility salt formed when KSO (aq) and AlCl (aq) are mixed? - A. K = SO + - B. K = K Cl + - C. K = Al SO + - D. K = Al SO 5. Which compound has the lowest solubility? A. ZnS B. CuS C. AgCl D. SrSO 6. What is the solubility of the salt PbCl? - A. 1.x10 M - B..x10 M - C..5x10 M -5 D. 1.x10 M
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 10 / 7 7. A solution is found to contain a Pb can exist in this solution before a precipitate forms? SO + of 0.10 M. What is the maximum - that A. B. C. D. SO SO SO SO =1.8x10 M =1.8x10 M =1.8x10 M =1.x10 M - -9 - -8 - -7 - - 8. Which solute will result in a molecular solution? A. HCN B. BaOH C. CH COOH D. CHCH OH 9. Which best describes the equilibrium in a saturated solution? A. The rate of crystallization determines the solubility. B. The rate of crystallization equals the rate of dissolving. C. There is no solid solute on the bottom of the container. D. The solute is completely dissolved and the equilibrium favours the products. 0. Which compound will have a solubility greater than 0.1 M at 5 C? A. SrS B. CoS C. BaSO D. AgSO 1. What is the net ionic equation for the reaction between 0.10 M NaS and 0.10 M A. Zn NO? = - Zn (aq)+s (aq) ZnS(s) + - B. Na (aq)+no (aq) NaNO (s) C. D. Na S(aq)+Zn NO (aq) ZnS(s)+NaNO (aq) + - + - + - Na (aq)+s (aq)+zn (aq)+no (aq) ZnS(s)+Na (aq)+no (aq)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 11 / 7. When equal volumes of 0.0 M NaOH and 0.0 M CaS are mixed together A. a precipitate forms and the trial K would be less than K B. no precipitate forms and the trial K would be less than K C. a precipitate forms and the trial K would be greater than K D. no precipitate forms and the trial K would be greater than K. Which of the following solutes will produce a molecular solution? A. HCl B. FeS C. HNO D. CHOH. Which of the following would best describe the solubility of a solute? A. litres per gram B. moles per litre C. grams per mole D. moles per second 5. Which compound will have the lowest solubility? A. FeS B. CaSO C. AgBrO D. FeNO 6. Which of the following precipitates may form when equal volumes of 0. M AgNO, 0. M SrCl and 0. M NaCO are mixed together? A. SrCO and AgCl B. AgCO and AgCl C. SrCO and AgCO D. SrCO, AgCO and AgCl
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 1 / 7 7. An experiment is conducted to identify an unknown cation that is present in each of four beakers. A. Ag B. Fe C. Ba D. Be 8. Given the equilibrium reaction Which A. K Ag S 1 B. K Ag S C. K D. K Ag S AgS AgNO NaS NaNO Which of the following could be the unknown cation? NaNO (aq) AgS(s) AgNO (aq) NaS(aq) K expression best describes the net ionic reaction?
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 1 / 7 9. Two salt solutions were mixed and a trial K was calculated to be value is 9.0x10. The K 10 1.0x10. From this information, which of the following is a true statement? 50. A saturated solution of SrSO has an SO 1.0x10 M of. What is the Sr? A. B. C. D..x10 M 5.8x10 M 1.0x10 M 7.x10 M 51. Which of the following would form a saturated solution when 0.010 mol of the solid solute is added to 100 ml of water? A. BaCO B. FeSO C. NaCN Pb NO D. 5. Which net ionic equation best describes the reaction that exists in a solution prepared Ca NO and 0.0 M NaCO? A. by mixing equal volumes of 0.0 M Ca (aq) CO (aq) CaCO (s) B. Na (aq) NO (aq) NaNO (s) C. D. Ca NO (aq) Na CO (aq) NaNO (s) CaCO (s) Ca NO (aq) Na CO (aq) NaNO (aq) CaCO (s)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 1 / 7 5. Which compound will have the greatest solubility in water? A. CuCl B. FeCO C. MgSO D. CuPO 5. Which cation below can be used to separate A. Sr B. Pb C. Cs D. Be SO from S ions by precipitation? 55. What will be the effect of adding some solid AgNO to a saturated solution of AgCl? A. The AgNO will not dissolve B. More solid AgCl will dissolve C. More solid AgCl will be produced D. The AgNO will not affect the AgCl equilibrium 56. For a saturated solution, the K expression does not contain any solid solute term. What is the reason for this? A. The solid solute is a product B. The solid solute is a reactant C. The solid solute continues to change in amount D. The solid solute does not change in concentration 57. Which of the statements below describes the K expression for the salt barium phohate? A. K Ba PO B. K Ba PO C. K Ba PO D. K Ba PO
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 15 / 7 58. What is the solubility of FeOH? 17 A..9x10 M 17 B. 1.x10 M 6 C..7x10 M 6 D..x10 M 59. Which of the following ions would have the highest concentration in 0.1 M A. Ba B. Ca C. Sr D. Mg CO? 60. Which of the solutes below can form an ionic solution with the highest conductivity? A. PbS B. CHCl C. NaNO D. CH COOH 61. The following data was collected to determine the solubility of a substance A..00x10 g/ml B. 5.00x10 mol C. 0.50 mol D. 1.00 mol/l Mass of solute dissolved 5.00 g Volume of solvent 50.0 ml Molar mass of solute 100.0 g/mol Molar mass of solvent 0.0 g/mol Which of the following best describes its solubility?
