NaOH is added to sea water containing 0.050 moles per liter of Mg2+ ion until the pH reaches 12.0. A certain quantity of Mg(OH)2 precipitates. How many parts per billion of magnesium are left behind in the solution? The Ksp of Mg(OH)2 is 7.1 × 10-12.Hint: Find [Mg2+], then convert to ppb.

A) 1.2 ppb B) 12 ppb C) 0.17 ppb D) 1.7 ppb E) 173 ppb A) 1.2 ppb B) 12 ppb C) 0.17 ppb D) 1.7 ppb E) 173 ppb

Calculate the minimum concentration of Ag+ ion that must be added to (or built up in)a 0.140 M Na2CrO4 solution, in order to initiate a precipitation of silver chromate. The Ksp of Ag2CrO4 is 1.2 × 10-12.Hint: Use an ICE table to help organize your given information and remember to account for the presence of a common ion.

A) 4.8 × 10-9 mol L-1 B) 2.9 × 10-6 mol L-1 C) 2.0 × 10-6 mol L-1 D) 9.5 × 10-7 mol L-1 E) 1.4 × 10-6 mol L-1 A) 4.8 × 10-9 mol L-1 B) 2.9 × 10-6 mol L-1 C) 2.0 × 10-6 mol L-1 D) 9.5 × 10-7 mol L-1 E) 1.4 × 10-6 mol L-1

The solubility product of barium fluoride (BaF2)is 1.7 × 10-6. Calculate the concentration of fluoride ions in a saturated solution of barium fluoride.

A) 7.6 × 10-3 M B) 1.5 × 10-2 M C) 3.4 × 10-5 M D) 1.7 × 10-6 M E) 3.4 × 10-6 M A) 7.6 × 10-3 M B) 1.5 × 10-2 M C) 3.4 × 10-5 M D) 1.7 × 10-6 M E) 3.4 × 10-6 M

The solubility of silver carbonate, Ag2CO3, in pure water is 1.27 × 10-4 moles per liter. Calculate the value of Ksp for silver carbonate from this data.

A) 1.64 × 10-11 B) 3.28 × 10-11 C) 2.04 × 10-12 D) 4.10 × 10-12 E) 8.19 × 10-12 A) 1.64 × 10-11 B) 3.28 × 10-11 C) 2.04 × 10-12 D) 4.10 × 10-12 E) 8.19 × 10-12

The solubility of zinc(II)phosphate, Zn3(PO4)2, in pure water is 1.5 × 10-7 moles per liter. Calculate the value of Ksp for zinc(II)phosphate from this data.

A) 2.3 × 10-14 B) 5.1 × 10-28 C) 2.7 × 10-33 D) 8.2 × 10-33 E) 7.6 × 10-35 A) 2.3 × 10-14 B) 5.1 × 10-28 C) 2.7 × 10-33 D) 8.2 × 10-33 E) 7.6 × 10-35

The solubility of calcium oxalate, CaC2O4, in pure water is 4.8 × 10-5 moles per liter. Calculate the value of Ksp for calcium oxalate from this data.

A) 2.4 × 10-5 B) 9.6 × 10-5 C) 4.6 × 10-9 D) 2.3 × 10-9 E) 5.3 × 10-18 A) 2.4 × 10-5 B) 9.6 × 10-5 C) 4.6 × 10-9 D) 2.3 × 10-9 E) 5.3 × 10-18

Exam 18: Solubility and Simultaneous Equilibria

NaOH is added to sea water containing 0.050 moles per liter of Mg²⁺ ion until the pH reaches 12.0. A certain quantity of Mg(OH)₂ precipitates. How many parts per billion of magnesium are left behind in the solution? The K_sp of Mg(OH)₂ is 7.1 × 10^-¹².Hint: Find [Mg²⁺^{], then convert to ppb.}

(Multiple Choice)

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Question 21

Calculate the minimum concentration of Ag⁺ ion that must be added to (or built up in)a 0.140 M Na₂CrO₄ solution, in order to initiate a precipitation of silver chromate. The K_sp of Ag₂CrO₄ is 1.2 × 10^-¹².Hint: Use an ICE table to help organize your given information and remember to account for the presence of a common ion.

(Multiple Choice)

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Question 22

Addition of a common ion to a solution of a slightly soluble salt will ________ the solubility of the slightly soluble salt.

(Short Answer)

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Question 23

200 mL of an aqueous solution contains 0.030 M concentrations of both Pb²⁺ and Ag⁺. If 100 mL of 6.0 × 10^-2 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 24

What is the solubility, in moles per liter, of AgCl (K_sp = 1.8 × 10^-10), in 0.0300 M CaCl₂ solution?Hint: Be sure to account for the presence of a common ion and carefully organize. You should also be able to simplify the math because the solubility is very low.

