k) Suppose your instructor handed you a bottle of sulfuric acid of unknown concentration. The chemistry department was considering using it for a summer program for elementary students to test rock samples to see if they contain limestone. However, they don't want to give it to the kids if it is too strong, and noone in the department was willing to drop some on their skin, and all the graduate students and TA's were already guinea pigs in other experiments, and the department did not want to compromise the data from that research in any way. So, the task falls to you, the eager undergraduate student.
(2 pts.) First, explain, using a chemical equation, and then describing it, how sulfuric acid could test for the presence of limestone. What specific reaction would be taking place, and what easily noticeable phenomenon would you be looking for when doing this test? Why?
[ii] (3 pts.) Suppose you take a 25.00 mL sample of this sulfuric acid solution. You then titrate it with a 0.1322 M potassium hyd
For titration with alkali you need to take such as phenolphthalein indicator. Titrating a solution of sulfuric acid is necessary to monitor the color of the solution. At the equivalence point it should become crimson.The process is explained by this: while potassium hydroxide solution was added dropwise, it neutralizes acid, which is in the same solution. after all of the acid neutralized, the solution is slightly alkaline environment and indicator changes color. To calculate the concentration of the acid the following formula can be applied: C2 = V1*C1/V2 C2 - acid concentration V2 - volume of acid C1 - concentration of alkali V1 - amount of potassium hydroxide used up to titrate.