Chemistry Study Guide

Chemistry Study Guide.
Unit 18 B Study Guide

Find the solubility (in mol/L) of lead(II) chloride (PbCl2) at 25oC. Ksp = 1. 62e–5.

A)1. 59e–2 B)2. 53e–2 C)6. 64e–17 D)2. 01e–3 E)2. 01e–2

The two salts AgX and AgY have very similar solubilities in water. It is known that the salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY 

A)Nothing. B)HY is stronger than HX. C)HX is stronger than HY. D)The acids have equal strengths. E)Cannot be determined.

Solubility Products (Ksp) BaSO41. 5   10-9 CoS5. 0   10-22 PbSO41. 3   10-8 AgBr5. 0   10-13 Which of the following compounds is the most soluble (in miles/liter) 

A)BaSO4 B)CoS C)PbSO4 D)AgBr E)BaCO3

How many moles of Fe(OH)2 [Ksp = 1. 8 10-15] will dissolve in 1. 0 liter of water buffered at pH = 11. 52 

A)1. 6e–10 B)3. 3e–3 C)1. 1e–5 D)6. 1e9 E)5. 4e–13

You have two salts, AgX and AgY, with very similar Ksp values. You know that Ka for HX is much greater than Ka for HY. Which salt is more soluble in acidic solution 

A)AgX B)AgY C)They are equally soluble in acidic solution. D)Cannot be determined by the information given. E)None of these (a-d).

You have a solution consisting of 0. 0 M Cl– and 0. 10 M CrO42–. You add 0. 10 M silver nitrate dropwise to this solution. Given that the Ksp for Ag2CrO4 is 9. 0   10–12, and that for AgCl is 1. 6   10–10, which of the following will precipitate first 

A)silver chloride B)silver chromate C)silver nitrate D)cannot be determined by the information given E)none of these

Which of the following compounds has the lowest solubility in mol/L in water 

A)Al(OH)3 Ksp = 2   10–32 B)CdS Ksp = 1. 0   10–28 C)PbSO4 Ksp = 1. 3   10–8 D)Sn(OH)2 Ksp = 3   10–27 E)MgC2O4 Ksp = 8. 6   10–5

The solubility of CaSO4 in pure water at 0oC is 1. 8 gram(s) per liter. The value of the solubility product is

A)1. 01e–2 B)1. 38e–3 C)1. 01e–1 D)1. 03e–4

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

A)greater than B)less than C)about the same as D)cannot be determined E)much different from

The molar solubility of PbI2 is 1. 47e–3 M. Calculate the value of Ksp for PbI2.

A)3. 18e–9 B)4. 32e–6 C)1. 27e–8 D)1. 47e–3 E)none of these

Calculate the concentration of chromate ion, , in a saturated solution of CaCrO4. (Ksp = 7. 08e–4)

A)2. 66e–2 M B)1. 42e–3 M C)7. 08e–4 M D)5. 01e–7 M E)3. 54e–4 M
Read this Practice Test Chem 105

Calculate the concentration of the silver ion in a saturated solution of silver chloride, AgCl (Ksp = 1. 63e–10).

A)1. 63e–10 B)1. 28e–5 C)2. 66e–20 D)3. 26e–10 E)none of these

The molar solubility of BaCO3 (Ksp = 1. 6   10–9) in 0. 10 M BaCl2 solution is:

A)1. 6   10–10 B)4. 0   10–5 C)7. 4   10–4 D)0. 10 E)none of these

It is observed that 7. 48 mmol of BaF2 will dissolve in 1. 0 L of water. Use these data to calculate the value of Ksp for barium fluoride.

A)1. 1e–4 B)4. 2e–7 C)1. 7e–6 D)2. 2e–4 E)5. 6e–5

The Ksp of AgI is 1. 5 10-16. Calculate the solubility in mol/L of AgI in a 0. 29 M NaI solution.

