Methylamine, CH3NH2, is a weak molecular base with a value of 4.4 × 10-4 for Kb. An aqueous solution contains 0.200 M CH3NH2 and 0.400 M CH3NH3Cl per liter as the only solutes. If the Ksp of Mg(OH)2 is 7.1 × 10-12, what is the maximum [Mg2+] that can coexist with these solutes in the solution?Hint: Use the Henderson-Hasselbalch formula to find the pOH of the solution, and then use that to find [OH-].

A) 8.1 × 10-9 B) 3.2 × 10-8 C) 9.2 × 10-6 D) 1.5 × 10-4 E) 3.7 × 10-1 A) 8.1 × 10-9 B) 3.2 × 10-8 C) 9.2 × 10-6 D) 1.5 × 10-4 E) 3.7 × 10-1

The solubility of magnesium carbonate, MgCO3, in pure water is 2.6 × 10-4 moles per liter. Calculate the value of Ksp for magnesium carbonate from this data.

A) 5.2 × 10-4 B) 6.8 × 10-8 C) 1.4 × 10-7 D) 2.7 × 10-7 E) 4.6 × 10-15 A) 5.2 × 10-4 B) 6.8 × 10-8 C) 1.4 × 10-7 D) 2.7 × 10-7 E) 4.6 × 10-15

Will a precipitate form when 20.0 mL of 1.8 × 10-3 M Pb(NO3)2 is added to 30.0 mL of5.0 × 10-4 M Na2SO4? The Ksp of (PbSO4)is 6.3 × 10-7.Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

A) no, because the ion product, Q sp B) no, because the ion product, Q > Ksp C) yes, because the ion product, Q sp D) yes, because the ion product, Q > Ksp E) no, because Ksp is less than the ion product A) no, because the ion product, Q sp B) no, because the ion product, Q > Ksp C) yes, because the ion product, Q sp D) yes, because the ion product, Q > Ksp E) no, because Ksp is less than the ion product

Methylamine, CH3NH2, is a weak molecular base with a value of 4.4 × 10-4 for Kb. An aqueous solution contains 0.200 M CH3NH2 and 0.300 M CH3NH3Cl per liter as the only solutes. If the Ksp of Fe(OH)2 is 7.9 × 10-16, what is the maximum [Fe2+] that can coexist with these solutes in the solution?Hint: Use the Henderson-Hasselbalch formula to find the pOH of the solution, and then use that to find [OH-].

A) 1.8 × 10-12 B) 9.0 × 10-12 C) 1.8 × 10-9 D) 9.2 × 10-9 E) 9.2 × 10-6 A) 1.8 × 10-12 B) 9.0 × 10-12 C) 1.8 × 10-9 D) 9.2 × 10-9 E) 9.2 × 10-6

The solubility product for Ag3PO4 is: Ksp = 2.8 × 10-18. What is the solubility of Ag3PO4 in water, in grams per liter?

A) 1.2 × 10-15 g/L B) 7.5 × 10-3 g/L C) 2.0 × 10-4 g/L D) 9.9 × 10-3 g/L E) 1.2 × 10-3 g/L A) 1.2 × 10-15 g/L B) 7.5 × 10-3 g/L C) 2.0 × 10-4 g/L D) 9.9 × 10-3 g/L E) 1.2 × 10-3 g/L

Exam 18: Solubility and Simultaneous Equilibria

Mercury ions (Hg²⁺)are very difficult to dissolve in a solution of water, or even a dilute solution of NaOH. But if ammonia is added to the water, mercury ions are more readily soluble. Which of the following best explains why this happens?

(Multiple Choice)

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Question 41

Methylamine, CH₃NH₂, is a weak molecular base with a value of 4.4 × 10^-4 for K_b. An aqueous solution contains 0.200 M CH₃NH₂ and 0.400 M CH₃NH₃Cl per liter as the only solutes. If the K_sp of Mg(OH)₂ is 7.1 × 10^-12, what is the maximum [Mg²⁺] that can coexist with these solutes in the solution?Hint: Use the Henderson-Hasselbalch formula to find the pOH of the solution, and then use that to find [OH^-^].

