Ch.15 - Acid and Base EquilibriumWorksheetSee 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

Solution: Answer the following questions dealing with the weak base ammonia.  A. Ammonia, NH3, is incredibly soluble in water. Why? B. Calculate the molarity and molality of a solution that is 30.0 g NH 3 in

Problem

Answer the following questions dealing with the weak base ammonia. 

A. Ammonia, NH3, is incredibly soluble in water. Why?

B. Calculate the molarity and molality of a solution that is 30.0 g NH 3 in 70.0 g water. The density of that solution is 0.982 g/mL. 

 

 

 

 

C. Consider the following solutions: 0.1 M NH 3(aq) and 0.1 M NaOH(aq).

Which solution has the highest osmotic pressure? ____________________________

Why?

 

Which solution has the highest boiling point? ____________________________ 

Why?

 

Which solution has the highest pH? ____________________________

Why?  

 

D. Calculate the pH of 0.1 M NH 3(aq). Kb of NH3 is 1.8 x 10-5 .