A)4. 4e–17B)0. 29 C)1. 5e-16 D)1. 2e–8 E)5. 2e–16

The molar solubility of AgCl (Ksp = 1. 6 10-10) in 0. 0013 M sodium chloride at 25oC is:

A)0. 0013 B)2. 1e–13 C)1. 2e–7 D)1. 6e-10 E)none of these

Silver chromate, Ag2CrO4, has a Ksp of 8. 95e–12. Calculate the solubility in mol/L of silver chromate.

A)1. 31e–4 M B)1. 65e–4 M C)2. 25e–12 M D)2. 08e–4 M E)1. 50e–6 M

The solubility in mol/L of Ag2CrO4 is 1. 2e–4 M. Calculate the Ksp for this compound.

A)2. 9e–8 B)1. 2e–4 C)6. 9e–12 D)1. 7e–12 E)2. 4e–4

Calculate the concentration of Al3+ in a saturated aqueous solution of Al(OH)3 (Ksp = 1. 8e–32).

A)6. 7e–9 B)1. 7e–34 C)1. e–8 D)6. 7e–34 E)5. 1e–9

The solubility in mol/L of M(OH)2 in 0. 016 M KOH is 1. 0 10-5 mol/L. What is the Ksp for M(OH)2 

A)2. 6e–9 B)1. 6e–7 C)2. 6e–4 D)4. 0e–15 E)1. 3e–6

The Ksp of PbSO4(s) is 1. 3 10-8. Calculate the solubility (in mol/L) of PbSO4(s) in a 0. 0085 M solution of Na2SO4.

A)1. 1e–10 M B)2. 3e–12 M C)1. 5e–6 M D)1. 3e-8 M E)1. 2e–3 M

The solubility of Cd(OH)2 in water is 1. 65e–5 mol/L. The Ksp value for Cd(OH)2 is:

A)1. 80e–14 B)4. 49e–15 C)5. 45e–10 D)1. 65e–5 E)none of these

The Ksp for PbF2 is 4. 0 10-8. If a 0. 056 M NaF solution is saturated with PbF2, what is the [Pb2+] in solution 

A)7. 1e–7 M B)1. 3e–10 M C)2. 3e–4 M D)1. 3e–5 M E)2. 2e–9 M

Chromate ion is added to a saturated solution of Ag2CrO4 to reach 0. 56 M . Calculate the final concentration of silver ion at equilibrium (Ksp for Ag2CrO4 is 9. 0 10-12).

A)2. 0e–6 M B)4. 0e–6 M C)5. 7e–6 M D)8. 0e–12 M E)2. 8e–6 M

The solubility of La(IO3)3 in a 0. 40 M KIO3 solution is 1. 0 10-7 mol/L. Calculate the Ksp for La(IO3)3.

A)6. 4e–2 B)4. 0e–8 C)6. 4e–9 D)6. 4e–23 E)none of these

In a solution prepared by adding excess PbI2(s) [Ksp = 1. 35e–8] to water, the [I-] at equilibrium is:

A)1. 50e–3 mol/L B)6. 75e–9 mol/L C)1. 16e–4 mol/L D)7. 9e–26 mol/L E)3. 00e–3 mol/L

Which of the following salts shows the lowest solubility in water  (Ksp values: Ag2S = 1. 6   10–49; Bi2S3 = 1. 0   10–72; HgS = 1. 6   10–54; Mg(OH)2 = 8. 9   10–12; MnS = 2. 3   10–13)

A)Bi2S3 B)Ag2S C)MnS D)HgS E)Mg(OH)2

The following question refers to the following: The solubility of silver phosphate (Ag3PO4) at 25oC is 1. 58e–5 mol/L. Determine the concentration of the Ag+ ion in a saturated solution.

A)1. 58e–5 M B)5. 27e–6 M C)4. 74e–5 M D)1. 90e5 M E)3. 94e–15 M

The following question refers to the following: The solubility of silver phosphate (Ag3PO4) at 25oC is 1. 3e–5 mol/L. What is the Ksp for the silver phosphate at 25oC 

A)1. 17e–13 B)1. 91e–18 C)7. 97e–10 D)7. 06e–20 E)none of these

Barium carbonate has a measured solubility of 4. 04e–5 at 25oC. Determine the Ksp.