(Multiple Choice)

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Question 42

The solubility of magnesium carbonate, MgCO₃, in pure water is 2.6 × 10^-⁴ moles per liter. Calculate the value of K_sp for magnesium carbonate from this data.

(Multiple Choice)

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Question 43

Will a precipitate form when 20.0 mL of 1.8 × 10^-³ M Pb(NO₃)₂ is added to 30.0 mL of5.0 × 10^-⁴M Na₂SO₄? The K_sp of (PbSO₄)is 6.3 × 10^-⁷.Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

(Multiple Choice)

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Question 44

Which of the following is the expression for the solubility product of calcium fluoride, CaF₂?

(Multiple Choice)

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Question 45

The solubility of barium carbonate is 14.8 mg L^-1 at 30 °C. Calculate the K_sp value for BaCO_3.

(Multiple Choice)

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Question 46

200 mL of an aqueous solution contains 0.030 M concentrations of both Pb²⁺ and Ag⁺. If 100 mL of 0.20 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The K_sp values for PbCl₂ and AgCl are 1.7 × 10^-5 and 1.8 × 10^-10.Hint: Remember that the solutions are being diluted and use the diluted concentrations.

(Short Answer)

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Question 47

What is the maximum concentration of Mg²⁺ ion that can exist in a 0.10 M NaF(aq)solution, without precipitating any magnesium fluoride? The K_sp of MgF₂ is 6.6 × 10^-⁹.

(Multiple Choice)

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Question 48

Given the following information: What is the equilibrium constant for the reaction below?

(Multiple Choice)

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Question 49

The sulfide ion is too basic to exist as such in aqueous solutions.

(True/False)

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Question 50

Methylamine, CH₃NH₂, is a weak molecular base with a value of 4.4 × 10^-4 for K_b. An aqueous solution contains 0.200 M CH₃NH₂ and 0.300 M CH₃NH₃Cl per liter as the only solutes. If the K_sp of Fe(OH)₂ is 7.9 × 10^-16, what is the maximum [Fe²⁺] that can coexist with these solutes in the solution?Hint: Use the Henderson-Hasselbalch formula to find the pOH of the solution, and then use that to find [OH^-^].

(Multiple Choice)

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Question 51

The formation constant for the diammine silver(I)ion is 1.6 × 10⁷, while the solubility product constant for silver chloride is 1.8 × 10¹⁰. What is the equilibrium constant for the reaction,AgCl(s)+ 2 NH₃(aq) Ag(NH₃)₂⁺(aq)+ Cl(aq)?

(Short Answer)

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Question 52

Metal cations in the chloride solubility group can be separated from other cations because they form ________ chloride compounds in a solution of HCl.

(Short Answer)

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Question 53

The solubility product for Ag₃PO₄ is: K_sp = 2.8 × 10^-¹⁸. What is the solubility of Ag₃PO₄ in water, in grams per liter?

(Multiple Choice)

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Question 54

Even though silver chloride is only very slightly soluble in water, addition of a reagent which forms complex ions with silver ions increases this solubility.

(True/False)

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Question 55

The K_sp value for barium chromate is 2.1 × 10^-10. A 4.16 g sample of BaCl₂ and a 5.83 g sample of potassium chromate were added to a 1.000 liter volumetric flask, and distilled water was added to the mark. After placing the stopper and shaking the flask to dissolve as much chemicals as would dissolve, how many grams of precipitate, if any, would be formed?Hint: Solving this problem requires comparing Q vs K_sp.

(Multiple Choice)

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Question 56

The solubility of strontium fluoride, SrF₂, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

(Multiple Choice)

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Question 57

What is the solubility, in moles per liter, of AgCl (K_sp = 1.8 × 10^-¹⁰), in 0.0100 molar aqueous potassium chloride solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.

