For Ca(OH)2,Ksp = 4.0 × 10−6.What will occur if 1.0 L of 0.100 M Ca(NO3)2 is prepared in a solution that is buffered at pH 12.50?

A) Q > Ksp.A precipitate will form. B) Ksp > Q.A precipitate will form. C) Q = Ksp.No precipitate will form. D) Q > Ksp.No precipitate will form. E) Ksp > Q.No precipitate will form. A) Q > Ksp.A precipitate will form. B) Ksp > Q.A precipitate will form. C) Q = Ksp.No precipitate will form. D) Q > Ksp.No precipitate will form. E) Ksp > Q.No precipitate will form.

The Ksp of BaSO4 is 1.1 × 10-10 at 25°C.What mass of BaSO4 (molar mass = 233.4 g/mol)will dissolve in 1.0 L of water at 25°C?

A) 2.6 × 10−8 g B) 4.5 × 10−8 g C) 1.0 × 10−5 g D) 1.6 × 10−4 g E) 2.4 × 10−3 g A) 2.6 × 10−8 g B) 4.5 × 10−8 g C) 1.0 × 10−5 g D) 1.6 × 10−4 g E) 2.4 × 10−3 g

For PbCl2,Ksp = 1.7 × 10−5.What will occur if 250 mL of 0.12 M Pb(NO3)2 is mixed with 250 mL of 0.070 M NaCl?

A) Q > Ksp.A precipitate will form. B) Ksp > Q.A precipitate will form. C) Q = Ksp.No precipitate will form. D) Q > Ksp.No precipitate will form. E) Ksp > Q.No precipitate will form. A) Q > Ksp.A precipitate will form. B) Ksp > Q.A precipitate will form. C) Q = Ksp.No precipitate will form. D) Q > Ksp.No precipitate will form. E) Ksp > Q.No precipitate will form.

The Ksp of calcium phosphate is 1 × 10−33.What is the concentration of Ca2+ in equilibrium with Ca3(PO4)2(s)if [PO43−] = 1 × 10−5 M?

A) 1 × 10−28 M B) 1 × 10−23 M C) 1 × 10−11 M D) 5 × 10−10 M E) 2 × 10−8 M A) 1 × 10−28 M B) 1 × 10−23 M C) 1 × 10−11 M D) 5 × 10−10 M E) 2 × 10−8 M

In the qualitative analysis scheme,Mg2+ is a group IV cation.What anion is used to precipitate Mg2+?

A) OH− B) Cl− C) PO43− D) S2− E) CO32− A) OH− B) Cl− C) PO43− D) S2− E) CO32−

What is the water solubility of Hg2Br2 (Ksp = 6 × 10−23)in moles per liter?

A) 8 × 10−12 M B) 1 × 10−8 M C) 2 × 10−8 M D) 4 × 10−8 M E) 3 × 10−6 M A) 8 × 10−12 M B) 1 × 10−8 M C) 2 × 10−8 M D) 4 × 10−8 M E) 3 × 10−6 M

What is the net ionic equation for the reaction of Ca3(PO4)2 with a strong acid?

A) Ca3(PO4)2(s)+ 6H+(aq)→ 3CaH3(s)+ 2PO43−(aq) B) Ca3(PO4)2(s)+ 6H+(aq)→ 3Ca2+(aq)+ 2H3PO4(aq) C) 2PO43−(aq)+ 2H+(aq)→ H2PO4−(aq) D) 3Ca2+(aq)+ 2PO43−(aq)+ 6H+(aq)→ 2H3PO4(aq)+ 3Ca2+(aq) E) Ca3(PO4)2(s)+ 16H+(aq)→ Ca3P2(s)+ 8H2O(l) A) Ca3(PO4)2(s)+ 6H+(aq)→ 3CaH3(s)+ 2PO43−(aq) B) Ca3(PO4)2(s)+ 6H+(aq)→ 3Ca2+(aq)+ 2H3PO4(aq) C) 2PO43−(aq)+ 2H+(aq)→ H2PO4−(aq) D) 3Ca2+(aq)+ 2PO43−(aq)+ 6H+(aq)→ 2H3PO4(aq)+ 3Ca2+(aq) E) Ca3(PO4)2(s)+ 16H+(aq)→ Ca3P2(s)+ 8H2O(l)

What is the water solubility of AgCl (Ksp = 1.8 × 10−10,MM = 143.4 g/mol)in grams per liter?

A) 1.3 × 10−12 g/L B) 2.6 × 10−8 g/L C) 9.4 × 10−8 g/L D) 9.6 × 10−4 g/L E) 1.9 × 10−3 g/L A) 1.3 × 10−12 g/L B) 2.6 × 10−8 g/L C) 9.4 × 10−8 g/L D) 9.6 × 10−4 g/L E) 1.9 × 10−3 g/L

What is the water solubility of AgCl (Ksp = 1.8 × 10−10)in 0.25 M NaCl?

