ine the [H+] in a solution prepared by dissolving 3.0g of nicotinic acid (MM=123.11 g/mol),HNic, in enough water to form 245ml of solution. 2) Calculate [H+] in a 0.100M 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.
Nicotinic acid, HC6H4O2N (Ka=1.4 x 10-5), is another name for niacin, an important member of the vitamin B group. Determine the [H+] in a solution prepared by dissolving 3.0g of nicotinic acid (MM=123.11 g/mol),HNic, in enough water to form 245ml of solution.
2) Calculate [H+] in a 0.100M solution of nitrous acid, HNO2, for which Ka = 6.0 x 10-4
3) The distilled water you use in the laboratory is slightly acidic because of dissolved CO2, which reacts to form carbonic acid, H2CO3. Calculate the pH of a0.0010M solution of H2CO3 and [CO32-] at equilibrium.
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
