the value of ki to calculate Use [H₂OJ Calculate [M30+ that would result from [H3O+] Ki for HX= 3.3 × 10 -4 [H₂O*] and [OH-] and % ionization solution of HX When of solution it is [04²] = 2x10] 3.4 moles of HX Found to calculate the finment concertade -10 Calculate ki for Hox C13₂031043=1*10* a .41m is dissolved at equilibrium that in I Liker
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.
![Use
[HOJ
Are value of ki to calculate the final concertade
сана
T
Calculate [H3O+] that would result
solution of HX
When
of solution
[04] = 2x10
from
ki for HX= 3.3 × 10-4
[H3O+] and [OH-] and % iomization
3.4 moles of
it is
-10
Calculate
of HX
is
dissolved
found at equilibrium that
ki for HX
14
a
[1₂0*31043=1×10
.41m
in I Liker](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffd4c8a78-94ed-40f4-97b5-ac0eacd4f1aa%2F6e8bc4c6-d140-4394-993f-3001b4f6927b%2Fpn1llro_processed.jpeg&w=3840&q=75)
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