3. A solution is 0.5 M NH4OCl. a. Determine the major species in this solution. b. Identify the strongest acid and strongest base in the solution and write the equilibrium reaction between these two. c. Calculate the equilibrium constant for the reaction in (b) using the equilibrium constants from Table 14.2 and 14.3 in your textbook.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
3. A solution is 0.5 M NH4OCl.
a. Determine the major species in this solution.
b. Identify the strongest acid and strongest base in the solution and write the equilibrium reaction between these two.
c. Calculate the equilibrium constant for the reaction in (b) using the equilibrium constants from Table 14.2 and 14.3 in your textbook. Note that the reaction for the autodissociation of water may also be helpful here.
d. Calculate the equilibrium concentrations of NH4 + , NH3, HOCl, and OCl- .
e. Use the equilibrium constant(s) from (c) to calculate the pH of the solution.
f. This problem generally reads “Calculate the pH of a 0.5 M NH4OCl solution.” Recap in general terms the steps taken to solve this problem.
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