Using the table of the weak base below, you have chosen Methylamine 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 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Kb Ammonia NH3 NH4+ 1.8 x 10-5 CH;NH,* 4.38 x 10-4 Methylamine CHẠNH, Ethylamine C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Aniline CH;NH, CH;NH;* 3.8 x 10-10 Pyridine C5H5N CH;NH* 1.7 x 10-⁹ 1. Compute the poH of the buffer solution. (answer in 2 decimal places)
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.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