(Multiple Choice)

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Question 25

The oxide ion can exist in aqueous solutions provided the pH is higher than 11.00.

(True/False)

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Question 26

The solubility of silver phosphate, Ag₃PO₄, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

(Multiple Choice)

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Question 27

The solubility product of barium fluoride (BaF₂)is 1.7 × 10^-⁶. Calculate the concentration of fluoride ions in a saturated solution of barium fluoride.

(Multiple Choice)

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Question 28

What is the solubility, in moles per liter, of PbSO₄ (K_sp = 6.3 × 10^-7)in 0.0230 molar MgSO₄ 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 29

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

(Multiple Choice)

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Question 30

A solution contains Ba²⁺ (1.0 × 10^-3 M), Ca²⁺(1.0 × 10^-3 M)and K⁺ (1.0 × 10^-3 M). Drops of a 5.0 × 10^-1 M solution of NaF were added through a microburet until the [F^-] in the solution mix reached 1.5 × 10^-3 M. Should a precipitate form? If so, what is the precipitate? The K_spvalues are BaF₂: 1.0 × 10^-6, CaF₂: 5.3 × 10^-9. (Neglect the slight change in volume resulting from the added NaF solution.)

(Multiple Choice)

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Question 31

The solubility of silver carbonate, Ag₂CO₃, in pure water is 1.27 × 10^-⁴ moles per liter. Calculate the value of K_sp for silver carbonate from this data.

(Multiple Choice)

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Question 32

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, what would be the barium ion concentration remaining in solution afterwards? Be mindful that a precipitate may be formed.Hint: Solving this problem requires comparing Q vs K_sp.

(Multiple Choice)

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Question 33

The solubility of lead iodide is 578 mg L^-1 at 25 °C. What is the K_sp for PbI₂?

(Multiple Choice)

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Question 34

A precipitate will form when a solution containing a cation and a solution containing an anion are mixed if the exceeds the value of the .

(Short Answer)

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Question 35

Which one of the following salts has the highest solubility in water, expressed in moles per liter?

(Multiple Choice)

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Question 36

Calculate the concentration of chloride ions in a saturated lead(II)chloride solution. The K_sp = 2.4 × 10^-4 for lead(II)chloride.

(Short Answer)

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Question 37

The solubility of zinc(II)phosphate, Zn₃(PO₄)₂, in pure water is 1.5 × 10^-⁷ moles per liter. Calculate the value of K_sp for zinc(II)phosphate from this data.

(Multiple Choice)

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Question 38

The formation constant for the tris(ethylenediammine)nickel(II)complex ion, [Ni(en)₃]²⁺, is 4.1 × 10¹⁷. What is the concentration of the free nickel(II)ion in a solution in which the equilibrium concentration of free ethylenediammine is 0.400 M, and that of the nickel complex above is 0.0100 M?

(Short Answer)

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Question 39

The solubility of calcium oxalate, CaC₂O₄, in pure water is 4.8 × 10^-⁵ moles per liter. Calculate the value of K_sp for calcium oxalate from this data.

(Multiple Choice)

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Question 40

Showing 21 - 40 of 120

Addition of a common ion to a solution of a slightly soluble salt will ________ the solubility of the slightly soluble salt.

What is the solubility, in moles per liter, of AgCl (K_sp = 1.8 × 10^-10), in 0.0300 M CaCl₂ solution?Hint: Be sure to account for the presence of a common ion and carefully organize. You should also be able to simplify the math because the solubility is very low.

The oxide ion can exist in aqueous solutions provided the pH is higher than 11.00.

The solubility of silver phosphate, Ag₃PO₄, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

The solubility product of barium fluoride (BaF₂)is 1.7 × 10^-⁶. Calculate the concentration of fluoride ions in a saturated solution of barium fluoride.

What is the solubility, in moles per liter, of PbSO₄ (K_sp = 6.3 × 10^-7)in 0.0230 molar MgSO₄ 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.

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

The solubility of silver carbonate, Ag₂CO₃, in pure water is 1.27 × 10^-⁴ moles per liter. Calculate the value of K_sp for silver carbonate from this data.

The solubility of lead iodide is 578 mg L^-1 at 25 °C. What is the K_sp for PbI₂?

A precipitate will form when a solution containing a cation and a solution containing an anion are mixed if the exceeds the value of the .

Which one of the following salts has the highest solubility in water, expressed in moles per liter?

