Method 1: Convert [OH-] to [H3O+] first, then insert [H3O+] directly into the pH equation. Type your numeric answer and submit 1e1 Answered - Incorrect 1 attempt left Q15.37 • Unanswered. Method 2: Convert [OH-] to pOH, then convert pOH to pH. Type your numeric answer and submit × You are incorrect Resubmit Open
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.
![Step 5: Once [OH-] at equilibrium is known, we can use one of two ways to determine the pH of the weak
base, as covered in Section 15.4.
Q15.36
Method 1: Convert [OH-] to [H3O+] first, then insert [H3O+] directly into the pH equation.
1e1
• Answered.
Type your numeric answer and submit
Answered - Incorrect. 1 attempt left
Q15.37
• Unanswered.
Method 2: Convert [OH-] to pOH, then convert pOH to pH.
Type your numeric answer and submit
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![Step 4: Plug the equilibrium expressions into the equation for K and solve for x.
[OH Jeq[NH4*Jeq
Kb =
[NH3Jeg
=
x²
2
1.2 - X
Equation 15.30
x²
1.2-X
+²
Because K₁ <10-5, the method of successive approximations is worth a try:
=
x²
2
[NH3], -X
1.8 x 10-5
≈1.8x10-5
1.2
x=4.6 x 10-³ M = [OH Jeg
-3
Equation 15.31
0.05 x 1.2 M = 0.06 M > 4.6 x 10-³ M
=
Equation 15.32
1.8 x 10-5
Remember, when K is on the borderline value of ≈10-5, it's a good habit to check and see if x < 5% of the
initial concentration of the original molecule.
.. assumption is valid
K
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