Determine the pH during the titration of 20.1 mL of 0.429 M hydrocyanic acid (K₂ = 4.0x10-10) by 0.359 M KOH at the following points. (a) Before the addition of any KOH (b) After the addition of 5.40 mL of KOH (c) At the half-equivalence point (the titration midpoint)

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**Title: Understanding pH Changes During Acid-Base Titration**

**Objective:**

Determine the pH during the titration of a solution containing 20.1 mL of 0.429 M hydrocyanic acid (HCN) by a 0.359 M KOH solution at specific points of the titration.

**Parameters:**
- Initial concentration of hydrocyanic acid (HCN): 0.429 M
- Volume of HCN: 20.1 mL
- Acid dissociation constant (Ka) of HCN: \(4.0 \times 10^{-10}\)
- Concentration of KOH: 0.359 M

**Points of Interest:**

(a) **Before the addition of any KOH:**  
Determine the initial pH of the hydrocyanic acid solution.

(b) **After the addition of 5.40 mL of KOH:**  
Calculate the pH after this specific volume of the base has been added.

(c) **At the half-equivalence point (titration midpoint):**  
Find the pH when half of the acid has been neutralized.

(d) **At the equivalence point:**  
Determine the pH at the point where the amount of added base equals the amount of acid originally present.

(e) **After the addition of 36.0 mL of KOH:**  
Calculate the pH after this entire volume of base has been added, well past the equivalence point.

**Note:** Calculating the pH at these points involves applying concepts from acid-base equilibria, stoichiometry, and the properties of weak acids and strong bases.
Transcribed Image Text:**Title: Understanding pH Changes During Acid-Base Titration** **Objective:** Determine the pH during the titration of a solution containing 20.1 mL of 0.429 M hydrocyanic acid (HCN) by a 0.359 M KOH solution at specific points of the titration. **Parameters:** - Initial concentration of hydrocyanic acid (HCN): 0.429 M - Volume of HCN: 20.1 mL - Acid dissociation constant (Ka) of HCN: \(4.0 \times 10^{-10}\) - Concentration of KOH: 0.359 M **Points of Interest:** (a) **Before the addition of any KOH:** Determine the initial pH of the hydrocyanic acid solution. (b) **After the addition of 5.40 mL of KOH:** Calculate the pH after this specific volume of the base has been added. (c) **At the half-equivalence point (titration midpoint):** Find the pH when half of the acid has been neutralized. (d) **At the equivalence point:** Determine the pH at the point where the amount of added base equals the amount of acid originally present. (e) **After the addition of 36.0 mL of KOH:** Calculate the pH after this entire volume of base has been added, well past the equivalence point. **Note:** Calculating the pH at these points involves applying concepts from acid-base equilibria, stoichiometry, and the properties of weak acids and strong bases.
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