Acid-Base Titration Lab

Acid-Base Titration Objectives 1. To titrate a hydrochloric irate solution of unknown concentration with like 0. 10M sodium hydroxide. 2. To utilize the titration data to cypher the molarity of the hydrochloric acid. Materials See handout for to a greater extent info. Procedure See handout for more than info. Data and Calculations Table 1 wad of NaOH Required to Neutralize 10. 00mL of Unknown HCl megabyte of NaOh Trial 1 Trial 2 Trial 3 Trial 4 Initial sight of NaOH(mL) 0. 0 11. 00 20. 85 30. 45 Final Volume of NaOH(mL) 11. 00 20. 85 30. 45 39. 98 Volume of NaOH used(mL) 11. 00 (Cancel out) 9. 85 9. 60 9. 53 Average Volume of NaOH = (9. 85+9. 60+9. 53)/3 = 9. 66mL model Calculations (9. 85+9. 60+9. 53)/3 = 9. 66mL The intermediate the great unwashed of NaOH used. Calculations 1. Moles NaOH = M x V = (0. 1M) (0. 00966L) = 0. 000966 moles 2. Moles HCl = moles NaOH 0. 000966 moles - 9. 6610-4 3. NaOH + HCl = NaCl + H2O Moles NaOH = M x V = (0. M)(0. 00966L) = 0. 000966 moles M oles HCl = moles NaOH HCl = moles/volumes = (0. 000966)/ (0. 0096L) HCl = 0. 1M Follow-up Questions 1. It result wee-wee no effect because the phenolphthalein only changes ruse depending on the pH level. Adding substances that will not change the pH level will have no effect. 2. We rinsed out the buret with NaOH, it is to neutralize any leftover acids that whitethorn have existed from previous experiments that the buret may have been used in. 4.When we added the NaOH, it instantly neutralize the HCl but because of HCl having more moles inside the beaker, the unneeded HCl instantly reverting the system patronize into a base. 5. HCl = 0. 1M pH = -logHCl pH = -log(0. 1M) pH = 1 Conclusion By utilise the titration data, we found out that the molarity of HCl is impact to the concentration of NaOH. This happens because the system is in a one-to-one relationship between the ii compounds. If we use the same amount of volume of HCl and NaOH, and mix the two, it will reach to a neu tral pH value.