The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a/ Determine the concentration of [OH] in the solution. b/ Write the expression for the Kb of NaCH3COO (aq) and calculate its values. c/ Calculate the pKa of CH3COOH.
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.
![The pH of a 1.00 M NaCH3COO (aq) solution is 9.38.
a/ Determine the concentration of [OH] in the solution.
b/ Write the expression for the Kb of NaCH3COO (aq) and calculate its values.
c/ Calculate the pKa of CH3COOH.
d/ HCI (aq) is added to 1.00 L solution of 1.00 M NaCH3CO0 (aq). Write the chemical reaction
between HCI (aq) and NaCH3COO (aq).
e/ How many mol of HCI (aq) is needed to make a buffer solution with pH = 5.00 from 1.00 L of 1.00
M NaCH3COO (aq).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa8ec82fe-f381-4cdb-86a9-4b343a3eed40%2Fb739c151-216a-4b7e-b856-05d54d7cb084%2Fhymgw_processed.png&w=3840&q=75)
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