finish. KHP is potassium hydrogen phthalate‚ and is a weak acid. Potassium hydrogen phthalate is a white‚ odorless crystal that is odorless and can cause mild skin irritation if not rinsed from skin in an aqueous form. (Chemistry Lab Manual) Sodium hydroxide‚ NaOH‚ is a very corrosive base‚ and is a white crystal in solid form. It can cause tissue damage if not kept from skin. (www.britannica.com) The chemical equation for KHP is KHC8H4O4. The chemical equation of sodium hydroxide is NaOH. (Chemistry
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weakly basic solutions. Once the solution is titrated to a more basic solution the indicator turns pink. Before titrating an unknown acid we will first standardize the NaOH solution. By this we mean we will accurately determine its concentration through a titration experiment. A known amount of a standard (we will use KHP)
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about how to standardize a Sodium Hydroxide (NaOH) solution by titrating it with pure sample of Potassium acid Phthalate (KHC8H4O4). This experiment has two sections. The first section is to standardize the Sodium Hydroxide by titration. Three sample of 0.7 – 0.9 g of solid KHP are place into each of the three numbered Erlenmeyer flasks. 50 ml of distilled water are added to each three of it from graduated cylinder and constantly shake it until the KHP solution are completely dissolve. 2 drops of
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hydroxide (NaOH) was determined by using a known amount of Potassium Hydrogen phthalate (KHP). The balanced chemical equation for the reaction is: KHC8H4O4(aq) + NaOH(aq) => H2O(l) + KNaC8H4O4(aq) (1) KHP was chosen as a good acid to standardize NaOH because it has high molecular weight and stable on drying. The standardized NaOH solution was then used to determined the percent composition of KHP in an unknown substance #47. Experimental Information Part 1: Standardization of NaOH NaOH solution
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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
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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
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We will also determine the unknown concentration of the strong base NaOH by its reaction with a known amount of the weak acid‚ potassium acid phtalate (HKC8H4O4‚ abbreviated KHP). This will be accomplished using the titration method. The KHP solution will be created and its volume and concentration recorded. The KHP solution will be poured in a flask along with a few drops of one of three indicators we will be evaluating. The NaOH solution will be poured into a buret (with volume markers) and will
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Experiment 2 Preparation of Primary Standard solutions and Standardizing Acid and Base solutions Objectives: The objective of this experiment is: 1- To prepare two primary standard solutions‚ KHP and Na2CO3 2- To standardize a sodium hydroxide solution using the prepared primary standard KHP. 3- To standardize a hydrochloric acid solution using the prepared primary standard Na2CO3. 4- To calculate the concentration of an unknown acid or base. Introduction A primary standard is a standard that
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unknown solution used‚ the unknown concentration can be calculated. For example‚ standard base solution (NaOH) is added from a burette to an accurately known volume of the acid solution (HCl). HCl(aq) + NaOH(aq) ------------> H 2 O(l) + NaCl(aq) This reaction (neutralization) can be written as a NET IONIC equation as follows: H+(aq) + OH-(aq) ----------> H 2 O(l) (2) (1) When sufficient NaOH has been added to react with all of the acid‚ the titration is complete -- the equivalence point has been
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concentration of the vinegar. Procedure: Part A – Standardization of a Sodium Hydroxide Solution 1. Prepare 150 mL of approximately 0.5M sodium hydroxide solution from solid NaOH. The solution can be prepared in a beaker‚ it is not necessary to use a graduated cylinder or a volumetric flask because the NaOH solution will be standardized. 2. Weigh a 150-mL beaker and record the mass to the nearest 0.001 g. Add approximately 0.5 grams of potassium hydrogen phthalate
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