Consider a buffer solution that contains 0.40 M C6H4(CO2H)2 and 0.25 M C6H4(CO2H)(CO2K). pKa(C6H4(CO2H)2)=2.95. Calculate its: a)pH, the change in pH if 0.160 g of solid NaOH is added to 200 mL of this solution.
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.
Consider a buffer solution that contains 0.40 M C6H4(CO2H)2 and 0.25 M C6H4(CO2H)(CO2K). pKa(C6H4(CO2H)2)=2.95.
Calculate its:
a)pH, the change in pH if 0.160 g of solid NaOH is added to 200 mL of this solution.
b)If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
