Lab Investigations of Buffers I. Purpose The purpose of this experiment was to get an understanding as to how to properly prepare chemical buffers. Also part of this experiment was to gauge the effectiveness of the buffers by measuring their pH levels in various titration solutions, using a pH meter. II. Procedure To start our experiment we had to prepare Buffer B, which was the . 060 M Ammonia/Ammonium solution. Using 3. 0 M ammonia, we had to calculate the proper volume of NH base by using the MOVIE equation. Calculation: Using pipettes we measured out the needed volume and transferred it to an
Erlenmeyer flask, which we eventually used to combine the solution. We also had to calculate the grams of salt needed to make Buffer B. The salt we used was ammonium chloride (Enoch). The calculation below shows how we found the appropriate weight. We used a scooping utensil to collect the salt and used a weigh boat to hold and measure the mass. (The weight of the weigh boat was zeroed out prior to measuring the salt). Once we added the salt
Molecular Equation: CHICHI + Noah Mechanic + H2O omelet Ionic Equation: H + CHICHI + An + OH -+ An + CHICHI + H2O Net lento Equation: H + OH H2O d. Compare/Contrast Titration Results: Between . MM acetic acid/. MM acetate buffer & 0. 060 M acetic acid solution I Initial pH I Buffer Regions I Equiv. Points I Volvo. Of Base needed I Solution A 14. 56 1 peak=4. 241 9. Mol 1 16. Iron I solution D | 2. 97 | Peak= 4. 241 15. 0 ml | 24. 0 ml I 6. Solution E would be the least effective buffer because it did the worst Job of keeping the pH close to the initial PH. Solution E did not last as long in the titration as any of the other solutions.