For NH4Cl and NaCH3COO, perform the following calculations: 1. Calculate [H3O+] using the equation below and the given pH values in Table 7b-1. 2. Calculate [OH-] using any of the equations below. [H3O+][OH-] = Kw = 1.00 × 10-14 OR pOH = 14 – pH [OH-] = 10-pOH 3. Construct an ICE table for the hydrolysable ion. 4. Calculate Kh using the equations below, whichever is applicable. If the ion is a conjugate acid of a weak base, then Kh = Ka. If the ion is a conjugate base of a weak acid, then Kh = Kb. Ka = weak base H3O+[cation or conjugate acid] 5. Calculate Ki using the given equation. If Kh = Ka, then Ki = Kb. If Kh = Kb, then Ki = Ka.
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.
For NH4Cl and NaCH3COO, perform the following calculations:
1. Calculate [H3O+] using the equation below and the given pH values in Table 7b-1.
2. Calculate [OH-] using any of the equations below.
[H3O+][OH-] = Kw = 1.00 × 10-14 OR
pOH = 14 – pH
[OH-] = 10-pOH
3. Construct an ICE table for the hydrolysable ion.
4. Calculate Kh using the equations below, whichever is applicable.
If the ion is a conjugate acid of a weak base, then Kh = Ka.
If the ion is a conjugate base of a weak acid, then Kh = Kb.
Ka = weak base H3O+[cation or conjugate acid]
5. Calculate Ki using the given equation.
If Kh = Ka, then Ki = Kb.
If Kh = Kb, then Ki = Ka.
KiKh = Kw
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For NH4Cl and NaCH3COO, perform the following calculations:
1. Calculate [H3O+] using the equation below and the given pH values in Table 7b-1.
2. Calculate [OH-] using any of the equations below.
[H3O+][OH-] = Kw = 1.00 × 10-14 OR
pOH = 14 – pH
[OH-] = 10-pOH
3. Construct an ICE table for the hydrolysable ion.
4. Calculate Kh using the equations below, whichever is applicable.
If the ion is a conjugate acid of a weak base, then Kh = Ka.
If the ion is a conjugate base of a weak acid, then Kh = Kb.
Ka = weak base H3O+[cation or conjugate acid]
5. Calculate Ki using the given equation.
If Kh = Ka, then Ki = Kb.
If Kh = Kb, then Ki = Ka.
KiKh = Kw
but only 4 &5
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