2. The weak acid hypochlorous acid (HClO) is formed in bleach solutions. If the pH of a 0.12 M solution of HClO is 4.19, what is the value of the Ka of this weak acid? 3. Calculate the % dissociation of a 0.0100 M HCN (hydrocyanic acid) solution. Ka=6.20 × 10–10. 4. Calculate the OH– concentration & pOH of a 0.075 M NH3 solution (Kb=1.75 × 10–5).
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.
2. The weak acid hypochlorous acid (HClO) is formed in bleach solutions. If the pH of a 0.12 M solution of
HClO is 4.19, what is the value of the Ka of this weak acid?
3. Calculate the % dissociation of a 0.0100 M HCN (hydrocyanic acid) solution. Ka=6.20 × 10–10.
4. Calculate the OH– concentration & pOH of a 0.075 M NH3 solution (Kb=1.75 × 10–5).
5. Calculate the pH of 0.10 M (COOH)2 (aq), oxalic acid. Ka1 = 5.9 × 10–2 ; Ka2 = 6.4 × 10–5.
6. Calculate the pH of a 0.055 M AlCl3 (aq) (aluminum chloride) solution. Ka for Al3+ is 1.2 × 10–5.
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