Calculate the volume of 6.00 M NaoH that is needed to prepare 250mL of an approximately 0.100 M NaOH solution. Transfer the calculated volume of the 6.00 M NaOH solution to a volumetric flask using a graduated cylinder. Obtain a 25mL buret‚ and rinse and fill it with the prepared base solution. Make sure there are no air bubbles trap within the buret. Calculate the amount of KHP required to reach equivalence point. Using a 125mL Erlenmeyer flask‚ place it on a balance‚ and add KHP to it until the balance
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in vinegar. Acetic acid is monoprotic and belongs to the carboxyl family of organic compounds. The titration method is used to neutralize the acids by using the standardized sodium hydroxide solution. It reacts with bases which is sodium hydroxide‚ NaOH to form salt and water. The equivalence point of this neutralization reaction can be determined using a chemical indicator to signal the endpoint. The graph should be plotting to take reading of the equivalence point. Once the equivalence point of
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Abstract: Introduction: Materials: * Chemicals: Buffer solution‚ pH 7.0‚ 50 mL Phenolphthalein indicator solution‚ 1.0 %‚ 1 mL Potassium hydrogen phthalate‚ KHC8H4O4‚ 2 g sodium hydroxide solution‚ NaOH‚ 0.1 M‚ 150 mL Unknown weak acid‚ 1.5g Water‚ distilled or deionized * Equipment: Balance Stir bar Beaker‚ 250mL Oven Buret‚ 50 mL pH sensor Desiccator Rising stand and buret clamp Erlenmeyer flask‚ 125mL Wash bottle with distilled water Funnel Weighing dishes‚ 2
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sit for two weeks shaking periodically. Part B: Prepare a NaOH solution by dissolving 14g of NaOH pellets in 500mL of deionized water. Next standardize the NaOH solution by picking weights of KHP ranging from 2g to 5g and add 50mL of water to the KHP and three drops phenolphthalein indicator. Titrate the solution to a pale pink endpoint. Three titrations should be done with varying KHP weights so as to get an accurate molarity for the NaOH solution. Part C: After two weeks have passed titrate the
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Standardization of NaOH and Determination of Unknown Acid KEYWORDS: quantitative analysis‚ titration‚ buret‚ endpoint‚ standardization‚ half-equivalence point‚ calorimetric titration‚ potentiometric titration ABSTRACT: The concentration of sodium hydroxide was determined by colorimetric titration‚ and the identity of an unknown acid was determined by potentiometric titration. In the first titration‚ a strong acid standard‚ potassium hydrogen phthalate (KHP)‚ was used‚ to determine the concentration
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titration. After standardization of our titrant‚ which in this case will be NaOH‚ we will use this along with the indicator Phenolphthalein‚ to titrate the vinegar to determine the concentration of Acetic Acid in the sample. Equipment and reagents- We will use a 50mL beaker‚ a graduated buret‚ spatula‚ droplet applicator‚ 125mL Erlenmeyer flask‚ hot plate‚ and a container of snow. The reagents we will use are KHP‚ NaOH‚ distilled water‚ Vinegar sample and Phenolphthalein. Procedure- (Refer
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Introduction: Experimental: 2.04 g of KHP‚ 100ml volumetric flask‚ distilled H2O‚ approximately 0.1 M of NaOH‚ Vinegar‚ Phenolphthalein‚ 250ml Erlenmeyer flask‚ weighing balance‚ Graduating Cylinder‚ burette and pH meter were used in our experiment. In our first part of our experiment to prepare a primary standard‚ 0.1 M solution of KHP‚ we carefully weighed out 2.04g of KHP in a weigh paper using the weighing balance and transferred the measured KHP into a 100ml volumetric flask. We rinsed
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phthalate (KHP) used to standardize the solution of NaOH in this experiment. Calculate the Molar Mass of KHP. Molar Mass= 204.22 g/mol Formula: KC8H5O4 2. Using your textbook or chemical dictionary‚ write the definition of indicator. Indicator- a substance added at the beginning of the titration that changes color at (or very near) the equivalence point. 3. Suppose a sodium hydroxide solution were to be standardized against pure solid primary standard grade KHP. If 0.4538
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about the standardization of bases (NaOH) and acids (HCl) which is basically making a dilution to change the molarity. The first reaction consists of titrating sodium hydroxide (NaOH) into potassium acid phthalate (KHP or K[HC8H4O4]): K+[HC8H4O4]- + Na+OH- => K+Na+[HC8H4O4]- + H2O The second titration we did was hydrochloric acid (HCl) with sodium hydroxide (NaOH): HCl(aq) + NaOH(aq) => NaCl(aq) + H2O(l) Procedure: You need to calculate the volume of 3 M NaOH needed to make 500 mL of a 0.1 M solution
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Acid-Base Titrations February 21‚ 2013 Abstract: With the given volume measurement of KHP and NaOH‚ the students experimented to calculate the mass of unknown acid and its equivalence point using a method called titration and titration curve. The known volume of an acid solution would be titrated by slowly adding drops of solution into NaOH‚ and the volume of base needed to react with the acid is measured throughout. By using those data‚ the students are able to find what they
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