Calculate the pH when 200.0 mL of a 1.00 M solution of HS1U1B12S1U1B0A (KS1U1B1a1S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P16S1S1P0, KS1U1B1a2S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P110S1S1P0) is titrated with the following volumes of 1.00 M NaOH. -400.0 mL of 1.00 M NaOH

A) 12.42 B) 11.76 C) 11.21 D) 10.00 E) None of these A) 12.42 B) 11.76 C) 11.21 D) 10.00 E) None of these

A titration of 100.0 mL of 1.00 M malonic acid (HS1U1B12S1U1B0A) was done with 1.00 M NaOH. For malonic acid, KS1U1B1a1S1U1B0 = 1.49 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P12S1S1P0, KS1U1B1a2S1U1B0 = 2.03 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P16S1S1P0. -Calculate [H+] after 150.0 mL of 1.00 M NaOH has been added.

A) 2.03 F1F1F1S1F1F1F10 10-6 M B) 1.41 F1F1F1S1F1F1F10 10-10 M C) 1.49 F1F1F1S1F1F1F10 10-2 M D) 1.00 F1F1F1S1F1F1F10 10-7 M E) none of these A) 2.03 F1F1F1S1F1F1F10 10-6 M B) 1.41 F1F1F1S1F1F1F10 10-10 M C) 1.49 F1F1F1S1F1F1F10 10-2 M D) 1.00 F1F1F1S1F1F1F10 10-7 M E) none of these

Calculate the pH when 200.0 mL of a 1.00 M solution of HS1U1B12S1U1B0A (KS1U1B1a1S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P16S1S1P0, KS1U1B1a2S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P110S1S1P0) is titrated with the following volumes of 1.00 M NaOH. -300.0 mL of 1.00 M NaOH

A) 10.00 B) 11.21 C) 9.50 D) 9.30 E) None of these A) 10.00 B) 11.21 C) 9.50 D) 9.30 E) None of these

The concentration of Al3+ in a saturated solution of Al(OH)3 at 25°C is 5.2 F1F1F1S1F1F1F10 10-9 M. Calculate the Ksp for Al(OH)3.

A) 7.3 F1F1F1S1F1F1F10 10-34 B) 2.9 F1F1F1S1F1F1F10 10-33 C) 2.0 F1F1F1S1F1F1F10 10-32 D) 5.6 F1F1F1S1F1F1F10 10-25 E) none of these A) 7.3 F1F1F1S1F1F1F10 10-34 B) 2.9 F1F1F1S1F1F1F10 10-33 C) 2.0 F1F1F1S1F1F1F10 10-32 D) 5.6 F1F1F1S1F1F1F10 10-25 E) none of these

Exam 8: Applications of Aqueous Equilibria

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Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -400.0 mL of 1.00 M NaOH

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Question 161

A 50.0-mL sample of 2.0  10^-⁴ M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃²^-: The concentration of Cu⁺ at equilibrium is

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Question 162

A 10-mL sample of tartaric acid is titrated to a phenolphthalein endpoint with 20. mL of 1.0 M NaOH. Assuming tartaric acid is diprotic, what is the molarity of the acid?

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Question 163

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49  10^-², K_a2 = 2.03  10^-⁶. -Calculate [H⁺] after 150.0 mL of 1.00 M NaOH has been added.

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Question 164

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -300.0 mL of 1.00 M NaOH

(Multiple Choice)

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Question 165

If 22 mL of 0.50 M HCl is added to 112 mL of 0.20 M NaOH, what is the final pH?

(Multiple Choice)

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Question 166

Which of the following compounds has the lowest solubility, in moles per liter, in water at 25°C?

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Question 167

A solution of hydrochloric acid of unknown concentration was titrated with 0.11 M NaOH. If a 150-mL sample of the HCl solution required exactly 12 mL of the NaOH solution to reach the equivalence point, what was the pH of the HCl solution?

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Question 168

It is observed that 7.5 mmol of BaF₂ will dissolve in 1.0 L of water. Use these data to calculate the value of K_sp for barium fluoride.

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Question 169

The concentration of Al³⁺ in a saturated solution of Al(OH)₃ at 25°C is 5.2  10^-⁹ M. Calculate the K_sp for Al(OH)₃.

