started off by preparing 250mL of NaOH solution. About 0.5 grams of NaOH were measured and then inserted into a 250mL volumetric flask. Once the NaOH was in the flask‚ it was then filled up to the 250mL line using deionized water. After the water was put in the flask‚ the solution was then mixed well until the NaOH dissolved well in the water. The second solution that was prepared was KHP. This was done by measuring 1 gram of KHP. After that was completed‚ the KHP was put in a beaker and filled up
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a report prepared by N. Skrynnikov‚ 2009) Abstract The concentration of an unknown acid (HA) solution was determined by titration with a standardized solution of sodium hydroxide. The standardization of NaOH was done by titration with a solid acid sample‚ potassium hydrogen phthalate (KHP)‚ and phenolphthalein indicator. The unknown concentration (Cunknown) was determined to be X.XX ± X.XX M at a 95% confidence interval‚ and the methods described herein constitute a simple and reproducible technique
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solution‚ NaOH * To standardise the base against potassium hydrogen phthalate * To analyse the unknown acetic acid RESULTS : A. Preparation of the sodium hydroxide solution Volume of NaOH taken from the stock solution = 3.33 mL B. Standardisation of the base against potassium hydrogen phthalate | 1 | 2 | 3 | Weight KHP | 1.0000 | 1.0004 | 1.0006 | Final volume of NaOH (mL) | 22.6 | 22.2 | 21.7 | Initial volume of NaOH (mL) | 0 | 0 | 0 | Volume of NaOH (mL) used
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the base NaOH with potassium hydrogen phthalate‚ or KHP. First‚ about 400 mL of NaOH (10 M) were poured into the 600-mL beaker. This was used to fill the burette. The 50-mL burette was rinsed through twice with 5 mL of NaOH. Then‚ the burette was mounted on the ring stand using a burette clamp and filled to 0 mL. Some of the NaOH was drained to fill the tip of the burette. The initial volume of NaOH‚ rounded to two decimal places‚ was recorded on a piece of paper. Next‚ 0.750 g of KHP (unknown molarity)
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acid is an organic compound with acidic properties. A base reacts with acids to form salts. Titrations are used to determine the concentration of unknown substances. The purpose of the KHP experiment was to determine the molarity of NaOH. HCl titrations are mainly to check technique and used to verify the molarity of NaOH solution. The hypothesis is that this acid is C4H3OCOOH. Experimental Procedure for melting point: The identification of the melting point of the organic acid was done to find another
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some parts during the experiments that the group could not distinguish when the color change occurred so there was more solute going into the mix than there should have been. Also at one point there was the mistake in part B of using KHP and HCl together instead of the NaOH so that mistake skewed results just a little. Conclusion: For this experiment‚ it was essential to make sure the correct solutes were being used properly‚ as we found out‚ it would not produce a color change if the wrong things
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CHEMICAL REACTIONS: ACID-BASE BUFFERS Short Overview Acids and bases represent two of the most common classes of compounds. Many studies have been done on these compounds‚ and their reactions are very important. Perhaps the most important reaction is the one in which an acid and base are combined‚ resulting in the formation of water (in aqueous solution) and a salt; this reaction is called neutralization. A buffer solution is a solution that contains both an acid and a salt
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adding NaOH. We had to do a standardization test because the NaOH has a high reactivity and that could cause a small change. The NaOH solution was supposed to have a molar concentration of .5 however when we standardized the solution we found the actual molarity of the solution to be .4761. This may be due to the fact that NaOH is almost impossible to have pure because it reacts with CO2 in the air. Strong bases are generally very reactive and it makes it hard to have a pure solution of NaOH
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dissolved in solution. It may also be used to calculate the molar mass of an unknown acid or base. Purpose: I. Prepare a standard solution of sodium hydroxide II. Standardize a sodium hydroxide solution by using potassium hydrogen phthalate (KHP) III. When given whether the acid is monoprotic‚ diprotic‚ or triprotic ‚ determine the molar mass of the unknown organic acid. IV. Calculate the Molarity of the Soft drink. Materials: * 50 mL Buret * Beaker * Erlenmeyer
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Introduction The goal of this lab was to correctly prepare a 0.2M solution of NaOH‚ identify highly acidic household cleaning chemicals‚ and determine their concentration (molarity) through titrations using the previously prepared 0.2M NaOH solution. Experimental First‚ to create 0.5L of 0.2M solution of NaOH‚ standard 3M NaOH solution was obtained. Next‚ calculations were performed to determine the amount 3M NaOH necessary to create 0.5L of the 0.2M solution and‚ as a result‚ 33.333ml of the
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