Chemistry Lab Report on standardization of acid and bases
Chemistry Lab Report on standardization of acid and bases.
Purpose: To prepare standardize solution of sodium hydroxide and to determine the concentration of unknown sulfuric acid solution. Data and Calculations: This experiment is divided into two parts (Part A and Part B). In the first part of experiment, the standardize solution of sodium hydroxide is prepared by titrating it with base Potassium hydrogen phthalate (KHP). The indicator Phenolphthalein is used to determine that whether titration is complete or not. PART A: Standardization of a Sodium Hydroxide solution NaOH Sample Code = O Trial 1 Mass of KHP transferred = 0.42 g Volume of Distilled water = 25 mL Volume of NaOH used = 22.50 mL Molar mass of KHP = 204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.42 g / 204.22 g/mol = 0.0021 moles Concentration of NaOH = No. of moles / Volume = [0.0021 mol / {(22.50 + 25) / 1000} L] * 100 = 4.4 M Trial 2 Mass of KHP transferred = 0.4139 g Volume of Distilled water = 25 mL Volume of NaOH used = 22.80 mL Molar mass of KHP = 204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.4139 g / 204.22 g/mol = 0.0020267 moles Concentration of NaOH = No. of moles / Volume = [0.0020267 mol / {(22.80 + 25) / 1000} L] * 100 = 4.24 M Trial 3 Mass of KHP transferred = 0.4239 g Volume of Distilled water = 25 mL Volume of NaOH used = 23.10 mL Molar mass of KHP = 204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.4239 g / 204.22 g/mol = 0.0020757 moles Concentration of NaOH = No. of moles / Volume = [0.0020757 mol / {(23.10 + 25) / 1000} L] * 100 = 4.32 M Trial 4 Mass of KHP transferred = 0.4311 g Volume of Distilled water = 25 mL Volume of NaOH used = 22.60 mL Molar mass of KHP = 204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.4311 g / 204.22 g/mol = 0.0021109 moles Concentration of NaOH = No. of moles / Volume = [0.0021109 mol / {(22.60 + 25) / 1000} L] * 100 = 4.43 M Table: Trail 1 Mass
Purpose: To prepare standardize solution of sodium hydroxide and to determine the concentration of unknown sulfuric acid solution. Data and Calculations: This experiment is divided into two parts (Part A and Part B). In the first part of experiment, the standardize solution of sodium hydroxide is prepared by titrating it with base Potassium hydrogen phthalate (KHP). The indicator Phenolphthalein is used to determine that whether titration is complete or not. PART A: Standardization of a Sodium Hydroxide solution NaOH Sample Code = O Trial 1 Mass of KHP transferred = 0.42 g Volume of Distilled water = 25 mL Volume of NaOH used = 22.50 mL Molar mass of KHP = 204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.42 g / 204.22 g/mol = 0.0021 moles Concentration of NaOH = No. of moles / Volume = [0.0021 mol / {(22.50 + 25) / 1000} L] * 100 = 4.4 M Trial 2 Mass of KHP transferred = 0.4139 g Volume of Distilled water = 25 mL Volume of NaOH used = 22.80 mL Molar mass of KHP = 204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.4139 g / 204.22 g/mol = 0.0020267 moles Concentration of NaOH = No. of moles / Volume = [0.0020267 mol / {(22.80 + 25) / 1000} L] * 100 = 4.24 M Trial 3 Mass of KHP transferred = 0.4239 g Volume of Distilled water = 25 mL Volume of NaOH used = 23.10 mL Molar mass of KHP = 204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.4239 g / 204.22 g/mol = 0.0020757 moles Concentration of NaOH = No. of moles / Volume = [0.0020757 mol / {(23.10 + 25) / 1000} L] * 100 = 4.32 M Trial 4 Mass of KHP transferred = 0.4311 g Volume of Distilled water = 25 mL Volume of NaOH used = 22.60 mL Molar mass of KHP = 204.22 g/mol No. of moles of KHP = Mass of KHP used / Molar mass = 0.4311 g / 204.22 g/mol = 0.0021109 moles Concentration of NaOH = No. of moles / Volume = [0.0021109 mol / {(22.60 + 25) / 1000} L] * 100 = 4.43 M Table: Trail 1 Mass