Labs
Standard Solution (Part A and B)
ABSTRACT The purpose of this experiment is to prepare a standard solution of potassium hydrogen phthalate and use titration to perform an acid/base reaction between the potassium hydrogen phthalate and sodium hydroxide to standardize approximately 0.10 M sodium hydroxide solution. To prepare the Potassium Hydrogen phthalate, a 2.00 grams of KHP was measured to an accurate measurement of 1.980 grams. A total of 100 mL of water was mixed with the KHP solution in the volumetric flask to finally prepare an acidic KHP solution. The molar mass of KHP was calculated and came to be 208.252 grams per mole. To find the moles of KHP, the mass of KHP (1.980 g) was divided by the molar mass of KHP ( 208.252 g) and .00951 moles are in the 1.980 grams of KHP. To find the molarity, the number of moles of KHP (.00951 moles) was divided by the volume of water in liters (.100 L) giving an answer of 0.0951 M. The second part of the experiment is the reaction of acid/base through titration. The acid, KHP, was placed in one burette while 100 mL of base, stock solution of NaOH, was placed in another burette. 25 mL of KHP was placed into the Erlenmeyer flask, which was also recorded as the volume of acid in the flask. A total of 19 mL of base, NaOH, was required for the endpoint, which was indicated by a very pale pink color. To calculate the molarity of NaOH, the following equation was used MNaOH x VNaOH = MKHP x VKHP therefore the molarity was .125 M.
INTRODUCTION
This lab experiment covers the preparation of standard solution and the acid/base titration. The first part of the lab is to prepare a standard solution of Potassium hydrogen per. A standard solution is a solution of known concentration, in which it is prepared using exacting techniques to make sure that the molarity is to the highest accuracy. The stock solution on the other hand, which is also a base in this experiment, is a large volume of a common reagent prepared
ABSTRACT The purpose of this experiment is to prepare a standard solution of potassium hydrogen phthalate and use titration to perform an acid/base reaction between the potassium hydrogen phthalate and sodium hydroxide to standardize approximately 0.10 M sodium hydroxide solution. To prepare the Potassium Hydrogen phthalate, a 2.00 grams of KHP was measured to an accurate measurement of 1.980 grams. A total of 100 mL of water was mixed with the KHP solution in the volumetric flask to finally prepare an acidic KHP solution. The molar mass of KHP was calculated and came to be 208.252 grams per mole. To find the moles of KHP, the mass of KHP (1.980 g) was divided by the molar mass of KHP ( 208.252 g) and .00951 moles are in the 1.980 grams of KHP. To find the molarity, the number of moles of KHP (.00951 moles) was divided by the volume of water in liters (.100 L) giving an answer of 0.0951 M. The second part of the experiment is the reaction of acid/base through titration. The acid, KHP, was placed in one burette while 100 mL of base, stock solution of NaOH, was placed in another burette. 25 mL of KHP was placed into the Erlenmeyer flask, which was also recorded as the volume of acid in the flask. A total of 19 mL of base, NaOH, was required for the endpoint, which was indicated by a very pale pink color. To calculate the molarity of NaOH, the following equation was used MNaOH x VNaOH = MKHP x VKHP therefore the molarity was .125 M.
INTRODUCTION
This lab experiment covers the preparation of standard solution and the acid/base titration. The first part of the lab is to prepare a standard solution of Potassium hydrogen per. A standard solution is a solution of known concentration, in which it is prepared using exacting techniques to make sure that the molarity is to the highest accuracy. The stock solution on the other hand, which is also a base in this experiment, is a large volume of a common reagent prepared