(Multiple Choice)

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Question 58

Which one of the compounds below has the lowest solubility in water, expressed in moles per liter?

(Multiple Choice)

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Question 59

Many metal sulfides have ________ solubilities.

(Short Answer)

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Question 60

Showing 41 - 60 of 120

Mercury ions (Hg²⁺)are very difficult to dissolve in a solution of water, or even a dilute solution of NaOH. But if ammonia is added to the water, mercury ions are more readily soluble. Which of the following best explains why this happens?

The solubility of magnesium carbonate, MgCO₃, in pure water is 2.6 × 10^-⁴ moles per liter. Calculate the value of K_sp for magnesium carbonate from this data.

Will a precipitate form when 20.0 mL of 1.8 × 10^-³ M Pb(NO₃)₂ is added to 30.0 mL of5.0 × 10^-⁴M Na₂SO₄? The K_sp of (PbSO₄)is 6.3 × 10^-⁷.Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

Which of the following is the expression for the solubility product of calcium fluoride, CaF₂?

The solubility of barium carbonate is 14.8 mg L^-1 at 30 °C. Calculate the K_sp value for BaCO_3.

What is the maximum concentration of Mg²⁺ ion that can exist in a 0.10 M NaF(aq)solution, without precipitating any magnesium fluoride? The K_sp of MgF₂ is 6.6 × 10^-⁹.

Given the following information: What is the equilibrium constant for the reaction below?

The sulfide ion is too basic to exist as such in aqueous solutions.

The formation constant for the diammine silver(I)ion is 1.6 × 10⁷, while the solubility product constant for silver chloride is 1.8 × 10¹⁰. What is the equilibrium constant for the reaction,AgCl(s)+ 2 NH₃(aq) Ag(NH₃)₂⁺(aq)+ Cl(aq)?

Metal cations in the chloride solubility group can be separated from other cations because they form ________ chloride compounds in a solution of HCl.

The solubility product for Ag₃PO₄ is: K_sp = 2.8 × 10^-¹⁸. What is the solubility of Ag₃PO₄ in water, in grams per liter?

Even though silver chloride is only very slightly soluble in water, addition of a reagent which forms complex ions with silver ions increases this solubility.

The solubility of strontium fluoride, SrF₂, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

What is the solubility, in moles per liter, of AgCl (K_sp = 1.8 × 10^-¹⁰), in 0.0100 molar aqueous potassium chloride solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.

Which one of the compounds below has the lowest solubility in water, expressed in moles per liter?

Many metal sulfides have ________ solubilities.

A Very Brief History of Chemistry

Scientific Measurements

Elements, Compounds, and the Periodic Table

The Mole and Stoichiometry

Molecular View of Reactions in Aqueous Solutions

Oxidation-Reduction Reactions

Energy and Chemical Change

The Quantum Mechanical Atom

The Basics of Chemical Bonding

Theories of Bonding and Structure

Properties of Gases

Intermolecular Attractions and the Properties of Liquids and Solids

Mixtures at the Molecular Level: Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases, a Molecular Look

Acid-Base Equilibria in Aqueous Solutions

Thermodynamics

Electrochemistry

Nuclear Reactions and Their Role in Chemistry

Metal Complexes

Organic Compounds, Polymers, and Biochemicals

Filters

Exam 18: Solubility and Simultaneous Equilibria

Mercury ions (Hg2+)are very difficult to dissolve in a solution of water, or even a dilute solution of NaOH. But if ammonia is added to the water, mercury ions are more readily soluble. Which of the following best explains why this happens?

The solubility of magnesium carbonate, MgCO3, in pure water is 2.6 × 10-4 moles per liter. Calculate the value of Ksp for magnesium carbonate from this data.

Will a precipitate form when 20.0 mL of 1.8 × 10-3 M Pb(NO3)2 is added to 30.0 mL of5.0 × 10-4 M Na2SO4? The Ksp of (PbSO4)is 6.3 × 10-7.Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

Which of the following is the expression for the solubility product of calcium fluoride, CaF2?

