Draw the graphic from Figure 15.12. Explain how it helps you calculate any of the values of [H3 O+ ], [OH- ], pH, pOH once the value of any one of them is kno
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.
Draw the graphic from Figure 15.12. Explain how it helps you calculate any of the values of
[H3 O+ ], [OH- ], pH, pOH once the value of any one of them is kno
![Figure 15.12 summarizes the ways we can interconvert [H*], [OH-],
pH, and pOH. The diagram may leave you wondering which path to
follow to make conversions, such as [OH-] to pH. Two equivalent sets
of calculations are shown: (i) [OH-] → pOH → pH or (ii) [OH¯] →
[H₂O¹] → pH. Using either results in the same answer.
pH
pH = -log[H3O+]
or
[H3O+] = 10¯pH
[H3O+] ←
pH = 14.00 – pOH
pOH = 14.00 - pH
Kw=1.00 × 10-1
- 14
pOH
=
pOH = -log[OH-]
or
[OH-] = 10-POH
[H3O+][OH-]
FIGURE 15.12 Pathways for interconverting [H₂O*], [OH-], pH, and pOH
values.
→ [OH-]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb034729f-db63-4235-9b33-79c3c77be50a%2F2c6aaebe-7e76-4a63-a822-4d2ea824fb8c%2Fwlpmyb_processed.png&w=3840&q=75)
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