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Calculate the pH at the following points in the titration of 25.00 ml of 0.250 M HNO3 with 0.250 M NaOH.  Before the addition of any NaOH After the addition of 10.00 ml of 0.250 M NaOH After the addition of 15.00 ml of 0.250 M NaOH sketch titration curve

Calculate the pH at the following points in the titration of 25.00 ml of 0.250 M HNO3 with 0.250 M NaOH.  Before the addition of any NaOH After the addition of 10.00 ml of 0.250 M NaOH After the addition of 15.00 ml of 0.250 M NaOH sketch titration curve

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Calculate the pH at the following points in the titration of 25.00 ml of 0.250 M HNO3 with 0.250 M NaOH. 

  1. Before the addition of any NaOH
  2. After the addition of 10.00 ml of 0.250 M NaOH
  3. After the addition of 15.00 ml of 0.250 M NaOH
  4. sketch titration curve
### Acid and Base Dissociation Constants and Solubility Product Constants #### Acid Dissociation Constants (Ka): - **HF:** \( K_a = 7.1 \times 10^{-4} \) - **HNO₂:** \( K_a = 4.5 \times 10^{-4} \) - **HCOOH (Formic Acid):** \( K_a = 1.7 \times 10^{-4} \) - **HC₃H₆O₃ (Lactic Acid):** \( K_a = 1.4 \times 10^{-4} \) - **CH₃CH₂COOH (Propionic Acid):** \( K_a = 1.3 \times 10^{-5} \) - **CH₃COOH (Acetic Acid):** \( K_a = 1.8 \times 10^{-5} \) - **C₆H₅COOH (Benzoic Acid):** \( K_a = 6.3 \times 10^{-5} \) - **HCN (Hydrocyanic Acid):** \( K_a = 4.9 \times 10^{-10} \) #### Base Dissociation Constants (Kb): - **CH₃NH₂ (Methylamine):** \( K_b = 4.4 \times 10^{-4} \) - **NH₃ (Ammonia):** \( K_b = 1.8 \times 10^{-5} \) - **C₅H₅N (Pyridine):** \( K_b = 1.7 \times 10^{-9} \) #### Solubility Product Constants (Ksp): - **PbCl₂ (Lead(II) Chloride):** \( K_{sp} = 1.7 \times 10^{-5} \) - **CuCl (Copper(I) Chloride):** \( K_{sp} = 1.9 \times 10^{-7} \) - **Mg(OH)₂ (Magnesium Hydroxide):** \( K_{sp} = 1.8 \times 10^{-11} \) ### Explanation: - **Acid Dissociation Constants (Ka):** These values indicate the strength of an acid in solution; larger values suggest stronger acids. - **Base Dissociation Constants (Kb):**
Transcribed Image Text:### Acid and Base Dissociation Constants and Solubility Product Constants #### Acid Dissociation Constants (Ka): - **HF:** \( K_a = 7.1 \times 10^{-4} \) - **HNO₂:** \( K_a = 4.5 \times 10^{-4} \) - **HCOOH (Formic Acid):** \( K_a = 1.7 \times 10^{-4} \) - **HC₃H₆O₃ (Lactic Acid):** \( K_a = 1.4 \times 10^{-4} \) - **CH₃CH₂COOH (Propionic Acid):** \( K_a = 1.3 \times 10^{-5} \) - **CH₃COOH (Acetic Acid):** \( K_a = 1.8 \times 10^{-5} \) - **C₆H₅COOH (Benzoic Acid):** \( K_a = 6.3 \times 10^{-5} \) - **HCN (Hydrocyanic Acid):** \( K_a = 4.9 \times 10^{-10} \) #### Base Dissociation Constants (Kb): - **CH₃NH₂ (Methylamine):** \( K_b = 4.4 \times 10^{-4} \) - **NH₃ (Ammonia):** \( K_b = 1.8 \times 10^{-5} \) - **C₅H₅N (Pyridine):** \( K_b = 1.7 \times 10^{-9} \) #### Solubility Product Constants (Ksp): - **PbCl₂ (Lead(II) Chloride):** \( K_{sp} = 1.7 \times 10^{-5} \) - **CuCl (Copper(I) Chloride):** \( K_{sp} = 1.9 \times 10^{-7} \) - **Mg(OH)₂ (Magnesium Hydroxide):** \( K_{sp} = 1.8 \times 10^{-11} \) ### Explanation: - **Acid Dissociation Constants (Ka):** These values indicate the strength of an acid in solution; larger values suggest stronger acids. - **Base Dissociation Constants (Kb):**
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