For example, if you mix aqueous solutions of AgNO3 and NaCl, there are two new combinations of ions possible. The silver nitrate solution contains Ag+(aq) and NO3-(aq). The sodium chloride contains Na+(aq) and Cl-(aq). Possible new combinations of these ions are AgCl and NaNO3. Note: these formulas would have been written in the upper right hand corner of each box before beginning the lab.
Isotopes Lab By: Darlene Cortez (1st Pd) Background: Atoms of the same element that have different masses are known as isotopes. The difference in mass between isotopes is the result of these atoms having different numbers of neutrons. Key vocabulary: Relative abundance- Relative abundance is a component of biodiversity and refers to how common or rare a species is relative to other species in a defined location or community. Weighted average - An average that takes into account the proportional relevance of each component, rather than treating each component equally. Average Atomic Mass- The mass calculated by summing the masses of an elements isotopes, each multiplied by its natural abundance on earth Mass Number- The total
Bonding Formal Lab Introduction (with Background information): Any substance, whether it is a metal or nonmetal, people can determine it by seeing if it is shiny, soft, or reactive. Metals are shiny, reactive, and have high melting points, while nonmetals are soft, have low melting points and not very reactive, and that is how anyone can determine whether a substance is a metal or a nonmetal. Covalent bonding is when two atoms share electrons, but it only occurs in two nonmetals only. They have low melting points and they are not soluble. Although, Ionic bonding is when an atom gives away elections to another atom, which only happens in a metal and a nonmetal, and they have high melting points and are soluble.
In each part of the experiment, you will be observing a different property of electrolytes. Keep in mind that you will be encountering three types of compounds and aqueous solutions: Ionic Compounds These are usually strong electrolytes and can be expected to 100% dissociate in aqueous solution. Example: NaNO 3 (s) → Na+(aq) + NO 3 –(aq) Molecular Compounds These are usually non-electrolytes. They do not dissociate to form ions. Resulting solutions do not conduct electricity.
What are the identities of the substances found after electrolysis and heating? The identities of the substances found were Iodine, Iodide ion (I-), Triodide ion(I3-), Zinc metal and Zinc ion(Zn2+) Post Lab questions: 1. What did this experiment convincingly show about the composition of the white solid? I put that the experiment showed us the white substance was comprised of Zinc ions and iodide ions, and that the two ions and be separated back into their respective elements 2. During the electrolysis, a gray solid formed on the negative wire of the battery and the dark red solution formed at the positive wire of the batter.
ABSTRACT: The lab of “observations of chemical changes” was to observe the changes that occur in chemical reactions and attempt to interpret these changes. In these experiments it taught me how to interpret chemical reactions with acids and bases. Also, how one chemical can have many different reactions when combined with other chemicals and how to interpret each reaction as what it could mean. I discovered not only how to measure out a well-balanced chemical combination to receive a reaction but to know how to test for acids and bases using a few different methods. Other tests also included in this experiment were testing for Sodium Bicarbonate, and Starch.
Hareem Qureshi Group 6 Presentation Lab 6: Grand Central Equation Focus Questions: * Zinc Iodide can be gained through more than one method. We experienced making Zinc Iodide through zinc granules and iodine chips first and then we used Barium Iodide and Zinc Sulfate to make the zinc iodide. Chemists should prepare Zinc Iodide from its Elements rather than using double replacement reaction between Barium Iodide and Zinc Sulfate. In comparison to the grand central equation lab, the castle of quantification lab proves several benefits of using just Zinc and Iodine in formation of Zinc Iodide. Zn + I2 ⟶ ZnI2 | BaI2·2H2O +ZnSO4·7H2O⟶ZnI2+BaSO4+9H2O | Zinc used: (2g x $0.0625)=$0.125Iodine used:(3g x $0.1003)=$0.301Material cost for 3.1g of ZnI2 =$0.498Material cost for 10g of ZnI2 = $1.6 | 0.48g of Zinc Sulfate heptahydrate used= $0.01940.62g of Barium Iodide dehydrate used= $0.549Material cost for 0.48g of Zinc Iodide= $0.5684Material cost for 10g of ZnI2 = $11.84 | % Yield from Zn and I2 reaction: 98.6%% Error: 1.39% | % Yield from BaI2·2H2O and ZnSO4·7H2O reaction:103.6%% Error: 3.6% | The data above shows that Zinc Iodide formation through elements is much more efficient than using compounds.
Calculations involving the Mole, Avogadro’s Number, Molar Mass, Mole-Mole and Mass-Mole calculations in chemical equations. Combustion analysis and calculation of empirical and molecular formulas from composition analysis. Electrolytes and non-electrolytes. Precipitation reactions and solubility rules. Writing balanced molecular equations and net ionic equations.
CHEMISTRY Name _____________________________ Lab - Molar Volume of a gas lAB 12 OBJECTIVE OF THE LAB: The purpose of this lab is to determine the molar volume of a sample of Hydrogen gas that is created through the reaction of Magnesium and Hydrochloric Acid. The concept of molar volume is that 1 mole of a gas occupies 22.4 liters at STP. Unfortunately the conditions of the lab are not at STP. You will have to use gas law formulas to calculate the volume that one mole of this gas would occupy at STP. In addition, since this lab is being done over water, and water will evaporate at any temperature, the vapor pressure of water must be determined.
,, II I Quantitative Measurements of the Solute Since the solute is the species involved in chemical transformations, our goal will be the determination ot"the number of moles of solute in a particular solution. To be definitive, you want to carry out a reaction that involves zinc iodide. Instead of getting the zinc iodide in the solid state, you go in the .lab and there is a flask that contains zinc iodide diss91ved in water (in the solution state). What might the label on the flask say that will tell you how much iodide there is in the water? · There are numerous measures of the amount of solute in solvent.