A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 × 10¬1º. 1 2 3 NEXT > Let x represent the original concentration of C6H;NH3* in the water. Based on the given values, set up the ICE table in order to determine the unknown. C6H;NH2(aq) + H20(1) = OH (aq) +C6H5NH;*(aq) Initial (M) |Change (M) Equilibriu m (M). RESET 0.50 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 - 1.6 x 10-10 -1.6 x 10-10 3.8 x 1010 -3.8 x 10-10 x + 4.20 x - 4.20 x+ 6.3 x 10-5 x - 6.3 x 10-5 x + 1.6 x 10-10 x - 1.6 x 1010 x + 3.8 x 10"10 x - 3.8 x 1010
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.
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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.
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