The solubility of barium carbonate is 14.8 mg L-1 at 30 °C. Calculate the Ksp value for BaCO3.

What is the maximum concentration of Mg2+ ion that can exist in a 0.10 M NaF(aq)solution, without precipitating any magnesium fluoride? The Ksp of MgF2 is 6.6 × 10-9.

Given the following information: What is the equilibrium constant for the reaction below?

The sulfide ion is too basic to exist as such in aqueous solutions.

The formation constant for the diammine silver(I)ion is 1.6 × 107, while the solubility product constant for silver chloride is 1.8 × 1010. What is the equilibrium constant for the reaction,AgCl(s)+ 2 NH3(aq) Ag(NH3)2+(aq)+ Cl(aq)?

Metal cations in the chloride solubility group can be separated from other cations because they form ________ chloride compounds in a solution of HCl.

The solubility product for Ag3PO4 is: Ksp = 2.8 × 10-18. What is the solubility of Ag3PO4 in water, in grams per liter?

Even though silver chloride is only very slightly soluble in water, addition of a reagent which forms complex ions with silver ions increases this solubility.

The solubility of strontium fluoride, SrF2, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

What is the solubility, in moles per liter, of AgCl (Ksp = 1.8 × 10-10), in 0.0100 molar aqueous potassium chloride solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.

Which one of the compounds below has the lowest solubility in water, expressed in moles per liter?

Many metal sulfides have ________ solubilities.

A Very Brief History of Chemistry

Scientific Measurements

Elements, Compounds, and the Periodic Table

The Mole and Stoichiometry

Molecular View of Reactions in Aqueous Solutions

Oxidation-Reduction Reactions

Energy and Chemical Change

The Quantum Mechanical Atom

The Basics of Chemical Bonding

Theories of Bonding and Structure

Properties of Gases

Intermolecular Attractions and the Properties of Liquids and Solids

Mixtures at the Molecular Level: Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases, a Molecular Look

Acid-Base Equilibria in Aqueous Solutions

Thermodynamics

Electrochemistry

Nuclear Reactions and Their Role in Chemistry

Metal Complexes

Organic Compounds, Polymers, and Biochemicals

Filters

Mercury ions (Hg²⁺)are very difficult to dissolve in a solution of water, or even a dilute solution of NaOH. But if ammonia is added to the water, mercury ions are more readily soluble. Which of the following best explains why this happens?

The solubility of magnesium carbonate, MgCO₃, in pure water is 2.6 × 10^-⁴ moles per liter. Calculate the value of K_sp for magnesium carbonate from this data.

Will a precipitate form when 20.0 mL of 1.8 × 10^-³ M Pb(NO₃)₂ is added to 30.0 mL of5.0 × 10^-⁴M Na₂SO₄? The K_sp of (PbSO₄)is 6.3 × 10^-⁷.Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

Which of the following is the expression for the solubility product of calcium fluoride, CaF₂?

The solubility of barium carbonate is 14.8 mg L^-1 at 30 °C. Calculate the K_sp value for BaCO_3.

What is the maximum concentration of Mg²⁺ ion that can exist in a 0.10 M NaF(aq)solution, without precipitating any magnesium fluoride? The K_sp of MgF₂ is 6.6 × 10^-⁹.

The formation constant for the diammine silver(I)ion is 1.6 × 10⁷, while the solubility product constant for silver chloride is 1.8 × 10¹⁰. What is the equilibrium constant for the reaction,AgCl(s)+ 2 NH₃(aq) Ag(NH₃)₂⁺(aq)+ Cl(aq)?

The solubility product for Ag₃PO₄ is: K_sp = 2.8 × 10^-¹⁸. What is the solubility of Ag₃PO₄ in water, in grams per liter?

The solubility of strontium fluoride, SrF₂, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

What is the solubility, in moles per liter, of AgCl (K_sp = 1.8 × 10^-¹⁰), in 0.0100 molar aqueous potassium chloride solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.