The pKa's of the three acid-conjugate base pairs derived from phosphoric acid, H3PO4, are 2.12, 7.21 and 12.32. How many g of sodium hydroxide would have be added to 150 mL of 0.1 M H3PO4 to prepare a buffer of pH = 7.41?

A) 0. 21 g B) 0.34 g C) 0.56 g D) 0.83 g E) 0.91 g A) 0. 21 g B) 0.34 g C) 0.56 g D) 0.83 g E) 0.91 g

Exam 16: Applications of Aqueous Equilibria

Calculate the pH in the titration of a 0.325 g sample of acetylsalicylic acid (see line drawing below) initially in 25.0 mL water with 0.102 M NaOH when (a) 6.23 mL and (b) 20.00 mL of titrant have been added.

(Short Answer)

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Question 41

The pK_a's of the three acid-conjugate base pairs derived from phosphoric acid, H₃PO₄, are 2.12, 7.21 and 12.32. How many g of sodium hydroxide would have be added to 150 mL of 0.1 M H₃PO₄ to prepare a buffer of pH = 7.41?

(Multiple Choice)

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Question 42

An aqueous solution is 0.2 M in both Mg²⁺ and Pb²⁺ ions. You wish to separate the two metal ions by adding oxalate, C₂O₄^2-. What is the concentration of lead when Mg²⁺begins to precipitate?K_sp (MgC₂O₄) = 8.5 x 10^-5 K_sp (PbC₂O₄) = 2.7 x 10^-11

(Short Answer)

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Question 43

Consider the titration of 25.0 mL of an 0.11 M lactic acid solution CH₃CH(OH)COOH (K_a= 8.4 x10^-4) with 0.150 M NaOH.a) Calculate the pH after 10 mL of the NaOH solution has been added.b) Calculate the pH of the solution at 10 mL of NaOH past the stoichiometric point.c) Would phenol red (pK_in = 7.9) or phenolphthalein (pK_in = 9.4) be a better indicator for this titration?

(Short Answer)

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Question 44

What is the pH of the resulting solution when 0.1 moles of HCl are added to 1 L of solution containing 0.12 moles of aqueous Na₂CO₃?If needed, use the following equation: pH = pK_a + log(A^-/HA)

(Short Answer)

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Question 45

Trisbipyridylruthenium (II), Ru²⁺(BIPY)₃, has been used in many studies, most recently to understand electrical conductivity in DNA molecules. Write all the equilibria in the formation of this complex.

(Essay)

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Question 46

Explain how to prepare a buffered solution of known pH and capacity.

(Essay)

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Question 47

What mass of sodium acetate must be added to 250 mL of 0.10 M acetic acid (pK_a = 4.75) to give a buffer of pH = 4.90?

(Short Answer)

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Question 48

Write the equation showing how Na₂HPO₄ and NaH₂PO₄ act as a buffer. Also write an equation showing how this buffer reacts when HCl is added.

(Essay)

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Question 49

What is the concentration of phosphate in a solution made from a 0.15 M phosphoric acid whose pH has been adjusted to 7.6 by the addition of solid sodium hydroxide (assume no volume change)?

(Short Answer)

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Question 50

Your friend at Podunk U. urgently emails asking if you remember any acid-base chemistry. His problem is that for his final organic lab problem he needs to report the pK_a of his acid. He did the pH titration, but only wrote down the following data for the titratant volumes: V = 14.27 mL; pH = 4.73. V_{equivalence point} = 22.43 mL. What is the pK_aof the unknown acid?

(Multiple Choice)

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Question 51

Which of the following is NOT one of the equilibria in the complexation of Ru(II) by ammonia (coordination number = 6)?

(Multiple Choice)

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Question 52

Use the concepts of K_sp and the common-ion effect to calculate solution concentrations.

(Essay)

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Question 53

A buffer is made by adding 0.82 moles of monohydrogen phosphate and 0.82 moles of dihydrogen phosphate to sufficient water to give a total volume of 1.0 L. Hydrogen chloride, 0.60 moles, is absorbed into the solution. What is the pH?

(Short Answer)

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Question 54

What is the solubility product expression for barium phosphate?

(Multiple Choice)

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Question 55

Two buffer solutions of the same pH are prepared. After adding 15 millimoles of acid to 250 mL of one solution, the pH changes by 0.02 pH unit. Adding 15 millimoles of acid to 250 mL of the second solution results in a 0.05 pH unit change. Which statement most accurately describes the differences between the two buffer solutions?