A)4. 04e–5 B)8. 08e–5 C)6. 36e–3 D)2. 64e–13 E)1. 63e–9

A 300. 0-mL saturated solution of copper(II) peroidate (Cu(IO4)2) contains 0. 38 grams of dissolved salt. Determine the Ksp.

A)1. 6e–5 B)3. 2e–5 C)2. 8e–3 D)9. 2e–8 E)2. 5e–9

The correct mathematical expression for finding the molar solubility (S) of Sn(OH)2 is:

A)2S2 = Ksp B)2S3 = Ksp C)108S5 = Ksp D)4S3 = Ksp E)8S3 = Ksp

The in a saturated solution of Ce(IO3)3 is 5. 60e–3 M. Calculate the Ksp for Ce(IO3)3.

A)3. 28e–10 B)2. 95e–9 C)1. 76e–7 D)1. 87e–3 E)none of these

Calculate the solubility of Ag2CrO4 [Ksp = 9. 0e-12] in a 1. 3e–2 M AgNO3 solution.

A)6. 9e–10 mol/L B)3. 5e–10 mol/L C)5. 3e–8 mol/L D)2. 7e–8 mol/L E)none of these

The solubility of Mg(OH)2 (Ksp = 8. 9 10-12) in 1. 0 L of a solution buffered (with large capacity) at pH 9. 58 is:

A)1. 3e8 moles B)6. 2e–3 moles C)2. 3e–7 moles D)3. 8e–5 moles E)none of these

Calculate the solubility of Ca3(PO4)2(s) (Ksp = 1. 3e-32) in a 4. 6e–2 M Ca(NO3)2 solution.

A)5. 8e–15 mol/L B)1. 2e–14 mol/L C)2. 7e–16 mol/L D)3. 3e–29 mol/L E)none of these

Calculate the solubility of Cu(OH)2 in a solution buffered at pH = 7. 18. (Ksp = 1. 6 10-19)

A)1. 5e–7 M B)1. 1e–12 M C)7. 0e–6 M D)2. 3e–14 M E)none of these

Given the following Ksp values which statement about solubility in mol/L in water is correct  KspKsp PbCrO42. 0   10–16Pb(OH)21. 2   10–15 Zn(OH)24. 5   10–17MnS2. 3   10–13

A)PbCrO4, Zn(OH)2, and Pb(OH)2 have equal solubilities in water. B)PbCrO4 has the lowest solubility in water. C)The solubility of MnS in water will not be pH dependent. D)MnS has the highest molar solubility in water. E)A saturated PbCrO4 solution will have a higher [Pb2+] than a saturated Pb(OH)2 solution.

The concentration of OH- in a saturated solution of Mg(OH)2 is 3. 62e–4 M. The Ksp of Mg(OH)2 is

A)6. 6e–8 B)4. 7e–11 C)1. 3e–7 D)3. 6e–4 E)2. 4e–11

How many moles of CaF2 will dissolve in 3. 0 liters of 0. 049 M NaF solution  (Ksp for CaF2 = 4. 0 10-11)

A)1. 7e–8 B)2. 7e–10 C)5. 0e–8 D)5. 6e–9 E)none of these

Which of the following compounds has the lowest solubility in mol/L in water at 25°C 

A)Ag3PO4 Ksp = 1. 8   10–18 B)Sn(OH)2 Ksp = 5   10–26 C)CdS Ksp = 3. 6   10–29 D)CaSO4 Ksp = 6. 1   10–5 E)Al(OH)3 Ksp = 2   10–33

A 100. -mL sample of solution contains 10. 0 mmol of Ca2+ ion. How many mmol of solid Na2SO4 must be added in order to cause precipitation of 99. 9% of the calcium as CaSO4  The Ksp of CaSO4 is 6. 1   10–5. Assume the volume remains constant.

