Baking soda (sodium bicarbonate, ) is an example of a base.

a. Draw the Lewis structure of the bicarbonate ion.

b. It is possible for this ion to act as an acid or a base? Explain why.

c. When placed in pure water, bicarbonate ion always acts as a base. Use the relationships in the table above to speculate why this is the case.

d. Propose (and write) a reaction in which bicarbonate ion would act as an acid.

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Allen CorderoLv6

22 Jan 2021

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Baking soda (sodium bicarbonate, NaHCO3) is an example of abase.
1. Draw the Lewis structure of the bicarbonate ion. It is possiblefor this ion to act as either an acid or a base. Explain why.
2. When placed in pure water, bicarbonate always acts as a base.Why is this?
3. Propose (and write) a reaction in which bicarbonate would act asan acid.

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) + HCO3â(aq) â Na+(aq) + CH3COOâ(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 agentâthat 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.

1.Which of the following statements are true about sulfuricacid's role in the esterification reaction. Note thatthere may be more than one correct answer.

		sulfuric acid is added to lower the boiling pointof the reaction mixture.
		sulfuric acid protonates the carboxylic acid inthe first step of the reaction mechanism
		sulfuric acid is used to ensure the alcohol willdissolve in ether
		sulfuric acid protonates the ester in the firststep of the reaction mechanism
		sulfuric acid protonates the alcohol in the firststep of the reaction mechanism
		sulfuric acid reduces the concentration ofOH^- and slows the reverse reaction.
		sulfuric acid is used to ensure the carboxylicacid will dissolve in ether
		sulfuric acid is added to react with excess sodiumbicarbonate in the first step of the reaction
		sulfuric acid acts as a catalyst for thereaction

2.Which of the following below explain why thealcohol is used in excess in this reaction. Note thatthere may be more than one answer.

		This is a reversible reaction and adding excessalcohol drives the reaction towards the products.
		This is a reversible reaction and adding excessalcohol drives the reaction towards the reactants.
		There is no need to add excess alcohol, excessester should be added.
		The alcohol is used in excess to make the reactionmixture soluble in ether during the extraction phase.
		The alcohol is used in excess to remove all of theprotons from the carboxylic acid.
		Excess alcohol completely neutralizes the sulfuricacid and makes the reaction safer.
		The alcohol is less expensive and easier to removefrom the product mixture than the carboxylic acid, but an excess ofeither would help in this reaction.

3.Why is a sodium bicarbonate solution used to extract the ether(organic) layer. Note that there may be more than onecorrect answer.

		sodium bicarbonate reacts with the ester to makeit soluble in water.
		sodium bicarbonate should not be added, sulfuricacid should be added during the extraction.
		sodium bicarbonate reacts with any leftoversulfuric acid to form a salt that is INsoluble in the organiclayer.
		sodium bicarbonate reacts with the alcohol to makeit soluble in water.
		sodium bicarbonate is added because it is lessexpensive than adding hydrochloric acid.
		sodium bicarbonate reacts with any leftovercarboxylic acid to form a salt that is INsoluble in the organiclayer.
		sodium bicarbonate reacts with any leftovercarboxylic acid to form a salt that is soluble in the organiclayer.
		sodium bicarbonate is used to react with ether andmake the yield of the ester product greater.
		sodium bicarbonate reacts with any leftoversulfuric acid to form a salt that is soluble in the organiclayer.