If you think carefully about what happens during the course of aweak acid–strong base titration, you can learn some very interestingthings. For example, let’s look back at Figure 17.9 and pretendyou did not know that acetic acid was the acid being titrated. Youcan figure out the pKa of a weak acid just by thinking about thedefinition of Ka and looking at the right place on the titrationcurve! Which of the following choices is the best way to do this? (a) At the equivalence point, pH = pKa. (b) Halfway to theequivalence point, pH = pKa. (c) Before any base is added,pH = pKa. (d) At the top of the graph with excess base added,pH = pKa.
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.
If you think carefully about what happens during the course of a
weak
things. For example, let’s look back at Figure 17.9 and pretend
you did not know that acetic acid was the acid being titrated. You
can figure out the pKa of a weak acid just by thinking about the
definition of Ka and looking at the right place on the titration
curve! Which of the following choices is the best way to do this?
(a) At the equivalence point, pH = pKa. (b) Halfway to the
equivalence point, pH = pKa. (c) Before any base is added,
pH = pKa. (d) At the top of the graph with excess base added,
pH = pKa.
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