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 16 / 7 6. Which value best represents the total ion concentration when 0.10 moles of KPO is present in 0.5 L of solution? A. 0.1 M B. 0. M C. 0. M D. 0.8 M 6. What will happen when equal volumes of 0.0 M NH S and 0.0 M Sr OH are mixed? A. SrS precipitates B. NHOH precipitates C. Both NHOHand SrS precipitate D. No precipitate forms 6. Which anion would be most effective in removing the cations reonsible for hard water? A. B. Cl C. D. S PO SO 65. Which of the following is the K expression for barium phohate? A. K Ba PO B. K Ba PO C. K Ba PO D. K Ba PO 66. The solubility of MgOH is found to be A. 6.9x10 1 B. 1.7x10 1 C. 1.x10 8 D. 1.x10 1.x10 M. What is its K?
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 17 / 7 67. Which of the following is true for the salt SrF at 5 C? A. It has a high solubility B. It will not dissolve at all C. Its solubility is 1.6x10 M D. Its solubility is 1.0x10 M 68. Which of the following ions could be used in the lowest concentration to remove Ag ions from a polluted water sample? A. I B. Br C. BrO D. CO 69. Which of the solutes below is both ionic and most soluble? A. RbOH B. CHOH C. CaOH D. FeOH 70. Which of the following is commonly used to describe the solubility of a solute? A. mass of solute moles of solute B. moles of solution mass of solute C. mass of solute volume of solution D. mass of solution volume of solute 71. Given a saturated solution of CaOH which of the following statements is always true? A. The Ca is twice that of OH B. The OH precipitates half as fast as the Ca C. The rate of crystallization equals the rate of dissolving D. The rate of dissolving is greater than the rate of crystallization
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 18 / 7 7. Solid NaCl is added to a saturated AgCl solution. How have the Ag changed when equilibrium has been re-established? and Cl 7. Which of the following expressions represents solution? Fe in a saturated FeOH K A. OH K B. OH C. D. K K OH OH 7. What is the value of K for ZnOH if the solubility of ZnOH is equal to A. 1.0x10 B..0x10 C. 1.8x10 11 D..0x10 16 6.x10 M? 75. What is the maximum number of moles of Cl that can exist in 500.0 ml of.0 M AgNO? A..5x10 11 B. 9.0x10 11 C. 1.8x10 10 D. 1.8x10 9
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 19 / 7 76. What is the concentration of the ions in.0 L of 0.50 M AlSO? 77. Consider the following equilibrium MgCO (s) Mg (aq) CO (aq) A. HCl B. KCO C. MgCO D. MgNO Adding which of the following would cause the solid to dissolve? 78. Which of the following compounds could be used to prepare a solution with a greater than 0.1 M? S A. ZnS B. PbS C. AgS D. RbS 79. Which of the following will not form a precipitate when mixed with an equal volume of 0. M AgNO? A. 0. M NaBr B. 0. M NaIO C. 0. M NaNO D. 0. M NaBrO
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 0 / 7 80. How many moles of solute are dissolved in 00.0 ml of a saturated solution of FeS? A. 1.x10 19 B. 6.0x10 19 C. 1.5x10 10 D. 7.7x10 10 81. Consider the following 10.0 ml solutions Equal moles of AgNO are added to each solution. It is observed that a precipitate forms in all but one solution. Which solution does not form a precipitate? A. Cl B. Br C. IO D. BrO 8. Which of the following could dissolve a precipitate of CaCO in a saturated solution A. NaOH B. CaCO C. HCO D. CaNO of CaCO?
