Hydroxide Essays

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 into

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 (NaOH)

Introduction: Benzaldehyde and acetone in ethanol solvent undergoes cross aldol condensation reaction to give dibenzalacetone. This reaction known as the Claisen-Schmidt reaction. Reaction: The benzalacetone, formed as an intermediate. Benzalacetone once formed, then easily react with another molecule of benzaldehyde to give dibenzalacetone. Procedure: 1. Take 8 mL of benzaldehyde in 100 mL beaker. 2. Add 2 mL of acetone to the benzaldehyde and mix. 3. Dissolve 5 g of NaOH into 50

pthalimide Reaction: (Step 2 is Hoffmann degradation reaction) Procedure: 4. Dissolve 15 g sodium hydroxide in 15 ml water. Keep the solution cool and add 4.2 mL bromine in one lot. 5. Shake the mixture till all the bromine has reacted. Maintain the temperature below 0 º C and finely add 12g powdered phtalimide in one lot. 6. Shake the mixture vigorously and add a cold solution of 11 g sodium hydroxide in 40 mL water. 7. Shake the reaction mixture and the temperature rises to about 70 0C . Warm the

AIM Design an experiment to study a thermodynamic property of a chemical substance, a chemical reaction, a physical change or chemical phenomenon. BACKGROUND INFORMATION Standard enthalpy change of solution, ∆Hsolnø, is the enthalpy change when one mole of a substance dissolves in water to form a solution of infinite dilution under standard conditions.1 The standard enthalpy change can either be exothermic or endothermic. An exothermic reaction is a reaction where energy is released as a form of

Organic chemistry II Experiment 3: chromic acid oxidation reaction Introduction: Camphor is very compact and its molecular structure is symmetrical which gives it the property to change directly from a solid to vapour when heated. Therefore, camphor can easily be purified by sublimation technique. Sublimation is a phase change in which a solid phase passes directly into the vapour without going through an intermediate liquid phase. Solids which have vapour pressure below melting points can be purified

obtained knowledge of the total acidity, the experiment can be performed with the purpose of determining the amount of %w/w of citric acid in Kool-Aid. Using a titrimetric analysis method, the analyte, total solution acidity and titrant, sodium hydroxide, undergo an acid-base titration. Differing from the redox titration undergone in experiment two in which the ascorbic acid is reacted with the reduced iodate in the presence of iodine ion generating iodine, which is the form that is used to further

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

with either sodium hydroxide (NaOH) or aqueous ammonia (NH₃). Can you make any correlation between the quantities of the heat given off and the fact that sodium hydroxide is a stronger base than ammonia (NH₃)? A negative ΔH indicates a process giving off heat, making it exothermic. Using the values collected throughout the experiment, there seems to be a trend between sodium hydroxide and aqueous ammonia, being that more heat is given off when the acids react with sodium hydroxide. From this we can

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

order to determine the molar concentration of the NaOH solution. As seen in Table 1, the known mass of KHC8H4O4 was 0.2037 g. The moles of KHC8H4O4, could then be calculated to get 9.97E-04 mol. Based on the balanced equation between the sodium hydroxide solution and primary standard acid, the mole ratio of 1:1 and the molar mass of NaOH was applied to calculate the molar concentration of NaOH, which was 5.42E-02 mol/L (Table 2). Since there was only one trial conducted for this part, the average

back titration is also known as indirect titration. A known mass of toothpaste is neutralised with a known concentration and volume of hydrochloric acid, HCl. The mixture is then further neutralised by a known concentration and volume of sodium hydroxide solution, NaOH to determine the number of mole of HCl that reacted with CaCO3 in the toothpaste. As the number of mole of CaCO3 is found through the mole ratio thus the mass of CaCO3 is known and the percentage of CaCO3 can be calculated. The percentage

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 a

When the sodium hydroxide pellet was added, the test tube became warm and it took awhile to dissolve. The dissolution of NaOH in water resulted in a basic solution (When tested with the red litmus paper, the paper turned a blue color and when tested with the blue litmus paper, the paper remained a blue color). The net ionic equation for the dissolution of NaOH in water is displayed below: NaOH(s) → Na+(aq) + OH-(aq) The addition of magnesium hydroxide to water resulted in a cloudy slurry. There

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 and swirling the solution, mixing 2 mL sulfuric acid and 4 mL sodium hydroxide 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

Equation: Cu(s) + 4HNO3(aq) —> Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) Reaction 2: when sodium hydroxide (NaOH) is added to copper (II) nitrate (Cu(NO3)2), a double displacement reaction will occur. Copper and sodium will displace each other to create copper (II) hydroxide and sodium nitrate. Balanced Chemical Equation: Cu(NO3)2 (aq) + 2NaOH (aq) —> CuOH2 (s) + 2NaNO3 (aq) Reaction 3: When copper (II) hydroxide is heated, a decomposition reaction will occur. The reaction will decompose forming two compounds

It is produced also by the reaction of ammonium nitrate and sodium hydroxide, sodium bicarbonate or sodium carbonate. NH4NO3 + NaOH → NaNO3 + NH4OH NH4NO3 + NaHCO3 → NaNO3 + NH4HCO3 2NH4NO3 + Na2CO3 → 2NaNO3 + (NH4)2CO3 Sodium Nitrate (Nitratine) is Isostructural with Calcium Carbonate (Calcite). This means they have similar

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