11. Solutions in which the... a. [H3O+] is greater than 1 x 10-7 M are reacidic [Choose one: acidic, basic, or neutral] b. [H3O+] is less than 1 x 10-7 M are basic [Choose one: acidic, basic, or neutral] c. [OH-] is greater than 1 x 10-7 M are basic [Choose one: acidic, basic, or neutral] d. [OH-] is less than 1 x 107 M are acidic [Choose one: (acidic, basic, or neutral] e. [H3O+] is equal to 1 x 10-7 M are neutral [Choose one: acidic, basic, or neutral]
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.
Can you help me with number 11 part A, number 11 part B, number 11 part C, number 11 part D, and number 11 part E? Can you explain it to me?
![11. Solutions in which the...
a. [H3O+] is greater than 1 x 10-7 M are acidic [Choose one: acidic, basic, or neutral]
b. [H3O+] is less than 1 x 107 M are basic
c. [OH-] is greater than 1 x 10-7 M are basi
[Choose one: acidic, basic, or neutral]
[Choose one: acidic, basic, or neutral]
d. [OH-] is less than 1 x 10-7 M are acidic [Choose one: (acidic, basic, or neutral]
e. [H3O+] is equal to 1 x 10-7 M are neutral [Choose one: acidic, basic, or neutral]
12. What is the concentration of H3O* and OH- for each of the following conditions?
a. pH = 8.0 H₂0+] = 1x10 mm [0H-] = 1×10 m²
b. pH=6.50 [H₂07] =3.2 x10 m [@H] = 3.1X10³ m
-4
c. pH = 10.60
[H₂0t] = 2.5X10m [H] = 4₁0x10 m
13. If the pH> pKa in a buffer solution, which is larger, the concentration of the acid form or the
concentration of base form.
Bast form [A]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9a3eba95-76ad-4127-bd45-150147d91186%2F4ee693e1-9b4a-4c85-8de6-b8ed74df846e%2Fzkgla9s_processed.jpeg&w=3840&q=75)
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