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Chapter 8: Problem 8

Identify the acid (proton donor) and the base (proton acceptor) for the reactants in each of the following: a. \(\mathrm{CO}_{3}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{HCO}_{3}^{-}(a q)+\mathrm{OH}^{-}(a q)\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{HSO}_{4}^{-}(a q)\)

Short Answer

Expert verified
a) Acid: \(\mathrm{H}_{2} \mathrm{O}\), Base: \(\mathrm{CO}_{3}^{2-}\) \ b) Acid: \(\mathrm{H}_{2} \mathrm{SO}_{4}\), Base: \(\mathrm{H}_{2}\mathrm{O}\)

Step by step solution

01

- Identify the Acid and Base for Reaction (a)

Analyze the reactants in the equation: \ \(\mathrm{CO}_{3}^{2-}(aq)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{HCO}_{3}^{-}(aq)+\mathrm{OH}^{-}(aq)\)\ - Carbonate ion (\(\mathrm{CO}_{3}^{2-}\)) accepts a proton from water, hence it acts as a base. \ - Water (\(\mathrm{H}_{2}\mathrm{O}\)) donates a proton, hence it acts as an acid.
02

- Identify the Acid and Base for Reaction (b)

Analyze the reactants in the equation: \ \(\mathrm{H}_{2} \mathrm{SO}_{4}(aq)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(aq)+\mathrm{HSO}_{4}^{-}(aq)\)\ - Sulfuric acid (\(\mathrm{H}_{2} \mathrm{SO}_{4}\)) donates a proton, hence it acts as an acid. \ - Water (\(\mathrm{H}_{2} \mathrm{O}\)) accepts a proton, hence it acts as a base.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

proton donor
In an acid-base reaction, the proton donor is the substance that gives away a proton (H+) to another substance. This is usually the definition of an acid in the Br酶nsted-Lowry theory. For example, in reaction (b), sulfuric acid (H2SO4) is the proton donor because it donates a proton to water. Similarly, in reaction (a), water (H2O) donates a proton to the carbonate ion (CO32-) and acts as the proton donor.
proton acceptor
The proton acceptor in an acid-base reaction is the substance that receives the proton (H+) from the proton donor. This is typically referred to as the base. For example, in reaction (a), the carbonate ion (CO32-) acts as the base because it accepts a proton from water. In reaction (b), water (H2O) acts as the proton acceptor when it receives a proton from sulfuric acid (H2SO4).
carbonate ion
The carbonate ion (CO32-) is a polyatomic ion and a common base in acid-base reactions. It is often found in various chemical and biological processes. In reaction (a), the carbonate ion accepts a proton from water and forms bicarbonate (HCO3-). This demonstrates that the carbonate ion acts as a base by accepting a proton and increasing the concentration of hydroxide ions (OH-) in solution.
sulfuric acid
Sulfuric acid (H2SO4) is a strong acid commonly used in various industrial and chemical processes. In reaction (b), sulfuric acid donates a proton to water, producing hydronium (H3O+) and bisulfate (HSO4-). Sulfuric acid is known for its ability to donate protons readily, making it a strong acid. Because it participates in many chemical reactions, understanding sulfuric acid's role as a proton donor is crucial in chemistry.
water as acid
Water (H2O) can act as an acid in certain reactions by donating a proton. An example is reaction (a), where water donates a proton to the carbonate ion (CO32-), resulting in the formation of bicarbonate (HCO3-) and hydroxide ions (OH-). In this context, water behaves as an acid, highlighting its amphoteric nature, which means it can act both as an acid and a base depending on the reaction.
water as base
Water is also capable of acting as a base by accepting a proton. In reaction (b), water accepts a proton from sulfuric acid (H2SO4), forming hydronium (H3O+). This shows water's role as a proton acceptor in this context, behaving as a base. Water's ability to act both as a proton donor and acceptor makes it crucial in many chemical reactions, especially those involving acids and bases.

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Most popular questions from this chapter

State whether each of the following solutions is acidic, basic, or neutral: a. soda, \(\mathrm{pH} 3.22\) b. shampoo, \(\mathrm{pH} 5.7\) c. laundry detergent, \(\mathrm{pH} 9.4\) d. rain, \(\mathrm{pH} 5.83\) e. honey, \(\mathrm{pH} 3.9\) f. cheese, \(\mathrm{pH} 5.2\)

Write the formula for each of the following acids and bases: a. magnesium hydroxide b. hydrofluoric acid c. phosphoric acid d. lithium hydroxide e. ammonium hydroxide f. sulfuric acid

In the blood plasma, \(\mathrm{pH}\) is maintained by the carbonic acid- bicarbonate buffer system. a. How is pH maintained when acid is added to the buffer system? b. How is pH maintained when base is added to the buffer system?

What are some similarities and differences between strong and weak acids?

Write a balanced equation for the neutralization of each of the following: a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)\) and \(\mathrm{NaOH}(a q)\) b. \(\mathrm{HI}(a q)\) and \(\mathrm{LiOH}(a q)\) c. \(\mathrm{HNO}_{3}(a q)\) and \(\mathrm{Ca}(\mathrm{OH})_{2}(s)\)
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