If 13.5g of NiCl2.6H2O is added to 500mL of 1.50M aqueous ammonia, what is the equilibrium concentration of Ni2+(aq)? The complex formed is $\left[ \mathrm { Ni } \left( \mathrm { NH } _ { 3 } \right) _ { 6 } \right] ^ { 2 + }$ Given Kf = 5.5×108.

A) 5.4×10-10 B) 6.7×10-9 C) 1.5×10-10 D) 8.7×10-8 E) 2.1×10-9 A) 5.4×10-10 B) 6.7×10-9 C) 1.5×10-10 D) 8.7×10-8 E) 2.1×10-9

If the Ksp for AgCl is equal to 4.65×10-9 and the Kf for $\mathrm { AgCl } _ { 2 } ^ { - }$ is equal to 8.7×105 at $35 ^ { \circ } \mathrm { C }$ , what is the solubility of AgCl in pure water at the same temperature?

A) 5.89×10-6M B) 7.12×10-5M C) 6.82×10-5M D) 3.38×10-6M E) 8.22×10-6M A) 5.89×10-6M B) 7.12×10-5M C) 6.82×10-5M D) 3.38×10-6M E) 8.22×10-6M

If the Ksp for Ca3(PO4)2 at $30 ^ { \circ } \mathrm { C }$ is 6.47×10-32, what is the aqueous solubility of Ca3(PO4)2 in terms of the mass of salt that dissolves in 100mL of water at the same temperature?

A) 4.47×10-5g B) 2.98×10-6g C) 7.65×10-5g D) 7.03×10-6g E) 5.20×10-6g A) 4.47×10-5g B) 2.98×10-6g C) 7.65×10-5g D) 7.03×10-6g E) 5.20×10-6g

Exam 17: Solubility and Complexation Equilibriums

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If 13.5g of NiCl₂.6H₂O is added to 500mL of 1.50M aqueous ammonia, what is the equilibrium concentration of Ni²⁺(aq)? The complex formed is $\left[ \mathrm { Ni } \left( \mathrm { NH } _ { 3 } \right) _ { 6 } \right] ^ { 2 + }$ Given K_f = 5.5×10⁸.

(Multiple Choice)

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Question 81

If the K_sp for AgCl is equal to 4.65×10^-9 and the K_f for $\mathrm { AgCl } _ { 2 } ^ { - }$ is equal to 8.7×10⁵ at $35 ^ { \circ } \mathrm { C }$ , what is the solubility of AgCl in pure water at the same temperature?

(Multiple Choice)

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Question 82

If the K_spfor Ca₃(PO₄)₂ at $30 ^ { \circ } \mathrm { C }$ is 6.47×10^-32, what is the aqueous solubility of Ca₃(PO₄)₂in terms of the mass of salt that dissolves in 100mL of water at the same temperature?

(Multiple Choice)

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Question 83

The ion product describes concentrations that are not necessarily equilibrium concentrations.

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Question 84

Adding a(n) _____ to detergents prevents the magnesium and calcium salts from precipitating because the equilibrium constant for complex-ion formation is large.

(Short Answer)

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Question 85

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If 13.5g of NiCl₂.6H₂O is added to 500mL of 1.50M aqueous ammonia, what is the equilibrium concentration of Ni²⁺(aq)? The complex formed is $\left[ \mathrm { Ni } \left( \mathrm { NH } _ { 3 } \right) _ { 6 } \right] ^ { 2 + }$ Given K_f = 5.5×10⁸.

If the K_sp for AgCl is equal to 4.65×10^-9 and the K_f for $\mathrm { AgCl } _ { 2 } ^ { - }$ is equal to 8.7×10⁵ at $35 ^ { \circ } \mathrm { C }$ , what is the solubility of AgCl in pure water at the same temperature?

If the K_spfor Ca₃(PO₄)₂ at $30 ^ { \circ } \mathrm { C }$ is 6.47×10^-32, what is the aqueous solubility of Ca₃(PO₄)₂in terms of the mass of salt that dissolves in 100mL of water at the same temperature?

The ion product describes concentrations that are not necessarily equilibrium concentrations.

Adding a(n) _____ to detergents prevents the magnesium and calcium salts from precipitating because the equilibrium constant for complex-ion formation is large.

Introduction to Chemistry

Molecules, Ions, and Chemical Formulas

Chemical Reactions

Reactions in Aqueous Solution

Energy Changes in Chemical Reactions

The Structure of Atoms

The Periodic Table and Periodic Trends

Ionic Versus Covalent Bonding

Molecular Geometry and Covalent Bonding Models

Gases

Liquids

Solids

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Acidbase Equilibriums

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Periodic Trends and the S-Block Elements

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Exam 17: Solubility and Complexation Equilibriums

If 13.5g of NiCl2.6H2O is added to 500mL of 1.50M aqueous ammonia, what is the equilibrium concentration of Ni2+(aq)? The complex formed is [Ni(NH3)6]2+\left[ \mathrm { Ni } \left( \mathrm { NH } _ { 3 } \right) _ { 6 } \right] ^ { 2 + }[Ni(NH3​)6​]2+ Given Kf = 5.5×108.

If the Ksp for AgCl is equal to 4.65×10-9 and the Kf for AgCl2−\mathrm { AgCl } _ { 2 } ^ { - }AgCl2−​ is equal to 8.7×105 at 35∘C35 ^ { \circ } \mathrm { C }35∘C , what is the solubility of AgCl in pure water at the same temperature?

If the Ksp for Ca3(PO4)2 at 30∘C30 ^ { \circ } \mathrm { C }30∘C is 6.47×10-32, what is the aqueous solubility of Ca3(PO4)2 in terms of the mass of salt that dissolves in 100mL of water at the same temperature?

The ion product describes concentrations that are not necessarily equilibrium concentrations.

Adding a(n) _____ to detergents prevents the magnesium and calcium salts from precipitating because the equilibrium constant for complex-ion formation is large.

Introduction to Chemistry

Molecules, Ions, and Chemical Formulas

Chemical Reactions

Reactions in Aqueous Solution

Energy Changes in Chemical Reactions

The Structure of Atoms

The Periodic Table and Periodic Trends

Ionic Versus Covalent Bonding

Molecular Geometry and Covalent Bonding Models

Gases

Liquids

Solids

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Acidbase Equilibriums

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Periodic Trends and the S-Block Elements

The P-Block Elements

The D-Block Elements

Organic Compounds

Filters

If 13.5g of NiCl₂.6H₂O is added to 500mL of 1.50M aqueous ammonia, what is the equilibrium concentration of Ni²⁺(aq)? The complex formed is $\left[ \mathrm { Ni } \left( \mathrm { NH } _ { 3 } \right) _ { 6 } \right] ^ { 2 + }$ Given K_f = 5.5×10⁸.

If the K_sp for AgCl is equal to 4.65×10^-9 and the K_f for $\mathrm { AgCl } _ { 2 } ^ { - }$ is equal to 8.7×10⁵ at $35 ^ { \circ } \mathrm { C }$ , what is the solubility of AgCl in pure water at the same temperature?

If the K_spfor Ca₃(PO₄)₂ at $30 ^ { \circ } \mathrm { C }$ is 6.47×10^-32, what is the aqueous solubility of Ca₃(PO₄)₂in terms of the mass of salt that dissolves in 100mL of water at the same temperature?