Can someone help with #3, #4, and the \"molarity of asprin\" section? My profess
ID: 978672 • Letter: C
Question
Can someone help with #3, #4, and the "molarity of asprin" section? My professor told me "to use the averages" because "my collected data was all over the place"- but I'm not sure where I use them!!
EXPERIMENTTITRATION OF A WEAK ACID determine the of a weak acid in a solution by titration with a known concentration of a strong baseTo calculate the mass of active material in a commercial tablet. DISCUSSION A quantitative technique determines how much of one or more components are present in a sample oft material. The two most common quantitative methods are volumetric and gravimetric analysis. Both analyses require a complete knowledge of the chemical reactions that occur between the unknown component analye) and known reactants reagents) The reaction between the analyte and the recent must be stoichiometric, quantitativeand complete. The reagent must react quickly with the analyse and the reaction must be specific, no side reactions can accur Volumetric analysis determines the concentration of an analyte by observing its reaction with a known quantity of standard reagentAnalyses are generally performed on liquid or aqueous solutionsThe most common method of volumetric analysis is titration. A titration determines the volume of standard reagent needed to react completely with a known volume of analyte. This reagent, called the titrantis a standard solution of known concentration. In a titration, the titrant is added to the analyte in small volume increments using a Baret. This method is based on a quantitative chemical reaction where I moles of titrant (n react with a modes of analyte A. St or water So in an ad - Products Theoretically, the end of a toration is reached when a stoichiometric equivalent amount of urant has been added to the analyte. This is called the equivalence point. Ideally, every titration the equivalence point, but in actuality, the end point is obtained. The end point is the experimental 1 of the stoichiometric equivalence of the titration. This point is indicated by a definite change in a physical or chemical property of the solution. In some titrationsthe change in color, ph, electrical of one of the reactants indicates the end point. In many citrationsan indicator is added to the solution being titrated. The indicator is designed to change color at the end point, thereby visually indicating the end of the titration. The difference between the end point and the equivalence point results in an error, called titration error. Choosing the best indicator and the most sensitive technique for determining a physical or chemical change can minimize this error The molar concentration of the analyte can be calculated from: (1) the volume of trant used to reach the (2) the molar concentration of the titrant(3) the volume of the analye, and (4) the stoichiometric ratio of the citrant to the analyte. The molar concentration of the analyte is given as: MLXV, In this experimentan acid base titration will be performed in which a weak aid of unknown concentration will be titrated with a standard solution of strong base. The weak acid is acetylsalicylic acid which is commonly known as aspirin. The strong base wased as the titrant is 00100 MN OHLThe weak acid and strong base react with one another to form a salt and water. HCHOA ag) + NaOHilag) NaCHOdaq) + HO) The end point of the titration can easily be detected by adding an acid-base indicator called phenolphthalein. The end point is observed when the solution changes from colorless to a faint pink that remains for 30 seconds. since the weak acid and base react with all mole ratio, the molarity of the acetylsalicylic acid can be calculated as: (M,Explanation / Answer
In the experiment, you have titrated weak acid (aspirin) with strong base (NaOH). But In the results of the titration, you are getting different values of NaOH used for neutralizing.
In point no. 3, you need to tell that what molarity of NaOH you used in the titration experiment.
In point no. 4, you need to tell that how much volume of aspirin you took for titration initially.
In point no. 5, you need to calculate the average molarity of aspirin. As your points are quite different from each other, so average is important. But before that, you need to calculate molarity of aspirin for each reading. That can be done by using following formula:
M1 V1 = M2 V2
On one side of this equation, you need to put parameters for NaOH and on the other you need to put for Aspirin. Suppose M1 and V1 are for NaOH and M2 and V2 are for aspirin. For NaOH, you know both the molarity of NaOH you took and the volume of NaOH used in titration. But for Aspirin, you only know the volume of aspirin you pipetted initally. So, you can calculate M2 as:
M2 = M1 V1 / V2
So, Just put these three values and you will get M2 for each reading, which is molarity of Aspirin for each reading.
Then you just need to take average of all the readings and that would be average molarity of aspirin.