A)17. 4 B)10. 0 C)61. 0 D)71. 0 E)2. 00

The Ksp of Al(OH)3 is 2 10-32. At what pH will a 0. 8 M Al3+ solution begin to show precipitation of Al(OH)3  A)3. 5 B)10. 5 C)1. 0 D)6. 0 E)3. 0

Use the following to answer questions 44-47: The following questions refer to the following system: 3. 5   102 mL of 3. 2 M Pb(NO3)2 and 2. 0   102 mL of 0. 20 M NaCl are added together. Ksp for the lead chloride is 1. 6   10–5.

Determine the ion product. A)1. 1   10–4 B)1. 5   10–2 C)7. 8   10–3 D)8. 1   10–4 E)none of these 45. Will precipitation occur  A)Yes B)No C)Maybe, it depends on the temperature. D)Maybe, it depends on the limiting reagent concentration. E)None of these.
What is the limiting reagent in the formation of the lead chloride 

A)Pb2+ B)Cl– C)(NO3)– D)PbCl2 E)Pb(NO3)2 47. Determine the equilibrium concentration of the chloride ion. A)3. 9   10–4 B)8. 0   10–6 C)2. 8   10–3 D)6. 1   10–2 E)none of these

The Ksp for BaF2 is 2. 4   10–5.When 10 mL of 0. 01 M NaF is mixed with 10 mL of 0. 01 M BaNO3, will a precipitate form 

A)No, because Q is 1   10–12 and since it is less than Ksp no precipitate will form. B)Yes, because Q is 1   10–12 and since it is less than Ksp a precipitate will form. C)No, because Q is 1. 25   10–7 and since it is less than Ksp no precipitate will form. D)Yes, because Q is 1. 25   10–7 and since it is less than Ksp a precipitate will form. E)none of the above

How many moles of Ca(NO3)2 must be added to 1. 0 L of a 0. 586 M HF solution to begin precipitation of CaF2(s)  For CaF2, Ksp = 4. 0 10-11.

A)5. 8e–11 B)6. 8e–11 C)1. 4e–11 D)1. 2e–10 E)1. 1e–5

Which of the following solid salts is more soluble in 1. 0 M H+ than in pure water 

A)NaCl B)CaCO3 C)KCl D)AgCl E)KNO3

A solution contains 0. 018 moles each of I–, Br–, and Cl–. When the solution is mixed with 200 mL of 0. 24 M AgNO3, how much AgCl(s) precipitates out  KspAgI = 1. 5   10-16 KspAgBr= 5. 0   10-13 KspAgCl= 1. 6   10-10

A)0. 0 g B)1. 7 g C)2. 6 g D)3. 3 g E)5. 0 g

A 50. 0-mL sample of 0. 100 M Ca(NO3)2 is mixed with 50. 00 mL of 0. 200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold  The Ksp for CaF2 is 4.   10–11. Moles Solid CaF2[Ca2+] (M)[F–] (M) Formed

A)5. 0   10–33. 5   10–4 M7. 0   10–4 M B)5. 0   10–33. 4   10–9 M0. 05M C)5. 0   10–3 2. 2   10–4 M4. 3   10–4 M D)5. 0   10–33. 5   10–4 M 4. 3   10–4 M E)10. 0   10–31. 3   10–5 M 1. 3   10–5 M

Silver acetate (AgC2H3O2) is a sparingly soluble salt with Ksp = 1. 9   10–3. Consider a saturated solution in equilibrium with the solid salt. Compare the effects on the solubility of adding to the solution either the acid HNO3 or the base NH3.

A)Either substance would decrease the solubility. B)NH3 would increase the solubility, but HNO3 would decrease it C)NH3 would increase the solubility, but HNO3 would have virtually no effect. D)Either substance would increase the solubility. E)NH3 would decrease the solubility, but HNO3 would increase it.

