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The classic volcano reaction is often performed by the simple mix of vinegar (CH3COOH) and sodium bicarbonate (NaHCO3) resulting in a large amount of CO2 foam being produced. How many moles and liters of gas would be produced by reacting 55.7 g of NaHCO3 with excess vinegar? Assume the reaction releases all the gas theoretically possible, and the reaction takes place at 22 C and 1 atm. NaHCO3(s) + CH3COOH(aq)-> CO2(g) + H2O(l) + NaC2H3O2(aq)

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Patrina SchowalterLv2
28 Sep 2019
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Related questions

The classic volcano reaction is often performed by the simple mix of vinegar (CH3COOH) and sodium bicarbonate (NaHCO3) resulting in a large amount of CO2 foam being produced. How many moles and liters of gas would be produced by reacting 55.7 g of NaHCO3 with excess vinegar? Assume the reaction releases all the gas theoretically possible, and the reaction takes place at 22C and 1 atm. NaHCO3(s) + CH3COOH)aq)-> CO2(g) + H2O(l) + NaC2H3O2(aq)

Alka Seltzer is an effervescent tablet that contains aspirin (acetylsalicylic acid), citric acid, and sodium bicarbonate (NaHCO3). As soon as the tablet dissolves in water, the NaHCO3 dissociates to form a bicarbonate ion (HCO3-) and a sodium ion (Na+)

1. NaHCO3(s) --> Na+(aq) + HCO3-(aq)

Acitic acid, which will ‘donate’ H+ to water to create H3O+(aq) is then added to the mixture. With the addition of acetic acid the following acid-base reaction then takes place:

2. HCO3-(aq) + H+(aq) --> H2O(l) + CO2 (g)

1.Based on your plot (from analysis section). Hint – Consider the reaction equation and vinegar is a source of H3O+ ions.

a) At what range of volumes of vinegar is H+ the limiting reactant?

b) At what range of volumes of vinegar is HCO3- the limiting reactant?

2. Based on your data and your plot, what is the percent by mass of NaHCO3 in the average Alka Seltzer tablet? Show any calculations used to determine your answer. Remember to average only the HCO3- limited range.

3. How might this product reduce indigestion or heartburn?

4. Mass can neither be created nor destroyed. If solution decreases in mass where did this “lost” mass go?

5. Would it be possible to do a similar experiment by measuring the volume of CO2 generated? Explain in detail.

Baking soda is pure sodium bicarbonate, NaHCO3, which dissolves and dissociates in water into thesodium ion and the bicarbonate ion. As most students know from demonstrations in grade school or athome, it can be mixed with vinegar for a rapid and entertaining chemical reaction that generates carbondioxide gas bubbling out of the reaction mixture.

The overall reaction can be written as:CH3COOH (aq) + Na+(aq) + HCO3–(aq) → Na+(aq) + CH3COO–(aq) + H2O(l) + CO2(g) in which the sodium ion is a spectator ion.

Baking soda or baking powder can be used in recipes as a leavening agent—that is, to produce carbondioxide gas to make dough or batter rise. Recipes using baking soda must include a separate acidicingredient such as buttermilk or vinegar. Recipes that do not include the separate addition of an acidicingredient usually require baking powder instead. Baking powder has a solid organic acid mixed in withthe baking soda, so that when the mixture is dissolved, the acid and sodium bicarbonate react with eachother. While commercial baking powder involves slightly more complicated chemistry, a good substitutefor baking powder can be made by adding baking soda to an acid such as potassium hydrogen tartrate(potassium bitartrate or cream of tartar). The formula for potassium hydrogen tartrate is KH C4H4O 6 . Your task is to devise a suitable substitute for baking powder by calculating the mass of cream of tartar in grams required to react with 10.00 g of baking soda. There should be enough cream of tartar added so that all of the baking soda will react to make carbon dioxide gas, but no more cream of tartar than that.

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