1. Calculate the pH of the following solutions: a. A solution prepared by mixing 30.0 mL of 2.0M NaOH with 300.0 mL of 0.55M formic acid. b. A solution prepared by adding 0.030 moles of HNO3 to 25.0 mL of 2.0M potassium carbonate c. 10.0 mL of 1.0 M HCl added to 50.0 mL of a solution that is 0.40M in both HF and NaF. d. 32 drops of 6.0M NaOH added to 40.0 mL of a solution that is 0.65M in acetic acid and 0.25M in calcium acetate. 20 drops = 1 mL
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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