1. Identify whether the following sets of acids and bases can function as a buffer solution. If the set can not be a buffer explain why. a. H2AsO4 and AsO43- b. H2O and Ca(OH)2 c. H2Se and KSeH d. HBrO2 and NaBrO3
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.
1. Identify whether the following sets of acids and bases can function as a buffer solution. If the set can not be a buffer explain why.
a. H2AsO4 and AsO43-
b. H2O and Ca(OH)2
c. H2Se and KSeH
d. HBrO2 and NaBrO3
2. A buffer was prepared by adding 12.00 g of Acetic acid, CH3COOH and 14.50 g of sodium acetate, CH3COONa to 250 mL of water. Ka = 1.8 x 10-5
a. Determine the pH of the buffer.
b. Determine the pH of the buffer after 16.50 mL of 2.00 M KOH was added
3. What mass of sodium benzoate, C6H5COONa should you add to 150 mL of a 0.15 M benzoic acid solution to obtain a buffer with a pH of 4.25? Ka = 6.5 x 10-5
4. Consider the titration of a 25.0 mL sample of 0.115 M RbOH with 0.225 M HCl.
a. Determine the initial pH of the RbOH solution.
b. Determine the milliliters of HCl needed to reach the equivalence point.
5. Determine the pH of a solution after mixing 60.0 mL of 0.250 M CH3COOH with 55.0 mL of 0.375 MKOH.Ka =1.8x10-5
6. Determine the pH of a solution after mixing 25.0 mL of 0.300 M CH3NH2 with 25.0 mL of 0.200 M HBr. Kb = 4.4 x 10-4
7. Determine the pH at the equivalence point when 20.0 mL of 0.606 M HBrO2 is mixed with 0.255 M NaOH. Ka = 1.2 x 10-5
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