Sodium hydroxide Essays

USES OF SODIUM HYDROXIDE, BLEACHING POWDER, BAKING POWDER, WASHING SODA Objective: To understand the use of common salt (NaCl) for preparation of chemicals such as Sodium hydroxide, Bleaching powder, Baking powder, Washing soda. The common salt (Chemical formula-NaCl, Chemical name- Sodium chloride) that we eat in our daily diet is the raw material for preparation of chemical compounds such as Sodium hydroxide, Bleaching powder, Baking powder, Washing soda. NaCl is a neutral salt. Sodium hydroxide

concentration of acid, we can use a known concentration of hydroxide base. This type of reaction is a neutralization reaction, where salt and water are products of the reaction: Acid + Base Salt +

Abstract The purpose of the experiment was to test which antacid medicine was most effective in decreasing the acidity levels in the stomach. Titration experiments involving hydrochloric acid and sodium hydroxide were used to test different antacids to see which one needed the least amount of sodium hydroxide to turn the solution pink. The antacids that were being compared in this experiment were Alcalak, Alka-Seltzer and Medi-First. With the use of M1 x V1 = M2 x V2 the excess volume of hydrochloric

acid was poured into the flask until there was a permanent pink colour. The acid was allowed to be poured for a little longer before the flask was removed and taken to a lab bench with a buret that contained 0.1 M sodium hydroxide, and the amount of acid used was recorded. The sodium hydroxide was added into the flask in small amounts

triprotic acid, with different volumes of sodium hydroxide. Introduction Procedure Phosphoric acid solution with a volume of 1.00 mL and a molarity of 6.00 M was transferred into a 125-mL Erlenmeyer flask using a volumetric pipette. Sodium hydroxide solution with a volume of 6.00 mL and a molarity of 3.00 M was transferred into a 50 mL beaker using a volumetric pipette. While swirling the phosphoric acid solution in the Erlenmeyer flask, the sodium hydroxide solution was added to it a few drops at

calcium chloride with 2 mL sodium phosphate, adding a few drops of water to a test tube containing 0.5 g copper sulfate, heating 0.5 g of copper(II) hydroxide in a test tube, adding a square piece of zinc to a test tube containing 3 mL 3M hydrochloric acid, mixing 2 mL 3M hydrochloric acid with 2 mL sodium carbonate, adding 0.1 g MnO2 to a test tube with 3 mL hydrogen peroxide, combusting a sodium acetate and ethanol solution, mixing 3 g ammonium chloride and 7 g strontium hydroxide octahydrate together

Beginning with the principles, Brønsted-Lowry acid base theory demonstrates that an acid donates a hydrogen ions, while a base accepts hydrogen ions. Strong acids have the an easier ability to donate hydrogen ions compared to weak acids.The goal for Experiment 8 Acid-Base Equilibria: Determination of Acid Ionization Constants is to recognize how different amounts of quantitative values can alter the pH in a solution. This procedure was carried out by mixinging specific acid or base solutions together

benzoic) to ions. Hydroxide ions on the other hand convert Phenols to ions. This makes them soluble in the aqueous layer as ions are soluble in water. However, addition of HCl to the aqueous ionic solutions regenerates non-ionic substances which are only soluble in the organic layer. Materials • 2M diethyl ether • Saturated NaCl solution • Saturated aqueous solution of Sodium bicarbonate

which has to deal with the laws according to which substances unite to form chemical compounds." In this exercise, we combined copper(II) sulfate pentahydrate with two moles of sodium hydroxide which produced copper(II) hydroxide and sodium sulfate (CuSO4 + 5H2O +2NaOH  Cu(OH)2 + Na2SO4). We then dissociated copper(II) hydroxide to produce copper(II) oxide and water (Cu(OH)2  CuO + H2O). The objective of this exercise is to perform a simple chemical reaction where the concept of stoichiometry is put

Purpose: The purpose of this lab is to titrate an unknown solid acid (KH2PO4) with a standardized sodium hydroxide solution. After recording and plotting the data, the acid’s equivalence point will be recorded once the color changes. Using the equivalence point, the halfway point will be calculated, which is used to determine the acid’s equilibrium constant. The acid’s calculated equilibrium constant will be compared with the acid’s established pKa value. Eventually using the NaOH and the acid’s

experiment, citric acid was titrated with sodium hydroxide producing an endpoint between pH range of 8.3-10. (EASYCHEM, 2018) Citric acid has three acidic protons therefore it is a triprotic acid (lumen, 2018). The accurate concentration of the sodium hydroxide must be known to determine the citric acid concentration. The aim of this experiment was to determine the citric acid(weak acid) content of Lemon Juice by titrating it with standard sodium hydroxide solution(strong base). Commercially available