(Multiple Choice)

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Question 56

A 1.32 g sample of solid CuCl₂•2H₂O is added to 1.21 L of 2.0 M aqueous ammonia. The formation constant for tetra-amminecopper (II) is 1.0 x 10¹². What is the concentration of aqueous copper (II) in this solution?

(Short Answer)

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Question 57

What is the solubility product expression for iron (III) hydroxide?

(Multiple Choice)

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Question 58

Write the formation constant expression for the formation of [Zn(OH)₄]^-2 from Zn(OH)_2(s).Zn(OH)_2(s) + OH^-(aq) [Zn(OH)₃]^-1(aq)[Zn(OH)₃]^-1(aq) + OH^-(aq) [Zn(OH)₄]^-2(aq)

(Essay)

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Question 59

How many grams of AgNO₃ will dissolve in 1.32 L of a pH = 12.23 solution (K_sp AgOH = 1.52 x 10^-8)?

(Short Answer)

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Question 60

Showing 41 - 60 of 66

Calculate the pH in the titration of a 0.325 g sample of acetylsalicylic acid (see line drawing below) initially in 25.0 mL water with 0.102 M NaOH when (a) 6.23 mL and (b) 20.00 mL of titrant have been added.

The pK_a's of the three acid-conjugate base pairs derived from phosphoric acid, H₃PO₄, are 2.12, 7.21 and 12.32. How many g of sodium hydroxide would have be added to 150 mL of 0.1 M H₃PO₄ to prepare a buffer of pH = 7.41?

An aqueous solution is 0.2 M in both Mg²⁺ and Pb²⁺ ions. You wish to separate the two metal ions by adding oxalate, C₂O₄^2-. What is the concentration of lead when Mg²⁺begins to precipitate?K_sp (MgC₂O₄) = 8.5 x 10^-5 K_sp (PbC₂O₄) = 2.7 x 10^-11

What is the pH of the resulting solution when 0.1 moles of HCl are added to 1 L of solution containing 0.12 moles of aqueous Na₂CO₃?If needed, use the following equation: pH = pK_a + log(A^-/HA)

Trisbipyridylruthenium (II), Ru²⁺(BIPY)₃, has been used in many studies, most recently to understand electrical conductivity in DNA molecules. Write all the equilibria in the formation of this complex.

Explain how to prepare a buffered solution of known pH and capacity.

What mass of sodium acetate must be added to 250 mL of 0.10 M acetic acid (pK_a = 4.75) to give a buffer of pH = 4.90?

Write the equation showing how Na₂HPO₄ and NaH₂PO₄ act as a buffer. Also write an equation showing how this buffer reacts when HCl is added.

What is the concentration of phosphate in a solution made from a 0.15 M phosphoric acid whose pH has been adjusted to 7.6 by the addition of solid sodium hydroxide (assume no volume change)?

Which of the following is NOT one of the equilibria in the complexation of Ru(II) by ammonia (coordination number = 6)?

Use the concepts of K_sp and the common-ion effect to calculate solution concentrations.

A buffer is made by adding 0.82 moles of monohydrogen phosphate and 0.82 moles of dihydrogen phosphate to sufficient water to give a total volume of 1.0 L. Hydrogen chloride, 0.60 moles, is absorbed into the solution. What is the pH?

What is the solubility product expression for barium phosphate?

A 1.32 g sample of solid CuCl₂•2H₂O is added to 1.21 L of 2.0 M aqueous ammonia. The formation constant for tetra-amminecopper (II) is 1.0 x 10¹². What is the concentration of aqueous copper (II) in this solution?

What is the solubility product expression for iron (III) hydroxide?

Write the formation constant expression for the formation of [Zn(OH)₄]^-2 from Zn(OH)_2(s).Zn(OH)_2(s) + OH^-(aq) [Zn(OH)₃]^-1(aq)[Zn(OH)₃]^-1(aq) + OH^-(aq) [Zn(OH)₄]^-2(aq)

How many grams of AgNO₃ will dissolve in 1.32 L of a pH = 12.23 solution (K_sp AgOH = 1.52 x 10^-8)?

Fundamental Concepts of Chemistry

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Exam 16: Applications of Aqueous Equilibria

Calculate the pH in the titration of a 0.325 g sample of acetylsalicylic acid (see line drawing below) initially in 25.0 mL water with 0.102 M NaOH when (a) 6.23 mL and (b) 20.00 mL of titrant have been added.

The pKa's of the three acid-conjugate base pairs derived from phosphoric acid, H3PO4, are 2.12, 7.21 and 12.32. How many g of sodium hydroxide would have be added to 150 mL of 0.1 M H3PO4 to prepare a buffer of pH = 7.41?

