Experiment 17 Determination of the Content of Borax 1. To know the application of acid-base titration. 2. To master the technology of titration and how to determine the end point of the titration. Borax (sodium borate Na2B4O7·10H2O) is soluble in water and produces Na+ and B4O72- ions. According to Brönsted definition B4O72- is a proton acceptor. It takes protons from water molecules and thus is a base. Therefore, the quantity of borax can be determined through acid-base titration. B4O72- + 7H2O = H3BO3 + 2OHWhen standard hydrochloric acid solution is used to titrate borax solution, the following reaction takes place: Na2B4O7·10H2O + 2HCl = 2NaCl + 4H3BO3 + 5H2O According to the equations above, at stoichiometric point, we have the following equations: n(HCl) = n(Na2B4O7·10H2O) Borax(%) = c(HCl) V (HCl) M ( Na 2 B4O7 ·10H 2O) 100% msample 2 1000 1. Preparation of Borax Solution 称量瓶:weighing bottle 硼砂: borax 分析天平:analytical balance 烧杯: beaker 1.9-2.1g of borax (±0.0001g precisely) →100mL 搅拌: stirring 玻璃棒: glass rod 刻度线: calibration mark Adding distilled water 2. Preparation of 0.1 mol/L HCl solution 300 mL Calculate the volume of concentrated HCl V(concentrated HCl) = ? mL? 量筒:measuring cylinder Adding distilled water to 300mL 3. Preparation of standard solution of Na2CO3 无水碳酸钠: anhydrous sodium carbonate 刻度线: calibration mark 1.2g~1.4g (±0.0001g precisely) Na2CO3 →250mL Adding distilled water 4. Standardization the concentration of HCl solution with anhydrous sodium carbonate HCl solution beforet itration : yellow The end of titration: orange 20.00mL Na2CO3 standard solution 2 drops of methyl orange indicator 5. Determination of the Content of Borax HCl solution beforet itration : yellow the endpoint of the titration : orange 20.00mL borax solution 2 drops of methyl red indicator