utorial Problem for Weak Base and Strong Acid ou are given an Erlenmeyer flask containing 100.00 mL of 0.100 M B and a buret containing 0.100 M HCI. B" is a weak acid with a K, of 5.9 x 10-6. Calculate the pH of the solution (to 2 decimal laces) after titrating the following volumes of HCI: Vhat is the pH after 0.0 mL HCI is added? 40M t this point no strong acid has been added, so you need to solve a weak base pH problem. Vhat volume of HCI is added at the equivalence point (to 0.1 mL)? 49 Vhat is the pH at the equivalence point? 40D t this point no strong acid or weak base remains, so you need to solve a weak acid pH problem for the weak base's conjugate acid. mL Vhat is the pH after 50.0 ml HCI is added? 40 ou are in the buffer region here. You need to find the relative ratio of [B-1/[HB]. Make sure to convert K, into K, before using the Henderson-Hasselbalch equation. Vhat is the pH after 150.0 mL HCI is added? 49 ou are in a region where both the weak conjugate acid and strong acid are present, so you need to solve a strong acid pH problem.
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.
Step by step
Solved in 3 steps with 2 images