Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Kb NH4+ 1.8 x 10-5 Ammonia Methylamine NH3 CH3NH2 CH3NH3+ 4.38 x 10-4 C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Ethylamine Aniline CH;NH, C6H5NH3+ Pyridine 3.8 x 10-10 1.7 x 10-⁹ C,H,N CH;NH* 1. Compute the poH of the buffer 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.
please answer in full decimal places
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
