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.
![Experiment 9.B
ACID-BASE TITRATION USING THE PH METER
Acids and bases react together to produce a salt and water. This reaction is called neutralization. The general
form of the reaction is the following:
HA + BOH →→→→→ B*A¯ + H₂O
Some specific examples are shown below:
HCI + NaOH → Naci + H₂O
HC] + NH4OH → NH4Cl + H₂O
HC₂H3O₂ + KOH
→ KC₂H₂O₂ + H₂O
→ NHÂNO3 + H₂O
HCHO, + NaOH
→ NaCHO₂ + H₂O
Titration is a method of very accurately determining the amount of one reagent needed to react with
another reagent. If these reagents are liquid, for example solutions of acid or base, then it is convenient to
measure the amounts by volume. Such a titration is called a volumetric titration.
HNO3 + NH4OH
One method of following the progress of an acid-base titration is by measuring the concentration of H*
or H3O* in the reaction flask. If a base is in the flask there will initially be a very low [H3O*]. As acid is added
to neutralize the base, the [H3O*]. increases. Just the opposite situation occurs if the flask initially contains
acid and base is being added.
The [H3O*] can be measured using a pH-meter, where pH is defined:
pH = -logio[H3O¹].
Therefore bases have high pH (low [H3O*]) and acids have low pH (high [H3O*]).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F89b1189c-c32b-4144-b592-a832138b3e54%2Fb64a5259-6bbe-4d63-9db0-57350f05691c%2Fxkfmk54_processed.jpeg&w=3840&q=75)
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