Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. relative pH of 0.1 M aqueous solution species H,O 4 H,PO, 5 HNO2 (Choose one) NO, 7 OH (Choose one) HF (Choose one)
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.
![Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next
to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on.
Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure
water to the pH of the other solutions.
Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases.
relative pH of
0.1 M aqueous solution
species
H20
4
H,PO4
5
HNO2
(Choose one) ▼
NO,
7
ОН
(Choose one) ▼
HF
|(Choose one) ▼](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F668f7243-fecb-4dca-9846-a35dbaef67d8%2Fcea30f82-fd2a-4f93-a545-d8dd1235e1fe%2Fwwj7ji_processed.png&w=3840&q=75)
![H,PO4
(Choose one)
F
6](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F668f7243-fecb-4dca-9846-a35dbaef67d8%2Fcea30f82-fd2a-4f93-a545-d8dd1235e1fe%2Fe2hg97j_processed.png&w=3840&q=75)
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