Question: calculate the pH of 50.0 mL H20 + 1.00 mL 0.6 M NaOH (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00
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.
Question: calculate the pH of 50.0 mL H20 + 1.00 mL 0.6 M NaOH
(below is the data to answer the answer)
| Deionized water | Acetate Buffer | Ammonia Buffer | ||
| pH of solution | 6.62 | 4.59 | 9.49 | |
| Ph of solution after addition of 1 mL of 0.6 M NaOH | 12.41 | 4.71 | 9.50 | |
| pH of solution after addition of 1 mL of 0.6 M HCl | 1.38 | 3.87 | 9.24 | |
Preparation of Buffer solutions
Mass of sodium acetate in acetate buffer ~ 1.1981
Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81
Mass of ammonium chloride ~ 1.2721
Volume of 5.0 M NH4OH ~ 6.00
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 4 images