The Ksp for Mn(OH)2 is 2. 0   10–13. At what pH will Mn(OH)2 begin to precipitate from a solution in which the initial concentration of Mn2+ is 0. 10 M 

A)6. 47 B)13. 3 C)5. 85 D)7. 03 E)8. 15

The concentration of Mg2+ in seawater is 0. 052 M. At what pH will 99% of the Mg2+ be precipitated as the hydroxide  (Ksp for Mg(OH)2 = 8. 9   10–12)

A)8. 35 B)9. 22 C)6. 50 D)10. 12 E)4. 86

Sodium chloride is added slowly to a solution that is 0. 010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1. 9   10–7, 1. 6   10–10, and 2. 0   10–13, respectively. Which compound will precipitate first 

A)CuCl(s) B)AgCl(s) C)AuCl(s) D)All will precipitate at the same time. E)Cannot be determined.

A 0. 012-mol sample of Na2SO4 is added to 400 mL of each of two solutions. One solution contains 1. 5   10–3 M BaCl2; the other contains 1. 5   10–3 M CaCl2. Given that Ksp for BaSO4 = 1. 5   10–9 and Ksp for CaSO4 = 6. 1   10–5:

A)BaSO4 would precipitate but CaSO4 would not. B)CaSO4 would precipitate but BaSO4 would not. C)Both BaSO4 and CaSO4 would precipitate. D)Neither BaSO4 nor CaSO4 would precipitate. E)Not enough information is given to determine if precipitation would occur.

Which of the following solid salts is more soluble in 1. 0 M H+ than in pure water 

A)NaCl B)KCl C)FePO4 D)AgCl E)KNO3

Which of the following solid salts should be more soluble in 1. 0 M NH3 than in water 

A)Na2CO3 B)KCl C)AgBr D)KNO3 E)none of these

The overall Kf for the complex ion Ag(NH3)2+ is 1. 7    The Ksp for AgI is 1. 5   10–16. What is the molar solubility of AgI in a solution that is 2. M in NH3 

A)1. 5   10–9 B)1. 3   10–3 C)1. 0   10–4 D)5. 8   10–12 E)8. 4   10–5 61.

If 30 mL of 5. 0   10–4 M Ca(NO3)2 are added to 70 mL of 2. 0   10–4 M NaF, will a precipitate occur  (Ksp of CaF2 = 4. 0   10–11)

A)No, because the ion product is greater than Ksp. B)Yes, because the ion product is less than Ksp. C)No, because the ion product is less than Ksp. D)Not enough information is given. E)Yes, because the ion product is greater than Ksp.

Given the following values of equilibrium constants: 1. 64e–19 What is the value of the equilibrium constant for the reaction:

A)1. 64e–19 B)1. 6e–32 C)1. e–6 D)6. 10e18 E)1. 0e13 Use the following to answer questions 63-65: A 50. 0-mL sample of 2. 0   10–4 M CuNO3 is added to 50. 0 mL of 4. 0 M NaCN. Cu+ reacts with CN– to form the complex ion Cu(CN)32–: Cu(CN)32– Cu+ + 3CN–

The concentration of CN– at equilibrium is

A)4. 0 M B)2. 0 M C)1. 0 M D)6. 0   10–4 M E)none of these

The concentration of Cu+ at equilibrium is

A)2. 0   10–4 M B)1. 0   10–4 M C)1. 2   10–14 M D)5. 0   10–14 M E)none of these

Calculate the solubility of CuBr(s) (Ksp = 1. 0   10–5) in 1. 0 L of 1. 0 M NaCN.
A)1. 0 mol/L B)1. 0   10–6 mol/L C)0. 33 mol/L D)1. 0   103 mol/L

E)none of these Use the following to answer questions
66-67: Consider a solution made by mixing 500. 0 mL of 4. 0 M NH3 and 500. 0 mL of 0. 40 M AgNO3. Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+: Ag+ + NH3 AgNH3+K1 = 2. 1   103 AgNH3+ + NH3 Ag(NH3)2+K2 = 8. 2   103