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 1 / 7 8. Which of the following will dissolve in water to produce a molecular solution? A. CaCl B. NaOH C. CHOH D. Sr OH 8. In a solubility equilibrium, the A. rate of dissolving equals the rate of crystallization B. neither dissolving nor crystallization are occurring C. concentration of solute and solvent are always equal D. mass of dissolved solute is greater than the mass of the solution 85. Which of the following solutions would have Fe 0.00M? A. 0.0 L of 0.050 M FeNO B. 0.80 L of 0.00 M FeSO C. 0.50 L of 0.00 M FeC6H5 O 7 D. 0.50 L of 0.010 M Fe CO 86. Which of the following substances has the lowest solubility? A. BaS B. CuS C. FeS D. ZnS 87. The complete ionic equation for the reaction between MgS and Sr OH is A. MgS(aq) Sr(OH) (aq) Mg(OH) (s) SrS(s) B. MgS(aq) Sr(OH) (aq) Mg(OH) (s) SrS(aq) C. Mg (aq) S (aq) Sr (aq) OH Mg (aq) OH (aq) SrS(s) D. Mg (aq) S (aq) Sr (aq) OH Mg OH (s) Sr (aq) S (aq) -
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P / 7 88. Consider the following equilibrium A. adding KOH B. adding NaS C. adding FeOH D. adding FeNO Fe OH (s) Fe (aq) OH (aq) Which of the following will cause the equilibrium to shift to the right? 89. Consider the following experiment A. 0.0 M OH B. 0.0 M NO C. 0.0 M D. 0.0 M PO SO 90. A compound has a solubility of A. CuS B. AgBr C. CaCO D. CaSO The unknown solution could contain 5 7.1x10 M at o 5 C. The compound is
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P / 7 91. A saturated solution of NaCl contains 6.5 g of solute in 0.100 L of solution. The solubility of the compound is A. 0.06 M B. 1.60 M C..65 M D. 6. M 9. Calculate the Li in 00.0 ml of 1.5 M LiSO A. 0.0 M B. 0.60 M C. 1.5 M D..0 M 9. When equal volumes of 0.0 M RbCl and 0.0 M SrS are combined A. no precipitate forms B. a precipitate of RbS only forms C. a precipitate of SrCl only forms D. precipitates of both RbS and SrCl form 9. A solution contains both Ag and Mg are removed one at a time by adding ions. During selective precipitation, these ions A. I followed by OH B. OH followed by S C. SO followed by Cl D. NO followed by PO 95. The K expression for a saturated solution of MgOH is A. K Mg OH MgOH B. K Mg OH C. K Mg OH D. K Mg OH
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P / 7 96. Consider the following saturated solutions: CuSO, BaSO, CaSO. The order of cation concentration, from highest to lowest, is A. B. C. D. Ba Ca Cu Ca Cu Ba Cu Ca Ba Cu Ba Ca 97. When 1.0x10 moles A. Trial K K and a precipitate forms B. Trial K K and a precipitate forms C. Trial K K and no precipitate forms D. Trial K K and no precipitate forms of CuCl (s) are added to 1.0 L of 98. Which of the following forms a molecular solution in water? A. SrSO B. NaPO C. C6H1 O 6 D. NHCH COO 1.0x10 M IO, the 99. Which of the following is necessary to form a saturated solution at equilibrium? A. excess solute B. an ionic solute C. solute of low solubility D. trial ion product is less than K 100. Which of the following will produce a solution with the highest OH? A. AgOH B. Sr OH C. FeOH D. MgOH
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 5 / 7 Written Questions 1. A 0.00 ml sample of a saturated solution of AgSO was heated in an evaporating dish until all the water was evaporated. The following data were recorded... Calculate the K value for AgSO. (5 marks). Consider the following equilibrium and accompanying graph... + - Zn IO (s) Zn (aq)+io (aq) A. Identify the stress applied at t 1. (1 mark) Complete the above graph from t 1 to t for the - IO. ( marks)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 6 / 7. Calculate the solubility of SrSO in grams per litre. ( marks). A 100.0 ml saturated solution of FeF contains 0.0787 g of solute. Determine the Fe + and the - F in the solution. ( marks) 5. Consider the following information and the accompanying diagram. In a titration - experiment, AgNO (aq) was used to determine the Cl in a water sample and the following data were recorded... + - Ag (aq)+cl (aq) AgCl(s) AgNO 0.15 M Volume of water sample containing Initial buret reading of AgNO Final buret reading of AgNO - Cl 0.00 ml 5.15 ml 7.15 ml Using the above data, determine the - Cl in the water sample. ( marks) 6. Calculate the mass of NaI necessary to begin precipitation of sample of 0.010 M CuNO. ( marks) + Cu from a 50.0 ml 