A) 4.5 × 10−11 M B) 7.2 × 10−10 M C) 1.8 × 10−9 M D) 1.7 × 10−7 M E) 1.3 × 10−5 M A) 4.5 × 10−11 M B) 7.2 × 10−10 M C) 1.8 × 10−9 M D) 1.7 × 10−7 M E) 1.3 × 10−5 M

What is the water solubility of AgI (Ksp = 1 × 10−16,MM = 234.8 g/mol)in moles per liter?

A) 1 × 10−32 M B) 1 × 10−16 M C) 1 × 10−8 M D) 2 × 10−6 M E) 4 × 10−11 M A) 1 × 10−32 M B) 1 × 10−16 M C) 1 × 10−8 M D) 2 × 10−6 M E) 4 × 10−11 M

Consider the equilibrium of magnesium fluoride,MgF2(s),in water. MgF2(s) ? Mg2+(aq)+ 2F?(aq), What is the effect of adding perchloric acid (i.e.decreasing the pH of solution)?

A) The acid will have no effect on the magnesium fluoride equilibrium. B) The F? will be protonated,resulting in more MgF2(s)dissolving. C) More MgF2(s)will be formed,thus reducing Mg2+ and F? concentrations in solution. D) Magnesium perchlorate,Mg(ClO4)2(s),will precipitate. E) Magnesium hydride,MgH2(s),will precipitate. A) The acid will have no effect on the magnesium fluoride equilibrium. B) The F? will be protonated,resulting in more MgF2(s)dissolving. C) More MgF2(s)will be formed,thus reducing Mg2+ and F? concentrations in solution. D) Magnesium perchlorate,Mg(ClO4)2(s),will precipitate. E) Magnesium hydride,MgH2(s),will precipitate.

A solution contains 0.10 M Ca2+ and 0.10 M Mg2+.The pH of the solution is raised without changing the volume of the solution.What percentage of Mg2+ remains in solution when Ca(OH)2(s)first begins to precipitate? (Ksp of Ca(OH)2 = 4.0 × 10−6 and Ksp of Mg(OH)2 = 7.1 × 10−12)

A) 1.8 × 10−4 % B) 4.0 × 10−4 % C) 6.3 × 10−3 % D) 7.2 × 10−3 % E) 1.4 × 10−2 % A) 1.8 × 10−4 % B) 4.0 × 10−4 % C) 6.3 × 10−3 % D) 7.2 × 10−3 % E) 1.4 × 10−2 %

Determine the equilibrium constant,K,for the following reaction, Ca(OH)2(s)+ 2H+(aq)→ Ca2+(aq)+ 2H2O(l) Given the Ksp of Ca(OH)2 is 4.0 × 10−6 and Kw is 1.0 × 10−-14.

A) 4.0 × 1020 B) 4.0 × 106 C) 1.0 × 1014 D) 2.5 × 109 E) 4.0 × 1022 A) 4.0 × 1020 B) 4.0 × 106 C) 1.0 × 1014 D) 2.5 × 109 E) 4.0 × 1022

Exam 15: Complex Ion and Precipitation Equilibria

An aqueous solution contains 0.010 M Br^- and 0.010 M I^-.If Ag⁺ is added until AgBr(s)just begins to precipitate,what are the concentrations of Ag⁺ and I^-? (K_sp of AgBr = 5.4 × 10^-13,K_sp of AgI = 8.5 × 10^-17)

(Multiple Choice)

(Multiple Choice)

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Question 59

Showing 41 - 59 of 59

Exam 15: Complex Ion and Precipitation Equilibria

An aqueous solution contains 0.010 M Br- and 0.010 M I-.If Ag+ is added until AgBr(s)just begins to precipitate,what are the concentrations of Ag+ and I-? (Ksp of AgBr = 5.4 × 10-13,Ksp of AgI = 8.5 × 10-17)

What is the net ionic equation for the reaction of ZnS with a strong acid?

What is the equilibrium constant expression for the dissolution of solid lead oxalate,PbC2O4,in water?

Which of the following metals will precipitate as chloride salts: Ag+,Pb2+,Ca2+,K+,and Cu2+?

For Ca(OH)2,Ksp = 4.0 × 10−6.What will occur if 1.0 L of 0.100 M Ca(NO3)2 is prepared in a solution that is buffered at pH 12.50?

The Ksp of BaSO4 is 1.1 × 10-10 at 25°C.What mass of BaSO4 (molar mass = 233.4 g/mol)will dissolve in 1.0 L of water at 25°C?