The concentration of Ag(NH3)2+ at equilibrium is:

A)2. 0 M B)0. 40 M C)0. 20 M D)1. 0   10–3 M E)none of these

The concentration of Ag+ at equilibrium is:

A)2. 0 M B)1. 2   10–8 M C)4. 5   10–9 M D)1. 6 M E)none of these
Use the following to answer questions 68-71: The following questions refer to the following system: 500. 0 mL of 0. 20 M Mn(NO3)2 are mixed with 1. 0 L of 1. 0 M Na2C2O4. The oxalate ion, C2O4, acts as a ligand to form a complex ion with the Mn2+ ion with a coordination number of two. Mn2+ + C2O42– MnC2O4K1 = 7. 9   103 [Mn(C2O4)2]2– MnC2O4 + C2O42–K2 = 1. 26   10–2

What is the equilibrium constant for the following formation: Mn2+ + 2C2O42– [Mn(C2O4)2]2–

A)1. 0 B)3. 7   102 C)2. 1   10–1 D)6. 3   105 E)none of these

Find the equilibrium concentration of the [Mn(C2O4)2]2– ion.

A)9. 2   10–5 M B)0. 01 M C)2. 5   10–8 D)1. 3   10–4 E)6. 7   10–3

Find the equilibrium concentration of the Mn(C2O4) ion.

A)9. 2   10–5 M B)0. 1 M C)2. 5   10–8 D)1. 3   10–4 E)6. 7   10–3

Find the equilibrium concentration of the Mn2+ ion.

A)9. 2   10–5 M B)0. 01 M C)2. 5   10–8 D)1. 3   10–4 E)6. 7   10–3

Calculate the molar concentration of uncomplexed Zn2+ in a solution that contains 0. 20 mole of Zn(NH3)42+ per liter and 0. 0116 M NH3 at equilibrium  The overall Kf for Zn(NH3)42+ is 3. 8   109.

A)2. 9   10–3 M B)8. 8   10–3 M C)6. 7   10–4 M D)2. 0   10–13 M E)none of these

The cation M2+ reacts with NH3 to form a series of complex ions as follows: M2+ + NH3 M(NH3)2+K1 = 102 M(NH3)2+ + NH3 M(NH3)22+K2 = 103 M(NH3)22+ + NH3 M(NH3)32+K3 = 102

A 1. 0   10–3 mol sample of M(NO3)2 is added to 1. 0 L of 15. 0 M NH3 (Kb = 1. 8   10–5). Choose the dominant species in this solution A)M2+ B)M(NH3)2+ C)M(NH3)22+ D)M(NH3)32+ 74.

The Kf for the complex ion Ag(NH3)2+ is 1. 7    The Ksp for AgCl is 1. 6   10–10. Calculate the molar solubility of AgCl in 1. 0 M NH3.

A)5. 2   10–2 B)4. 7   10–2 C)2. 9   10–3 D)1. 3   10–5 E)1. 7   10–10

The two salts AgX and AgY exhibit very similar solubilities in water. It is known that the salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY 

A)Nothing. B)HY is stronger than HX. C)HX is stronger than HY. D)The acids are weak acids and have equal values for Ka. E)Both acids are strong.
Answer Key 1. A 2. B 3. C 4. A 5. B 6. A 7. B 8. D 9. C 10. C 11. A 12. B 13. E 14. C 15. E 16. C 17. A 18. C 19. E 20. A 21. C 22. A 23. D 24. B 25. C 26. E 27. D 28. C 29. B 30. E 31. D 32. D 33. A 34. C 35. B 36. A 37. C 38. B 39. E 40. C 41. C 42. D 43. A 44. A 45. A 46. B 47. C 48. C 49. D 50. B 51. B 52. C 53. D 54. E 55. D 56. C 57. A 58. C 59. C 60. C 61. C 62. C 63. B 64. C 65. C 66. C 67. C 68. D 69. E 70. D 71. C 72. A 73. D 74. B 75. B

Chemistry Study Guide

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