**Calculate the pH when 45.0 mL of 0.200 M HBr is mixed with 43.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 × 10⁻⁴).**This problem involves a reaction between hydrobromic acid (HBr), a strong acid, and methylamine (CH₃NH₂), a weak base. The goal is to determine the pH of the resulting solution after the acid-base reaction.**Conceptual Steps to Solve the Problem:**1. **Calculate moles of HBr and CH₃NH₂**: - Use the formula: moles = molarity × volume (L). 2. **Determine the limiting reactant**: - This will be the reactant that is completely consumed in the reaction. 3. **Calculate the amount of CH₃NH₃⁺ formed**: - The reaction between HBr and CH₃NH₂ will form the conjugate acid CH₃NH₃⁺.4. **Calculate the pH**: - If there is an excess of strong acid, use it to find the pH directly. - If the base is in excess, calculate the concentration of CH₃NH₃⁺ and use it to determine the pH of the solution considering the hydrolysis of CH₃NH₃⁺.### Additional Information:- **Equilibrium Calculations** may be required if there is a significant concentration of the weak base or its conjugate acid.- **pH determination of weak acid salts** involves using the relationship between Ka and Kb: - \( K_w = K_a \times K_b \) - \( K_a = \frac{K_w}{K_b} \) for weak base conjugates.This is an acidity/basicity determination problem that involves stoichiometry, the concept of limiting reactions, and equilibrium. Perfect for chemistry students studying acid-base reactions and pH calculations.

pH of mixture =? Volume of HBr = 45.0 mL = 0.045 L Concentration of HBr = 0.200 M Volume of CH3NH2 =…

Answered: Calculate the pH when 45.0 mL of 0.200…

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Calculate the pH when 45.0 mL of 0.200 M HBr is mixed with 43.0 mL of 0.400 M CH:NH2 (Kb = 4.4 × 104).

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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

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Question

**Calculate the pH when 45.0 mL of 0.200 M HBr is mixed with 43.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 × 10⁻⁴).**

This problem involves a reaction between hydrobromic acid (HBr), a strong acid, and methylamine (CH₃NH₂), a weak base. The goal is to determine the pH of the resulting solution after the acid-base reaction.

**Conceptual Steps to Solve the Problem:**

1. **Calculate moles of HBr and CH₃NH₂**:
- Use the formula: moles = molarity × volume (L).

2. **Determine the limiting reactant**:
- This will be the reactant that is completely consumed in the reaction.

3. **Calculate the amount of CH₃NH₃⁺ formed**:
- The reaction between HBr and CH₃NH₂ will form the conjugate acid CH₃NH₃⁺.

4. **Calculate the pH**:
- If there is an excess of strong acid, use it to find the pH directly.
- If the base is in excess, calculate the concentration of CH₃NH₃⁺ and use it to determine the pH of the solution considering the hydrolysis of CH₃NH₃⁺.

### Additional Information:
- **Equilibrium Calculations** may be required if there is a significant concentration of the weak base or its conjugate acid.
- **pH determination of weak acid salts** involves using the relationship between Ka and Kb:
- \( K_w = K_a \times K_b \)
- \( K_a = \frac{K_w}{K_b} \) for weak base conjugates.

This is an acidity/basicity determination problem that involves stoichiometry, the concept of limiting reactions, and equilibrium. Perfect for chemistry students studying acid-base reactions and pH calculations.

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