7. A. Write the net ionic equation for the reaction between PbNO and NaCl. ( marks)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 7 / 7 B. Determine, with calculations, whether a precipitate will form when 15.0 ml of 0.050 M Pb NO is added to 5.0 ml of 0.085 M NaCl. ( marks) 8. After a 50.0 ml sample of a saturated solution of AgSO was heated to dryness, - 7.x10 g of solid AgSO remained. What is the value of marks) K for AgSO? (5 9. Calculate the maximum mass of BaCl (s) that can be added to 50 ml of 0.50 M PbNO (aq) without forming a precipitate of PbCl (s). (6 marks) 10. Sufficient Na SO is added to 0.10 M Ba NO to cause a precipitate to form. A. Write the net ionic equation for the precipitate formation. (1 mark) B. Calculate the SO - at the moment the precipitate starts to form. ( marks) 11. Calculate the mass of solid AgNO that can be added to.0 L of a 0.10 M K CrO solution in order to just start precipitation. ( marks)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 8 / 7 1. A. How would a saturated solution be prepared at room temperature? (1 mark) B. Write a chemical equation to illustrate the equilibrium that exists in a saturated solution of Be PO. ( marks) 1. Calculate the iodate ion concentration in a saturated copper (II) iodate solution at 5C. ( marks) 1. A solution is prepared by mixing equal moles of BaNO, K SO, and BaS and precipitation occurs. Identify the precipitate(s) and write the net ionic equation Precipitate (1 mark) Net Ionic Equation ( marks) + 15. What is the maximum Pb that can exist in a saturated solution of BaSO without causing precipitate formation? ( marks)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 9 / 7 16. Consider the equilibrium for a saturated solution of CaCO... CaCO (s) Ca +CO + - + What is the maximum Mg that can exist in a saturated solution of CaCO without causing a precipitate to form? ( marks) 17. Consider the equilibrium for a saturated solution of PbI (s)... PbI (s) + - Pb (aq)+i (aq) + What is the maximum Ag that can exist in a saturated solution of PbI (s) without causing a precipitate to form? ( marks)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 0 / 7 18. Consider the following equilibrium... + - Mg OH (s) Mg (aq)+oh (aq) A. What happens to the amount of solid MgOH (s) when some HCl(aq) is added? (1 mark) B. On the graph below, sketch the effect of adding HCl(aq) at time t 1. ( marks) 19. Will a precipitate form when 10.0 ml of 1.0 M PbNO is mixed with 0.0 ml of -.0x10 M NaCl? Justify your answer. ( marks) 0. At 5 C, will a precipitate form when 5.0 ml of 0.010 M Pb NO is combined with 75.0 ml of 0.010 M NaI? Support your answer with calculations. ( marks)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 1 / 7 1. Write the complete ionic equation for the reaction between NaBrO and AgNO. (1 mark) A. Complete Ionic Equation B. What is the maximum NaBrO that can exist in equilibrium with.0 M AgNO? ( marks). Write the balanced complete ionic equation for the reaction that occurs when 0.0 M Ba NO is added to an equal volume of 0.0 M NaCO. ( marks) of Complete Ionic Equation. Calculate the minimum number of moles of PbNO required to start precipitation in 50.0 ml of 0.15 M ZnI. (5 marks). In a titration, 5.00 ml of NaCl(aq) reacts completely with.0 ml of 0.100 M AgNO. What is the Cl in the original solution? ( marks)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P / 7 5. The following data was obtained when 0.0 ml of a saturated solution of PbI was evaporated to dryness. Use this information to determine the K of PbI. ( marks) 6. Calculate the molar solubility of SrF. ( marks)
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P / 7 Multiple Choice Questions Answer Key 1 B 1 A 1 A 61 A 81 D A D C 6 D 8 A A A D 6 D 8 C B C B 6 C 8 A 5 C 5 D 5 A 65 B 85 D 6 D 6 B 6 D 66 A 86 B 7 C 7 B 7 B 67 D 87 D 8 D 8 A 8 A 68 A 88 B 9 D 9 A 9 B 69 A 89 A 10 C 0 C 50 A 70 C 90 C 11 B 1 A 51 A 71 C 91 D 1 C B 5 A 7 B 9 D 1 B D 5 C 7 B 9 A 1 A C 5 A 7 D 9 A 15 C 5 B 55 C 75 A 95 B 16 D 6 A 56 D 76 B 96 C 17 B 7 C 57 B 77 A 97 D 18 D 8 D 58 D 78 D 98 C 19 B 9 B 59 D 79 C 99 A 0 C 0 A 60 C 80 C 100 B
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R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P / 7 19. 0.
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R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 7 / 7 5. 6.