Properties of Ammonium Compounds

KIO3 + 6 HCl + 6 Na2S2O3 → 3 Na2S4O6 + KI +3 H2o + 6 NaCl

2. Summarize the following description of a chemical reaction in the form of a balanced chemical equation?

sodium thiosulphate + hydrochloric acid = sodium chloride (salt) + sulphur + water + sulphur dioxide

to the unknown solution in order to completely precipitate the cations in part A. 2 A compound

Ammonium nitrate (NH4NO3), is classified as a salt. The salt family of chemicals contains ions, which are particles with electrical charges. Due to the fact that opposite polarity ions attract each other, they form a solid crystal that is called salt. This when seen by the naked eye seem like a simple reaction. Bu, in reality this occurs in two different steps and each step a change of energy takes place.

When the red Co(NO3)2*6H2O crystal was added to the white NH4 crystal, and water was added to dissolve, the solution turned blue in color. As the solution was nixed, the color changed to that of a blue-purple and a blue precipitate formed. When the 6 M NH3 began to be added, the color shifted to dark purple color after 15 mL of ammonia and the amount of the precipitate was less. After 20 mL of ammonia, the solution became a red brown with very little of the blue precipitate. After 30 mL of ammonia, the solution was similar in color to an iodine solution, a dark brown-red, almost black in color. At this point there was no visible precipitate on the surface of the solution. After 40 mL of the ammonia had been added, the solution was the same iodine like color as before. When closely examined, there was a black precipitate that had settled on the bottom of the beaker. At this point, hydrogen peroxide, 3% H2O2, was added to solution. After 4 mL of the H2O2 was added, the solution was the same color and the precipitate had not changes. After 8 mL of the H2O2, there was not noticeable change. After 12 mL of the H2O2, the solution was slightly redder in color but the precipitate had not changed. After 15 mL of H2O2, the solution was the same color and no changes had occurred to the precipitate. At 17 mL, the solution began to effervesce slightly, though there

Environment/industry specific concern: Minimal risk, this chemical is only used when the facility is not in operation. For example, the fogging equipment is set to run at the end of the day for a short period and allowed to dissipate overnight before production commences the next day. Elevated risk is introduced

This experiment was conducted under conditions described by Williamson, 2003. To begin, approximately 150 mg of cyclohexanone was placed into a vial. In a separate 10 x 100 mL reaction tube, 1.0 mL of HNO3 was added by pipette, along with a pre-weighed boiling chip. The reaction tube containing the nitric acid was clamped into a sand bath under the fume hood and heated at a low setting. One drop of cyclohexanone was careful added to the nitric acid. The presence of a brown oxide indicated that the reaction had begun, at which point the reaction tube was removed from the sand bath.

Write a balanced chemical equation for each reaction #1-8. Classify each reaction using the information provided in the

The purpose of this experiment was to identity, analyze and synthesize an unknown white compound. The identity of the unknown compound was determined by a flame and ion test to identify the cation and anion present in the compound. To confirm the identity, an ammonium test and conductivity test was conducted. After, the unknown compound, which was identified as Calcium(II)Nitrate, was synthesized in an acid-base reaction between Nitric Acid and Calcium Carbonate. The increments used were done so in order to obtain a theoretical yield of 1.0 gram of Ca(NO3)2.

Stoichiometry has many uses in the real world. In the chemical industry and in professional scientific experiments, scientists use stoichiometry to save money. Scientists use stoichiometric calculations to determine the amount of a substance they need to purchase for a specific reaction. There are four possible reactions that can occur when sodium bicarbonate thermally decomposes. In this lab, stoichiometry was used to find out which balanced chemical equation out the four best represents the thermal decomposition of sodium bicarbonate.

Introduction: In this lab report I will demonstrate a brief explanation of the thermochemistry, in details, useful terms for this report, the enthalpy of the various reactions as well as some calculations for further explanation about the subject. The goal of this report is to compute the specific and approximate molar mass of a metal, the enthalpy of a neutralization of two acids and finally the enthalpy of an unknown salt. ΔfH explains the change in the enthalpy when one mole of a specific substance is formed from its elements in the standard states. Standard states can be expressed as a pressure of one atmosphere and a temperature of 25 Celsius.

The HSE says that many substances can be dangerous to health including, toxic gases, large and heavy items, dangerous machines and many more act 1974 introduces ways to reduce injuries against these hazardous items towards health. Curtesy of www.Hse.gov.uk b) According to the HSE what are the main ways in which individuals may be exposed to harmful substances?

In the fourth reaction, 15 mL of 6.0 M sulfuric acid was added to the copper (II) oxide while stirring. The balanced equation for this reaction is as follows:

There is a type of reaction in which Nitrogen atom doesn’t realese from the salt. This type of reaction is called reduction reaction, it done by using SNCl2 or Na2So3 to give hydrasin derivatives.