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Learning Goal: To learn about titration types and how to calculate pH at different points of titration. In an acid-base titration, titrant (solution of a base or acid) is added slowly to an analyte (solution of an acid or base). The titration is often monitored using a pH meter. A plot of pH as a function of the volume of titrant added is called a pH titration curve. Prior to the titration, the pH is determined by the concentration of the analyte. When the titrant. added, it begins to neutralize the analyte. The decrease in the analyte concentration changes the pH. At the equivalence point, equivalent quantities of acid and base have been mixed together such that the acid-base reaction is complete, and the pH is determined by the product. At 25°C: in the case of a strong acid-strong base titration, the salt formed is neutral and pH = 7: in a weak acid-strong base titration, a basic salt is produced and pH > 7: and in a weak base-strong acid titration, the salt is acidic and pH <7. After the equivalence point, the pH is determined by the concentration of excess titrant. Note: For simplicity and clarity, assume thoughout this item that the temperature is 25°C. Part A Identify each type of titration curve. Note that the analyte is stated first, followed by the titrant. Drag each graph to the appropriate bin.. View Available Hint(s) ml. of titrant Strong acid-strong base ml. of titrant Weak acid-strong base mL of titrant Weak base-strong acid ml of titrant Reset Help Polyprotic acid-strong base

Learning Goal: To learn about titration types and how to calculate pH at different points of titration. In an acid-base titration, titrant (solution of a base or acid) is added slowly to an analyte (solution of an acid or base). The titration is often monitored using a pH meter. A plot of pH as a function of the volume of titrant added is called a pH titration curve. Prior to the titration, the pH is determined by the concentration of the analyte. When the titrant. added, it begins to neutralize the analyte. The decrease in the analyte concentration changes the pH. At the equivalence point, equivalent quantities of acid and base have been mixed together such that the acid-base reaction is complete, and the pH is determined by the product. At 25°C: in the case of a strong acid-strong base titration, the salt formed is neutral and pH = 7: in a weak acid-strong base titration, a basic salt is produced and pH > 7: and in a weak base-strong acid titration, the salt is acidic and pH <7. After the equivalence point, the pH is determined by the concentration of excess titrant. Note: For simplicity and clarity, assume thoughout this item that the temperature is 25°C. Part A Identify each type of titration curve. Note that the analyte is stated first, followed by the titrant. Drag each graph to the appropriate bin.. View Available Hint(s) ml. of titrant Strong acid-strong base ml. of titrant Weak acid-strong base mL of titrant Weak base-strong acid ml of titrant Reset Help Polyprotic acid-strong base

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 108QRT
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+ Titrations Learning Goal: To learn about titration types and how to calculate pH at different points of titration. Part A In an acid-base titration, a titrant (solution of a base or acid) is added slowly to an analyte (solution of an acid or base). The titration is often monitored using a pH meter. A plot of pH as a function of the volume of titrant added is called a pH titration curve. Prior to the titration, the pH is determined by the concentration of the analyte. When the titrant is added. begins to neutralize the analyte. The decrease in the analyte concentration changes the pH. At the equivalence point, equivalent quantities acid and base have been mixed together such that the acid-base reaction is complete, and the pH is determined by the product. At 25°C: in the case of a strong acid-strong base titration, the salt formed is neutral and pH = 7: in a weak acid-strong base titration, a basic salt is produced and pH > 7; and in a weak base-strong acid titration, the salt is acidic and pH <7. After the equivalence point, the pH is determined by the concentration of excess titrant. Note: For simplicity and clarity, assume thoughout this item that the temperature is 25°C. Identify each type of titration curve. Note that the analyte is stated first, followed by the titrant. Drag each graph to the appropriate bin. ▸ View Available Hint(s) mL of titrant Strong acid-strong base mL of titrant Weak acid-strong base M mL of titrant Polyprotic acid-strong base mL of titrant Reset Help Weak base-strong acid 24 of 39 Review | Constants | Periodic Table
Transcribed Image Text:+ Titrations Learning Goal: To learn about titration types and how to calculate pH at different points of titration. Part A In an acid-base titration, a titrant (solution of a base or acid) is added slowly to an analyte (solution of an acid or base). The titration is often monitored using a pH meter. A plot of pH as a function of the volume of titrant added is called a pH titration curve. Prior to the titration, the pH is determined by the concentration of the analyte. When the titrant is added. begins to neutralize the analyte. The decrease in the analyte concentration changes the pH. At the equivalence point, equivalent quantities acid and base have been mixed together such that the acid-base reaction is complete, and the pH is determined by the product. At 25°C: in the case of a strong acid-strong base titration, the salt formed is neutral and pH = 7: in a weak acid-strong base titration, a basic salt is produced and pH > 7; and in a weak base-strong acid titration, the salt is acidic and pH <7. After the equivalence point, the pH is determined by the concentration of excess titrant. Note: For simplicity and clarity, assume thoughout this item that the temperature is 25°C. Identify each type of titration curve. Note that the analyte is stated first, followed by the titrant. Drag each graph to the appropriate bin. ▸ View Available Hint(s) mL of titrant Strong acid-strong base mL of titrant Weak acid-strong base M mL of titrant Polyprotic acid-strong base mL of titrant Reset Help Weak base-strong acid 24 of 39 Review | Constants | Periodic Table
+ Titrations Part B A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 13.0 mL of KOH. Express your answer numerically. ▸ View Available Hint(s) pH = Submit Part C pH = A 75.0-mL volume of 0.200 M NH3 (Kb 1.8 x 10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 17.0 mL of HNO3. Express your answer numerically. ▸ View Available Hint(s) Submit |V | ΑΣΦ Part D |VD ΑΣΦ 6 |VD ΑΣΦ 6 A 52.0-mL volume of 0.35 M CH3COOH (Ka 1.8 x 10-5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 21.0 mL of NaOH. Express your answer numerically. ▸ View Available Hint(s)
Transcribed Image Text:+ Titrations Part B A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 13.0 mL of KOH. Express your answer numerically. ▸ View Available Hint(s) pH = Submit Part C pH = A 75.0-mL volume of 0.200 M NH3 (Kb 1.8 x 10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 17.0 mL of HNO3. Express your answer numerically. ▸ View Available Hint(s) Submit |V | ΑΣΦ Part D |VD ΑΣΦ 6 |VD ΑΣΦ 6 A 52.0-mL volume of 0.35 M CH3COOH (Ka 1.8 x 10-5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 21.0 mL of NaOH. Express your answer numerically. ▸ View Available Hint(s)
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