An aqueous solution is 0.2 M in both Mg2+ and Pb2+ ions. You wish to separate the two metal ions by adding oxalate, C2O42-. What is the concentration of lead when Mg2+ begins to precipitate?Ksp (MgC2O4) = 8.5 x 10-5 Ksp (PbC2O4) = 2.7 x 10-11

What is the pH of the resulting solution when 0.1 moles of HCl are added to 1 L of solution containing 0.12 moles of aqueous Na2CO3?If needed, use the following equation: pH = pKa + log(A-/HA)

Trisbipyridylruthenium (II), Ru2+(BIPY)3, has been used in many studies, most recently to understand electrical conductivity in DNA molecules. Write all the equilibria in the formation of this complex.

Explain how to prepare a buffered solution of known pH and capacity.

What mass of sodium acetate must be added to 250 mL of 0.10 M acetic acid (pKa = 4.75) to give a buffer of pH = 4.90?

Write the equation showing how Na2HPO4 and NaH2PO4 act as a buffer. Also write an equation showing how this buffer reacts when HCl is added.

What is the concentration of phosphate in a solution made from a 0.15 M phosphoric acid whose pH has been adjusted to 7.6 by the addition of solid sodium hydroxide (assume no volume change)?

Which of the following is NOT one of the equilibria in the complexation of Ru(II) by ammonia (coordination number = 6)?

Use the concepts of Ksp and the common-ion effect to calculate solution concentrations.

A buffer is made by adding 0.82 moles of monohydrogen phosphate and 0.82 moles of dihydrogen phosphate to sufficient water to give a total volume of 1.0 L. Hydrogen chloride, 0.60 moles, is absorbed into the solution. What is the pH?

What is the solubility product expression for barium phosphate?

A 1.32 g sample of solid CuCl2•2H2O is added to 1.21 L of 2.0 M aqueous ammonia. The formation constant for tetra-amminecopper (II) is 1.0 x 1012. What is the concentration of aqueous copper (II) in this solution?

What is the solubility product expression for iron (III) hydroxide?

Write the formation constant expression for the formation of [Zn(OH)4]-2 from Zn(OH)2(s).Zn(OH)2(s) + OH-(aq) [Zn(OH)3]-1(aq)[Zn(OH)3]-1(aq) + OH-(aq) [Zn(OH)4]-2(aq)

How many grams of AgNO3 will dissolve in 1.32 L of a pH = 12.23 solution (Ksp AgOH = 1.52 x 10-8)?

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

The pK_a's of the three acid-conjugate base pairs derived from phosphoric acid, H₃PO₄, are 2.12, 7.21 and 12.32. How many g of sodium hydroxide would have be added to 150 mL of 0.1 M H₃PO₄ to prepare a buffer of pH = 7.41?

An aqueous solution is 0.2 M in both Mg²⁺ and Pb²⁺ ions. You wish to separate the two metal ions by adding oxalate, C₂O₄^2-. What is the concentration of lead when Mg²⁺begins to precipitate?K_sp (MgC₂O₄) = 8.5 x 10^-5 K_sp (PbC₂O₄) = 2.7 x 10^-11

What is the pH of the resulting solution when 0.1 moles of HCl are added to 1 L of solution containing 0.12 moles of aqueous Na₂CO₃?If needed, use the following equation: pH = pK_a + log(A^-/HA)

Trisbipyridylruthenium (II), Ru²⁺(BIPY)₃, has been used in many studies, most recently to understand electrical conductivity in DNA molecules. Write all the equilibria in the formation of this complex.

What mass of sodium acetate must be added to 250 mL of 0.10 M acetic acid (pK_a = 4.75) to give a buffer of pH = 4.90?

Write the equation showing how Na₂HPO₄ and NaH₂PO₄ act as a buffer. Also write an equation showing how this buffer reacts when HCl is added.

Use the concepts of K_sp and the common-ion effect to calculate solution concentrations.

A 1.32 g sample of solid CuCl₂•2H₂O is added to 1.21 L of 2.0 M aqueous ammonia. The formation constant for tetra-amminecopper (II) is 1.0 x 10¹². What is the concentration of aqueous copper (II) in this solution?

Write the formation constant expression for the formation of [Zn(OH)₄]^-2 from Zn(OH)_2(s).Zn(OH)_2(s) + OH^-(aq) [Zn(OH)₃]^-1(aq)[Zn(OH)₃]^-1(aq) + OH^-(aq) [Zn(OH)₄]^-2(aq)

How many grams of AgNO₃ will dissolve in 1.32 L of a pH = 12.23 solution (K_sp AgOH = 1.52 x 10^-8)?