Determine the pH of the following solutions, given that Ka (HF) = 6.8 x 10-4. Hint: 1. Diagnose the scenario (i.e. strong acid + weak base, etc.), 2. If buffer solution, make use of Henderson-Hasselback eqn and 3. If strong acid/base added to buffer, write out reaction with strong acid or base on the left hand side, then calculate ICE change. a. 0.5 moles of NaF b. A solution with 0.5 moles HF (Ka = 6.8 x 10^-4) and 0.5 moles NaF, to which 0.1 moles HCl is added.
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.
Determine the pH of the following solutions, given that Ka (HF) = 6.8 x 10-4.
Hint: 1. Diagnose the scenario (i.e. strong acid + weak base, etc.), 2. If buffer solution, make use
of Henderson-Hasselback eqn and 3. If strong acid/base added to buffer, write out reaction with
strong acid or base on the left hand side, then calculate ICE change.
a. 0.5 moles of NaF
b. A solution with 0.5 moles HF (Ka = 6.8 x 10^-4) and 0.5 moles NaF, to which 0.1 moles HCl
is added.
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