For PbCl2,Ksp = 1.7 × 10−5.What will occur if 250 mL of 0.12 M Pb(NO3)2 is mixed with 250 mL of 0.070 M NaCl?

The Ksp of calcium phosphate is 1 × 10−33.What is the concentration of Ca2+ in equilibrium with Ca3(PO4)2(s)if [PO43−] = 1 × 10−5 M?

In the qualitative analysis scheme,Mg2+ is a group IV cation.What anion is used to precipitate Mg2+?

What is the water solubility of Hg2Br2 (Ksp = 6 × 10−23)in moles per liter?

What is the net ionic equation for the reaction of an aqueous solution of AgNO3 and NH3?

What is the net ionic equation for the reaction of Ca3(PO4)2 with a strong acid?

What is the water solubility of AgCl (Ksp = 1.8 × 10−10,MM = 143.4 g/mol)in grams per liter?

What is the water solubility of AgCl (Ksp = 1.8 × 10−10)in 0.25 M NaCl?

What is the water solubility of AgI (Ksp = 1 × 10−16,MM = 234.8 g/mol)in moles per liter?

Consider the equilibrium of magnesium fluoride,MgF2(s),in water. MgF2(s) ? Mg2+(aq)+ 2F?(aq), What is the effect of adding perchloric acid (i.e.decreasing the pH of solution)?

Which of the following equations represents the formation constant of Ti(NH3)63+?

A solution contains 0.10 M Ca2+ and 0.10 M Mg2+.The pH of the solution is raised without changing the volume of the solution.What percentage of Mg2+ remains in solution when Ca(OH)2(s)first begins to precipitate? (Ksp of Ca(OH)2 = 4.0 × 10−6 and Ksp of Mg(OH)2 = 7.1 × 10−12)

Determine the equilibrium constant,K,for the following reaction, Ca(OH)2(s)+ 2H+(aq)→ Ca2+(aq)+ 2H2O(l) Given the Ksp of Ca(OH)2 is 4.0 × 10−6 and Kw is 1.0 × 10−-14.

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An aqueous solution contains 0.010 M Br^- and 0.010 M I^-.If Ag⁺ is added until AgBr(s)just begins to precipitate,what are the concentrations of Ag⁺ and I^-? (K_sp of AgBr = 5.4 × 10^-13,K_sp of AgI = 8.5 × 10^-17)

What is the equilibrium constant expression for the dissolution of solid lead oxalate,PbC₂O₄,in water?

Which of the following metals will precipitate as chloride salts: Ag⁺,Pb²⁺,Ca²⁺,K⁺,and Cu²⁺?

For Ca(OH)₂,K_sp = 4.0 × 10−⁶.What will occur if 1.0 L of 0.100 M Ca(NO₃)₂ is prepared in a solution that is buffered at pH 12.50?

The K_sp of BaSO₄ is 1.1 × 10^-10 at 25°C.What mass of BaSO₄ (molar mass = 233.4 g/mol)will dissolve in 1.0 L of water at 25°C?

For PbCl₂,K_sp = 1.7 × 10−⁵.What will occur if 250 mL of 0.12 M Pb(NO₃)₂ is mixed with 250 mL of 0.070 M NaCl?

The K_sp of calcium phosphate is 1 × 10−³³.What is the concentration of Ca²⁺ in equilibrium with Ca₃(PO₄)₂(s)if [PO₄³⁻] = 1 × 10−⁵ M?

In the qualitative analysis scheme,Mg²⁺ is a group IV cation.What anion is used to precipitate Mg²⁺?

What is the water solubility of Hg₂Br₂ (K_sp = 6 × 10−²³)in moles per liter?

What is the net ionic equation for the reaction of an aqueous solution of AgNO₃ and NH₃?

What is the net ionic equation for the reaction of Ca₃(PO₄)₂ with a strong acid?

What is the water solubility of AgCl (K_sp = 1.8 × 10−¹⁰,MM = 143.4 g/mol)in grams per liter?

What is the water solubility of AgCl (K_sp = 1.8 × 10−¹⁰)in 0.25 M NaCl?

What is the water solubility of AgI (K_sp = 1 × 10−¹⁶,MM = 234.8 g/mol)in moles per liter?

Consider the equilibrium of magnesium fluoride,MgF₂(s),in water. MgF₂(s) ? Mg²⁺(aq)+ 2F?(aq), What is the effect of adding perchloric acid (i.e.decreasing the pH of solution)?

Which of the following equations represents the formation constant of Ti(NH₃)₆³⁺?

Determine the equilibrium constant,K,for the following reaction, Ca(OH)₂(s)+ 2H⁺(aq)→ Ca²⁺(aq)+ 2H₂O(l) Given the K_sp of Ca(OH)₂ is 4.0 × 10−⁶ and K_w is 1.0 × 10−^-14.