Informal Lab Report Essay

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Table of Contents/Labs Lab # | Title | Page | | Informal Lab Report Procedures & Grading Rubric | 2-4 | 1 | How Many Drops Of Water Can Fit On A Penny? | 5-6 | 2 | Is The Potassium Chloride Mixture Homogeneous or Heterogeneous? | 7 | 3 | What Are The Densities Of Pre- And Post-1982 Pennies? | 8 | 4 | Which Type Of Glassware Is Most Accurate? | 9 | 5 | What Is The Relative Abundance Of Pre- And Post-1982 Pennies In A Sample of 1982 Pennies? | 10 | 6 | What Are The Identities Of The Unknown Substances? (Flame Test Lab) | 11 | 7 | How Does The Placement Of Elements On The Periodic Table Demonstrate The Periodic Law? | 12-13 | 8 | How Do Ionic Bonds Form? | 14 | 9 | Is The Substance Ionic Or Covalent? | 15 |…show more content…
What determines the ratio of elements in an ionic compound? (i.e. why are NaCl in a 1:1 ratio but CaCl2 has a 2:1 ratio of elements?) 2. Two ionic compounds often react so that the positive and negative ions change places. For example, AgNO3 and NaCl will react to form AgCl and NaNO3. Predict the results of the reaction between barium carbonate and magnesium sulfate. Write the formulas and the names of the reactants and products. 3. Bring in the ingredient labels of 2 different food items that contain ionic compounds. In your lab report, list the food item and all of the ingredients that you believe are ionic in that food. Conclusion: Instead of a formal conclusion, restate the original question and answer it. Lab #09: Is the Substance Ionic or Covalent? Purpose: To identify compounds as ionic or covalent based on their properties. We will do this by testing melting point, conductivity, and solubility. Hypothesis: Draw a chart in which you will predict what your results will look like for the three different tests for an ionic compound and a covalent compound. We will fill this table in…show more content…
Add the HCl SLOWLY to the magnesium by running it down the side of the beaker. Adding the acid too quickly will result in the spattering of the acid. Write down any observations of the reaction. 6. After all the acid has been completely added and the reaction has stopped, use a pipette to add a few extra drops of acid into the beaker until the reaction stops. 7. Place the beaker on a hot plate and heat on a high setting to boil off the water. WARNING: THERE WILL BE A SMALL AMOUNT OF HYDROCHLORIC ACID BOILING OF THE MIXTURE. DO NOT PLACE YOUR FACE DIRECTLY ABOVE THE BEAKER. 8. When ALL of the water is gone, allow the beaker to return completely to room temperature on the table and measure its mass. NOTE: Never place a hot beaker directly on the table. Use the wire gauze as a barrier. 9. Heat the beaker again on the hot plate for a minute, cool to room temperature, and measure its mass. Continue the heating and cooling process until you obtain two consecutive constant masses. 10. Dispose of the magnesium chloride down the sink. Rinse out the beaker and set it to dry for the next

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