To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid. Part A Sulfuric acid, H2SO4, is a strong acid. Its complete dissociation in aqueous solution is represented as Calculate the concentration of H* ions in a 0.010 mol L1 aqueous solution of sulfuric acid. H2SO4H + HSO4 Express your answer to three decimal places and include the appropriate units. A HSO4 anion can dissociate further by • View Available Hint(s) HSO, =H + SO,? but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as HẢ Ka, = = 0.012 х.10п HSO,] mol [H*] = 0,0145 • 10-1 1 Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Part B Calculate the concentration of SOQ ions in a 0.010 mol L aqueous solution of sulfuric acid. Express your answer to four decimal places and include the appropriate units. > View Available Hint(s) HẢ ? (SO,² ] = Value Units
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 with 1 images