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The iodide ion concentration in a solution may be determined by the precipitation of silver iodide. Ag+(aq)+I(aq)AgI(s) A student finds that 21.71mL of 0.7950M silver nitrate is needed to precipitate all of the iodide ion in a 10.00- mL sample of an unknown. What is the molarity of the iodide ion in the student's unknown? The concentration of H3AsO3 in a solution is determined by titrating it with a 0.1049MCe4t solution. The balanced net ionic equation for the reaction is: 2Ce4+(aq)+H3AsO3(aq)+5H2O(l)2Ce3+(aq)+H3AsO4(aq)+2H3O+(aq) In one experiment, 23.70mL of the 0.1049MCe41 solution is required to react completely with 25.00mLL of the H3AsO3 solution. Calculate the concentration of the H3AsO3 solution. Show. Tutar 5t+p) Consider the reaction between 72.8mL of 0.309MHClO4 and 40.9mL of 0.135MNaOH. Determine the concentration of H+and ions left over after the reaction goes to completion. HOW DO WE GET THERE? What is the amount of each reactant present in the solution? Write a net ionic equation for the overall reaction that occurs when aqueous solutions of ascorbic acid (H2C6H6O6) and sodium hydroxide are combined. Assume excess base. Be sure to specify states such as (aq) or (s)