The experiment for this report is 5, 6, and 7. In experiment 5 there are given a Sodium Hydroxide which is 4.126 g when it is weighted and a KHP also with the NaOH there’s two other experiment that are used to find the titration of molarity in the three chemical balances. In exp. 6 and 7 there using the NaOH to find titration in an acid and vinegar by going through three trails to see how much sodium hydroxide is pick in it until it turns light pink, however if it turns dark pink there’s an error

becomes high enough to cause discomfort, brought about by the ingestion of certain types of food, an antacid preparation can be taken to neutralize the excess stomach acid. The active ingredient in every antacid is a base, the most common being metal hydroxides, metal carbonates or a mixture of the two. Table 1 lists the active ingredients in several commercial brands of antacid. Table 1. Brands of antacid tablets and their major ingredients Brand Name Major ingredient Recommended dose Alka-Seltzer NaHCO3

evaporator, obtaining crude trimyristin, which was then purified via recrystallization with 95% ethanol. This yielded 0.230g of purified trimyristin, in the form of a white powder. The trimyristin was then mixed with sodium hydroxide and 95% ethanol under gentle reflux, yielding sodium myristate. Finally, concentrated hydrochloric acid was added dropwise, yielding myristic acid. I obtained a yield of 408.3% (0.523g) of the myristic acid

Then 35 ml of 1.00 M of Sodium hydroxide was measured and set aside. Using the calorimeter, the hydrochloric acid was stirred heartily and its temperature was recorded as the initial temperature. The temperature of the Sodium hydroxide was assumed to be similar because they were both in the same conditions (lab) for the exact amount of time. Next the Sodium Hydroxide solution was added to the hydrochloric acid solution in the cups and stirred until

of a given material known as concentration is in a substance or mixture. In this lab, the student also learns the technique of using titration. The concentration of the acid we used in class will be sampled with a standardize solution such as sodium hydroxide with an environmentally indicator to show the physical change of color that occurs to the solution by the acid. The equipment necessary for the titration experiment follows: 0.1M NaOH, Acid solution, Anthocyanin (which is found in red cabbage

In the chemical reaction of hydrochloric acid, HCl, and sodium hydroxide, NaOH, the theoretical ratio is one HCL for every one NaOH. By then taking a known measurement of HCl, in this case 10mL, in addition to the phenolphthalein indicator and deionized water, and titrating it with NaOH, the amount of NaOH that causes the reaction to be complete was calculable given that we know when the reaction was complete. After calculating the moles of each substance added to complete the reaction, the experimental

2.2 Chemicals and reagents The API of AN (99.9% pure) 1000mg was purchased from market. HPLC grade acetonitrile (SD fine limited). Analytical grade hydrochloric acid ,sodium hydroxide flakes, hydrogen peroxide. Milli-Q Water purchased from market.. 2.3 Details of Method Chromatographic conditions: Reversed Phase High Performance liquid chromatography method with UV detection separation was achieved on zorbox Agilent Eclipsc XDB column c18(150 nm× 4.6 mm×5µm) as stationary phase with binary gradient

after reflux Dense gas can be seen Washing the ester with distilled water The ester layer is immiscible with distilled water. Washing the ester with sodium carbonate solution Effervescence -bubbles of gas produced -a ‘pop’ sound could be heard when the separating funnel is closed and opened again. The ester layer is immiscible with the sodium carbonate solution Adding anhydrous calcium chloride into the ester solution Heat would be produced as the surface of the conical flask feels warm.

Verna Wang Hannah Palmer CHEM 101-069 Lab 11-19-16 Stoichiometry and Limiting Reagents Lab Report Purpose: We are using the reaction of sodium hydroxide and calcium chloride to illustrate stoichiometry by demonstrating proportions needed to cause a reaction to take place. Background: Just like a recipe would call for a specific amount of one ingredient to a specific amount of another, stoichiometry is the same exact method for calculating moles in a chemical reaction. Sometimes, we may not have