Ch.16 - Aqueous Equilibrium WorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Problem

1.00 g CH3NH3Cl (MW = 67.52 g/mol) and 1.00 g Ba(OH) 2∙8H2O (a strong base, MW = 315.47 g/mol) are added to 80 mL of water and dissolved. The resulting solution is diluted to 100 mL with water at 25°C.

Is this an acidic or basic buffer? Justify your answer.

A. neutral

B. acidic neutral

C. basic neutral

Solution

We are being asked to determine if the resulting solution is an acidic or basic buffer.


We will calculate the pH of the solution at the equivalence point using the following steps:

Step 1. Write the chemical equation for the reaction between CH3NH3Cl and Ba(OH)2.
Step 2. Calculate the initial amounts of CH3NH3Cl and Ba(OH)2 in moles before the reaction happens.
Step 3. Construct an ICF Chart.
Step 4. Calculate pH.


Step 1. Write the chemical equation for the reaction between CH3NH3Cl and Ba(OH)2.

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