**Buffer Preparation and pH Calculation****Scenario:**Consider a buffer made by adding 42.3 g of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH.**Given:**- The base dissociation constant (Kb) for (CH₃)₂NH is 5.4 x 10⁻⁴.**Question:**What is the pH of the buffer after 0.300 mol of H⁺ have been added?**Steps for Calculation:**1. **Determine the Moles of Each Component:** - Calculate moles of (CH₃)₂NH₂I using its molar mass. - Calculate initial moles of (CH₃)₂NH using its concentration and volume.2. **Buffer Reaction:** - Consider the buffer reaction between (CH₃)₂NH and added H⁺ ions. - Adjust the moles of components based on the reaction with H⁺.3. **Utilize the Henderson-Hasselbalch Equation:** - Use the pKb to find the pKa. - Apply the equation to find the pH of the buffer solution after the addition of H⁺ ions. This problem involves using concepts of buffer solution chemistry and equilibrium constants to calculate the resulting pH when an acid is introduced to the system.

A buffer is made of a weak base and salt of that base. When an acid is added to the buffer, the base…

Answered: Consider a buffer made by adding 42.3 g…

Consider a buffer made by adding 42.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)»NH (Kb = 5.4 x 10 4) What is the pH of the buffer after 0.300 mol of Ht have been added?

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

Section: Chapter Questions

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Question

**Buffer Preparation and pH Calculation**

**Scenario:**
Consider a buffer made by adding 42.3 g of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH.

**Given:**
- The base dissociation constant (Kb) for (CH₃)₂NH is 5.4 x 10⁻⁴.

**Question:**
What is the pH of the buffer after 0.300 mol of H⁺ have been added?

**Steps for Calculation:**

1. **Determine the Moles of Each Component:**
- Calculate moles of (CH₃)₂NH₂I using its molar mass.
- Calculate initial moles of (CH₃)₂NH using its concentration and volume.

2. **Buffer Reaction:**
- Consider the buffer reaction between (CH₃)₂NH and added H⁺ ions.
- Adjust the moles of components based on the reaction with H⁺.

3. **Utilize the Henderson-Hasselbalch Equation:**
- Use the pKb to find the pKa.
- Apply the equation to find the pH of the buffer solution after the addition of H⁺ ions.

This problem involves using concepts of buffer solution chemistry and equilibrium constants to calculate the resulting pH when an acid is introduced to the system.

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