6. Compare the strengths of the following pairs of acids: a. HF and HBr b. H2SO4 versus H2SeO4, and H3PO4 versus H3ASO4 and C1O4H versus CIO₂H (trends with oxoacids)
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.
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Using the pKa of acetic acid/sodium acetate 4.74 and the equation pH = pKa + log[base]/
[acid] How many mL of sodium acetate will she need? What is the final
concentration (in molarity) of the sodium acetate and the acetic acid. Use this
information to prove that the student has correctly calculated the volume of sodium
acetate that she needs.
5. Calculate the concentrations of H+, HCO3-, and CO3-2- in a 0.025M H₂CO3 solution
6. Compare the strengths of the following pairs of acids:
a. HF and HBr
b. H2SO4 versus H2SeO4, and H3PO4 versus H3AsO4 and C1O4H versus CIO2H (trends
with oxoacids)
7. Calculate the pH of 0.10M Ammonia (NH3) Repeat the calculation after addition of 25
mL of 0.1M HCI.
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