Which laboratory values are of concern to you? Why? y. Sodium: may be an indication that the patient is not getting adequate absorption required. SBO’s may cause severe fluctuations in F&E balances.
An error that could have occurred is that the students did not leave the crucible on the hot plate long enough for the color to change. Another error could have been that the temperature was not hot enough. In order to correct these errors, the students would need enough time to do the experiment thoroughly and would also need to check the temperature on the hot plate. References: Deng, Yuanjian, and Sapp, John B. General Chemistry Laboratory Fifth Edition.
Rajeev Pathapati Limiting Reactant Lab Chemistry 6th Due: 2/9/12 Introduction: When a chemical reaction occurs, there is usually a limiting reactant. In a chemical reaction, the limiting reactant, also known as the limiting reagent, is the reactant that is totally consumed at the end of a chemical reaction, and is the reactant that limits the amount of product formed. This also results in excess of the other reactant(s). The reaction tested in this experiment was between a Copper (II) Chloride aqueous solution, and Aluminum metal. The purpose of the lab was to determine which reactant was the limiting reactant, and to see how much of the other reactant was used.
Calculate the percent by mass of NaClO in the commercial bleach. (Start with molarity of concentrated NaClO found in part 4. Determine the molarity per mL instead of liter. Next, divide by the density (you’ll have a label of mole/g at this point). Then multiply this by the molar mass of NaClO which has a label of g/mol so all labels cancel.
What might be the problem with this microscope? It can be cause either due to dirty eyepiece or objective lance or poor resolution. Other reason can be if oil immersion wasn't performed. 3. Why is it important to center a specimen on low power before attempting on focus on it at high power?
Or two, the oppositely charged ions will be attracted to each other with such force that, it will form an ionic compound that is insoluble in water. The insoluble product is the precipitate. These reactions are known as double replacement reaction. Safety The use of protective goggles were required during this experiment due to the harmful chemical being mixed together as well as the harmful reactions occurring as ionic compounds were being mixed. Also we must be wary of wafting these compounds correctly, to directly sniff any of these reactions could turn out very dangerously.
The following data were obtained when a sample of barium chloride hydrate was analyzed as described in the Procedure section. Calculate (a) the mass of the hydrate, (b) the mass of water lost during heating, and (c) the percent water in the hydrate. Mass of empty test tube 18.42 g Mass of test tube and hydrate (before heating) 20.75 g Mass of test tube and anhydrous salt (after heating) 20.41 g. Mass of the Hydrate is 2.33g. Loss (H2O) is 0.34g. Percent H2O in Hydrate is equal 0.34/2.33=14.6% 3.
4. Measurement uncertainties are given in this experiment. Are they reasonable? Explain. The measurement uncertainties given in this experiment are not reasonable considering the quality of equipments used throughout the experiment.
Introduction: In Stoichiometry, you can figure out how much product is produced from a chemical reaction by using the starting amount of a substance, while using math. Stoichiometry is the study of the relationships or ratios between two or more substances undergoing a physical or chemical change (Helmenstine). Since all reactions are dependent on how much was started with, we use those numbers to get the product number. In a limiting reactant problem, an amount is given for both the reactants. The smaller amount will ‘limit” how much the reactant can produce.
Grind an aspirin tablet into a fine powder by using a mortar and pestle. Weigh accurately an aspirin powder. Determine the mass and record it on a data table. 2. Put aspirin powder in a beaker and pipette exactly 30 cm3 of a 1 M NaOH solution onto the powder.