Zinc oxide

If you see a deep blue color add more zinc powder until there is no change in color of the solution in the test tube. XI. Inside the fume hood, add a good amount of Hydrochloric Acid, HCl(aq), to the solution in the 250 ml beaker to remove excess zinc. (accelerate reaction by heating if the reaction appears slow) XII. Take the 250 ml beaker to your lab bench. Set up a gravity filtration with

doing this lab we will practice using a spectrophotometer and review the names of equipment such as volumetric glassware, pipets, and volumetric flasks. Background: Pennies before 1983 were made with pure copper, while pennies minted after 1983 have a zinc core and a copper shell. The difference between the two types of pennies is the reason why we have to use a penny minted after 1983 for this experiment. Also, a Spec 20 spectroscopic measures the intensity of a light beam after the light beam goes

Blood lead and zinc levels were examined among workers having occupational exposure to these metals. The effect of the lead exposure was evident due to number of manifestation reported in this study and the elevation in the levels of lead among workers due to exposure at workplace environment. The group of workers (W4 and W5) exceed the biological exposure index (BEI) of American Conference of Governmental Industrial Hygienist (ACGIH) which is set as 30µg/dL (ACGIH, 2011). Clearly these two groups

In this lab, we balanced the equation xZn(s) + yHCl(aq) → ZnxCly (s) + y/2H2(g) by the information obtained from the lab. When zinc and hydrochloric acid are mixed together, the reaction took place in an evaporating dish that was accompanied by hydrogen gas. Then we measured out the mass of zinc and chlorine in the reaction and calculated the empirical formula of zinc chloride which was ZnCl8. Based on the conservation of mass, we balanced the equation and got Zn(s) + 8 HCl (aq) → ZnCl8 (s) + 4 H2

Zinc Zinc, number 30 on the periodic table and a bluish-white metallic element, exists naturally in air, water and soil. It is present everywhere in the environment. All life on earth has evolved in the presence of zinc. Natural processes such as erosion, forest fires, aerosol formation above the seas and volcanic eruptions continuously transport Zinc. Zinc melts at about 420° C and boils at about 907° C. Zinc is efficient for plants. Zinc-deficient soils present in many parts of the world

All chemicals were of analytical grade. Electrolytic zinc powders were produced by electrolysis of alkaline solutions containing zinc oxide. These solutions were prepared by dissolving a given amount of ZnO in 6 mol L-1 NaOH. After complete dissolution, solutions were stored in 500 ml volumetric flasks. Removing of water from the prepared zinc powder was performed using analytical grade ethanol and acetone mixture. 2.2 Electrolytic cell The electrochemical cell consists of a 0.5 L Pyrex beaker

Observations Nitric Acid Station: Cu(s) + 4HNO3(aq) Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) Before Copper is a reddish brown powdery and lustrous substance. HNO3(aq) is colorless and transparent liquid. During Adding HNO3(aq) made the solid copper change color and state of matter. The solid brown copper turned into a green liquid. Bubbles formed at the surface of the solution and a yellow-brown gas was released. The beaker became warmer and the temperature of the solution increased. After The substance

of the electrical energy in batteries. During my reading, I found out that the first battery was actually invented by Italian physicist Count Alessandro Volta and was demonstrated to Napoleon Bonaparte in 1801. Constructed from alternating discs of zinc and copper wit pieces of cardboard soaked in brine between the metals, this was the first battery that produced a reliable steady current of electricity. The reason why this works is because, as I found out, batteries use the process of redox reactions

to safeguard. The sacrificial anode will get depleted in place of the metal it is protecting. This is why it is referred to as “sacrificial” anode. The materials used for making a sacrificial anode are either comparatively pure active metals such as Zinc and Magnesium, or alloys of Magnesium or Aluminium precisely developed to be used as a sacrificial anode. They are used to protect water-heaters, pipelines, underground tanks, hulls of ships, etc.

grade and were used without further purification. Zinc acetate monohydrate [Zn(CH3COO)2 .H2O] Merck > 98%, and sodium hydroxide (99.5%, NaOH) pellets were purchased from R &M chemicals (UK). Indium nitrate trihydrate, distilled water was ethanol used throughout the experiments, PEG 20000, Triton X-100. For device fabrication materials were procured from Solaronix. In a typical synthesis process, the reaction solution was prepared by mixing 6g of Zinc acetate dihydrate in 70:30 ratio of ethanol/water