Lareina the laboratory technician is given the task of making a solution containing HOBr (Ka=2.8×10−9) and KOBr and testing its behavior when strong acid or base is added to it. Part 1 First, Lareina combines 86.1 g KOBr and 250 mL of 1.45 M HOBr, and adds enough distilled water to make 800 mL of solution. What is the pH of this solution? pH solution = Part 2 Next, Lareina adds 12.0 mL of 2.20 M HNO3 to 360 mL of the solution made in Part 1. What is the pH of the solution after the HNO3 is added? pH after HNO3 added = Part 3 Finally, Lareina adds 10.0 mL of 2.20
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.
Lareina the laboratory technician is given the task of making a solution containing HOBr (Ka=2.8×10−9) and KOBr and testing its behavior when strong acid or base is added to it.
Part 1
First, Lareina combines 86.1 g KOBr and 250 mL of 1.45 M HOBr, and adds enough distilled water to make 800 mL of solution. What is the pH of this solution?
pH solution =
Part 2
Next, Lareina adds 12.0 mL of 2.20 M HNO3 to 360 mL of the solution made in Part 1. What is the pH of the solution after the HNO3 is added?
pH after HNO3 added =
Part 3
Finally, Lareina adds 10.0 mL of 2.20 M NaOH ito 365 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added?
pH after NaOH added =
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