On the report sheet, record the initial reading of the NaOH solution in the buret to the nearest Set up a ring stand with a buret clamp and place a clean buret in the buret clamp. Label a 250-mL beaker as “NaOH” and a 400-mL beaker as “Waste.” 2. 1. Add 2 drops of phenolphthalein indicator. d. Using a sample of KHP which has been contaminated with NaCl? The NaOH solution is standardized using the titration of a primary standard of KHP (Figure 2). 2. EXPERIMENT 7: ACID-BASE TITRATION: STANDARDIZATION 89 How to Record Buret Readings 1. Introduction Sodium hydroxide is hygroscopic and absorbs water from the air when you place it on the balance for massing. Calculate the number of moles of NaOH required to neutralize this amount of KHP. Swirl to dissolve the KHP completely. + NaOH + H 2 O KHP (MM = 204.2 g/mol) Equation 4 . Part I: Standardization of NaOH Solution (Use the data provided by your instructor) Trial 1 Trial 2 Trial 3 Mass of KHC5H404 0.1165 g 0.1697 g 0.1575 Moles of KHC5H.04 0.000820 mol 0.000831 mol 0.000770 mol Moles of NaOH 0.000820 mol 0.000831 mol 0.000770mol Buret Reading (final) 8.20 ml 16.25 ml 23.60 ml Buret Reading (initial) 0.00 ml 8.20 ml 16.25 ml Volume of NaOH used 8.20 ml. Part 2: Standardization of NaOH solution. After finding the mean of the concentration, the standard deviation was found to be 0.4. 1. (1 mark) 2. Calculate the number of moles of KHP in 25.00mL of standard solution. At your bench add about 50 ml of distilled water to KHP sample #1. PART II: Standardization of an Unknown NaOH Solution . D. STANDARDIZATION OF THE NaOH SOLUTION 1. ... Part I: Using KHP for Standardization 1. Standardization of a NaOH Lab ***There are sections for calculated values in this table. Standardization of a NaOH Solution with Potassium Hydrogen Phthalate (KHP) Objective You will determine the concentration (standardize) of an unknown solution of NaOH using the primary standard, potassium hydrogen phthalate. (note, KHP is a monoprotic acid; show all equations to explain) (2 marks) 3. Table 1: Standardization of Sodium Hydroxide Solution Mass of Pure KHP (g) Amount of NaOH used in titration (mL) Moles of KHP (mol) Concentration of NaOH in pure KHP (M) Trail 1 0.5244 33.4 0.078 2. The titration reaction of KHP with NaOH is as follows: Trial 2 0.5433 30.8 0.077 2. Title: Standardization of a NaOH Solution with Potassium Hydrogen Phthlate (KHP) Author: Currie(this one) Description: This lab has been generated by all members of the discipline but this one is K. Currie's … By knowing the masses of KHP, we can determine the number of moles used in the titration: At the equivalence point, then: moles NaOH = moles KHP Thus, the molarity of the NaOH solution is determined via the volume of the base used in the titration: Procedure: Part 1: Obtain 75-mL of approximate 0.1 M NaOH Obtain 75-mL of approximate 0.1 M NaOH. Conclusion: Write a 4-8 sentence conclusion in journal. You will be using the buret calibrated in Part 1 of this exercise and the data provided in Table 2 report the standardized concentration of the NaOH solution. Please make a separate table for those in the analysis section at the appropriate time. 1 4 KHP Standardization of NaOH web version 02-03.

standardization of naoh with khp conclusion

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