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6.) If our actual yield was 13 grams of sodium chloride, what would our percent yield for this reaction be?Formula for percent yield is:Example: I expected to get 30 grams; I ended up getting 25 grams.7.) Is the answer in #6 reasonable? If so, explain why you think this was a reasonable answer.8.) What are some factors that might cause the percent yield to be lower than 100%? Make sure you discuss specificexamples of how this might happen.IntroductionIn this lab, you will need to do a reaction where baking soda will react with an excess of vinegar. By doing this, you will(hopefully!) ensure that you will get 100% actual yield for the reaction.For our reaction, we will need to use 0.05 moles of baking soda, which we will call by its chemical name, sodiumhydrogen carbonate (NaHCO 3 ) for the rest of this lab. If we use much more than 0.05 moles of baking soda, the reactionwill be too large and we will rest having some of the reaction products pour over the side of the flask when we mix itwith the vinegar (which we call acetic acid – CH 3 COOH).In the space below, use dimensional analysis to calculate the amount of sodium hydrogen carbonate we will need forthis lab:FOR THIS LAB, WE WILL USE ______________GRAMS OF SODIUM HYDROGEN CARBONATE52
Using stoichiometry, how many moles and grams of sodium acetate do we expect to get? Show your calculations below.Using stoichiometry, how many moles and liters of CO 2 do we expect to get? Show your calculations below.Materials_____grams of baking soda (how much did you calculate you would need in the introduction?)150 mL of vinegar1 cupA 500 mL flaskStirring rod30 ml of waterHot plateGraduated cylinderMethodsIn this section, you will now carry out the reaction that was discussed at the beginning of this lab.1.) Observe 3 physical properties of vinegar and baking soda. Write down your observations in the Data & Observationsection of this lab.2.) In a cup, measure out the weight of sodium hydrogen carbonate that you calculated you would need in theintroduction section of this lab. Don’t forget to tare (zero) the weight of the cup. Make sure the amount that you use isas close as possible to the amount that you calculated. Write the exact amount of sodium hydrogen carbonate that youused here:Amount of sodium hydrogen carbonate that you actually used: _____________________grams3.) Add 30 mL of water to the cup containing the sodium hydrogen carbonate. Stir the solution until most or all of it isdissolved (if a little won’t dissolve, that’s okay).4.) Weigh a 500 mL flask. You will need the weight of an empty flask at the end of the lab.Weight of empty 500 mL flask: __________________ grams5.) Add the sodium hydrogen carbonate solution to the empty 500 mL flask.6.) In a graduated cylinder, measure out 150 mL of acetic acid (aka vinegar) and slowly add it to the sodium hydrogencarbonate solution. You will observe the formation of bubbles when the acetic acid is added to the sodium hydrogen53
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Page 9 and 10: STEP 3: EVIDENCE FOR CHEMICAL REACT
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Page 21 and 22: HomeworkFor each problem, balance t
Page 23 and 24: STEP 6: DIMENSIONAL ANALYSIS PART 1
Page 25 and 26: EX #4: How many seconds are in a ye
Page 27 and 28: 1.) How many nickels are in 10 dime
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Page 34 and 35: STEP 9: MOLES & GRAMSReview:1.) How
Page 36: HOMEWORKMolar MassDo the following
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Page 41 and 42: Mole-Volume Conversions1. Determine
Page 43 and 44: 5. How many particles are there in
Page 45 and 46: Example #1: Now, try with a real ch
Page 47 and 48: STEP 13: STOICHIOMETRY PART 21.) Ba
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