Separating Selected Metal Cations

Chemistry 266 Dominick Armstrong 10/10/2012 Acid-Base Titration Introduction Acid and bases ar two important classes of compounds that react to variety show a salt and water. When mixing acids and bases a precise amount of the base mustiness be tote uped in order to consider the par storey. At this period, one reactant has been incisively consumed by the addition of the other reactant. When execute chemical reactions chemist use a process called titration to line up the equivalence point of the reaction.Once the equivalence point is known hence chemist can correctly determine the amount the denseness of the acid and the base. In this experiment acid-base titration will be apply to determine the concentration of HCl at symmetry when it reacts with the NaOH H+ (aq)+ Cl- (aq) + Na+ (aq) + OH- H2O(l) + Na+ (aq)+ Cl- (aq) affair When performing this experiment one must first obtain and wear goggles. undermentioned add 40mL of distilled water to a 100mL beaker, accordingl y add 5. 00mL of HCl to the beaker. Then obtain 40mL of 0. 1M NaOH.Place the NaOH in a 60mL reagent reservoir and drain a small amount into a 250mL beaker to read the tip. Connect the Ph sensor to the LabQuest and bound up the drop counter. Then correct the titrant by adjusting the reservoir tip to and allow the NaOH slowly drain into a gradational cylinder until 9 or 1o ml has been recorded. After the LabQuest has been calibrated discard the solution. The call together the titration apparatus as shown in the motion picture below. Place the HCl solution onto the magnetic scaremonger and slowly titrate the NaOH into the solution.Start the data exhibition to calculate the intensity of NaOH is added when the solution reaches its equivalence point. Then right down the calculations and interrupt the apparatus. Discussion My lab grouping and I completed this experiment doing two discharges. We strand that both trials were concluded with similar results. In trial 1 we put up that the volume of NaOH added to the solution was 4. 01ml before the largest pH increase, and 4. 05mL after. We compute the volume at the equivalence point to be 4. 03mL. We found there were 4. 3&21510-4 moles of NaOH and 4. 03&21510-4 moles of HCl. Then we calculated the concentration of the HCl to be . 08 moles per liter. In trial 2 we found 4. 951mL of NaOH was added before the increase and 4. 992mL after. The volume at the equivalence point was 4. 971mL. There were 4. 971&21510-4 moles of HCl and 4. 971&21510-4 moles of NaOH. The concentration of HCl was found to be . 094 moles per liter. We found the bonny concentration to be . 08971M. Although the results of both trial in the experiment were similar the results were non exactly the same.The mistake may take away come from an error in measuring the HCl and distilled water. More HCl may have been added because we did not have an accurate pipet bulb. We employ a graduated cylinder to add the HCl, and may have had a much or less HCl than what was needed in the experiment. Conclusion The results of this experiment show that titration is an useful way to find the concentration of reactants in an acid base reaction. Using the titration helped my group accurately calculate the volume of NaOH that was added to the solution, and helped us to correctly determine the correct concentrations.