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Question 170

Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What major species is(are) present at point III?

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Question 171

Showing 161 - 171 of 171

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -400.0 mL of 1.00 M NaOH

A 50.0-mL sample of 2.0  10^-⁴ M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃²^-: The concentration of Cu⁺ at equilibrium is

A 10-mL sample of tartaric acid is titrated to a phenolphthalein endpoint with 20. mL of 1.0 M NaOH. Assuming tartaric acid is diprotic, what is the molarity of the acid?

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49  10^-², K_a2 = 2.03  10^-⁶. -Calculate [H⁺] after 150.0 mL of 1.00 M NaOH has been added.

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -300.0 mL of 1.00 M NaOH

If 22 mL of 0.50 M HCl is added to 112 mL of 0.20 M NaOH, what is the final pH?

Which of the following compounds has the lowest solubility, in moles per liter, in water at 25°C?

A solution of hydrochloric acid of unknown concentration was titrated with 0.11 M NaOH. If a 150-mL sample of the HCl solution required exactly 12 mL of the NaOH solution to reach the equivalence point, what was the pH of the HCl solution?

It is observed that 7.5 mmol of BaF₂ will dissolve in 1.0 L of water. Use these data to calculate the value of K_sp for barium fluoride.

The concentration of Al³⁺ in a saturated solution of Al(OH)₃ at 25°C is 5.2  10^-⁹ M. Calculate the K_sp for Al(OH)₃.

Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What major species is(are) present at point III?

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Exam 8: Applications of Aqueous Equilibria

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0  10-6, Ka2 = 1.0  10-10) is titrated with the following volumes of 1.00 M NaOH. -400.0 mL of 1.00 M NaOH

A 50.0-mL sample of 2.0  10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. Cu+ reacts with CN- to form the complex ion Cu(CN)32-: The concentration of Cu+ at equilibrium is

A 10-mL sample of tartaric acid is titrated to a phenolphthalein endpoint with 20. mL of 1.0 M NaOH. Assuming tartaric acid is diprotic, what is the molarity of the acid?

A titration of 100.0 mL of 1.00 M malonic acid (H2A) was done with 1.00 M NaOH. For malonic acid, Ka1 = 1.49  10-2, Ka2 = 2.03  10-6. -Calculate [H+] after 150.0 mL of 1.00 M NaOH has been added.

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0  10-6, Ka2 = 1.0  10-10) is titrated with the following volumes of 1.00 M NaOH. -300.0 mL of 1.00 M NaOH

If 22 mL of 0.50 M HCl is added to 112 mL of 0.20 M NaOH, what is the final pH?

Which of the following compounds has the lowest solubility, in moles per liter, in water at 25°C?

A solution of hydrochloric acid of unknown concentration was titrated with 0.11 M NaOH. If a 150-mL sample of the HCl solution required exactly 12 mL of the NaOH solution to reach the equivalence point, what was the pH of the HCl solution?

It is observed that 7.5 mmol of BaF2 will dissolve in 1.0 L of water. Use these data to calculate the value of Ksp for barium fluoride.

The concentration of Al3+ in a saturated solution of Al(OH)3 at 25°C is 5.2  10-9 M. Calculate the Ksp for Al(OH)3.

Consider the following information about the diprotic acid ascorbic acid (H2As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na2As, with standard HCl is shown below: -What major species is(are) present at point III?

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Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

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Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

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Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -400.0 mL of 1.00 M NaOH

A 50.0-mL sample of 2.0  10^-⁴ M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃²^-: The concentration of Cu⁺ at equilibrium is

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49  10^-², K_a2 = 2.03  10^-⁶. -Calculate [H⁺] after 150.0 mL of 1.00 M NaOH has been added.

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -300.0 mL of 1.00 M NaOH

It is observed that 7.5 mmol of BaF₂ will dissolve in 1.0 L of water. Use these data to calculate the value of K_sp for barium fluoride.

The concentration of Al³⁺ in a saturated solution of Al(OH)₃ at 25°C is 5.2  10^-⁹ M. Calculate the K_sp for Al(OH)₃.

Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What major species is(are) present at point III?