Calculate the concentration of chloride ions in a saturated lead(II)chloride solution. The K_sp = 2.4 × 10^-4 for lead(II)chloride.

The solubility of zinc(II)phosphate, Zn₃(PO₄)₂, in pure water is 1.5 × 10^-⁷ moles per liter. Calculate the value of K_sp for zinc(II)phosphate from this data.

The solubility of calcium oxalate, CaC₂O₄, in pure water is 4.8 × 10^-⁵ moles per liter. Calculate the value of K_sp for calcium oxalate from this data.

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

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Exam 18: Solubility and Simultaneous Equilibria

NaOH is added to sea water containing 0.050 moles per liter of Mg2+ ion until the pH reaches 12.0. A certain quantity of Mg(OH)2 precipitates. How many parts per billion of magnesium are left behind in the solution? The Ksp of Mg(OH)2 is 7.1 × 10-12.Hint: Find [Mg2+], then convert to ppb.

Addition of a common ion to a solution of a slightly soluble salt will ________ the solubility of the slightly soluble salt.

What is the solubility, in moles per liter, of AgCl (Ksp = 1.8 × 10-10), in 0.0300 M CaCl2 solution?Hint: Be sure to account for the presence of a common ion and carefully organize. You should also be able to simplify the math because the solubility is very low.

The oxide ion can exist in aqueous solutions provided the pH is higher than 11.00.

The solubility of silver phosphate, Ag3PO4, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

The solubility product of barium fluoride (BaF2)is 1.7 × 10-6. Calculate the concentration of fluoride ions in a saturated solution of barium fluoride.

What is the solubility, in moles per liter, of PbSO4 (Ksp = 6.3 × 10-7)in 0.0230 molar MgSO4 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.

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

The solubility of silver carbonate, Ag2CO3, in pure water is 1.27 × 10-4 moles per liter. Calculate the value of Ksp for silver carbonate from this data.

The solubility of lead iodide is 578 mg L-1 at 25 °C. What is the Ksp for PbI2?

A precipitate will form when a solution containing a cation and a solution containing an anion are mixed if the ________ exceeds the value of the ________.

Which one of the following salts has the highest solubility in water, expressed in moles per liter?

Calculate the concentration of chloride ions in a saturated lead(II)chloride solution. The Ksp = 2.4 × 10-4 for lead(II)chloride.

The solubility of zinc(II)phosphate, Zn3(PO4)2, in pure water is 1.5 × 10-7 moles per liter. Calculate the value of Ksp for zinc(II)phosphate from this data.

The formation constant for the tris(ethylenediammine)nickel(II)complex ion, [Ni(en)3]2+, is 4.1 × 1017. What is the concentration of the free nickel(II)ion in a solution in which the equilibrium concentration of free ethylenediammine is 0.400 M, and that of the nickel complex above is 0.0100 M?

The solubility of calcium oxalate, CaC2O4, in pure water is 4.8 × 10-5 moles per liter. Calculate the value of Ksp for calcium oxalate from this data.

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

What is the solubility, in moles per liter, of AgCl (K_sp = 1.8 × 10^-10), in 0.0300 M CaCl₂ solution?Hint: Be sure to account for the presence of a common ion and carefully organize. You should also be able to simplify the math because the solubility is very low.

The solubility of silver phosphate, Ag₃PO₄, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

The solubility product of barium fluoride (BaF₂)is 1.7 × 10^-⁶. Calculate the concentration of fluoride ions in a saturated solution of barium fluoride.

What is the solubility, in moles per liter, of PbSO₄ (K_sp = 6.3 × 10^-7)in 0.0230 molar MgSO₄ 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.

The solubility of silver carbonate, Ag₂CO₃, in pure water is 1.27 × 10^-⁴ moles per liter. Calculate the value of K_sp for silver carbonate from this data.

The solubility of lead iodide is 578 mg L^-1 at 25 °C. What is the K_sp for PbI₂?

A precipitate will form when a solution containing a cation and a solution containing an anion are mixed if the exceeds the value of the .

Calculate the concentration of chloride ions in a saturated lead(II)chloride solution. The K_sp = 2.4 × 10^-4 for lead(II)chloride.

The solubility of zinc(II)phosphate, Zn₃(PO₄)₂, in pure water is 1.5 × 10^-⁷ moles per liter. Calculate the value of K_sp for zinc(II)phosphate from this data.

The solubility of calcium oxalate, CaC₂O₄, in pure water is 4.8 × 10^-⁵ moles per liter. Calculate the value of K_sp for calcium oxalate from this data.