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Chapter 4: Problem 29

For an acid-base reaction, what is the reacting species, that is, the ion or molecule that appears in the chemical equation, in the following acids? (a) perchloric acid (b) hydriodic acid (c) nitrous acid (d) nitric acid (e) lactic acid \(\left(\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{3}\right)\)

Short Answer

Expert verified
Question: Identify the reacting species (ions or molecules) that are involved in an acid-base reaction for the given acids: (a) Perchloric Acid, (b) Hydriodic Acid, (c) Nitrous Acid, (d) Nitric Acid, and (e) Lactic Acid. Answer: (a) HClO4 → H+ + ClO4-, (b) HI → H+ + I-, (c) HNO2 → H+ + NO2-, (d) HNO3 → H+ + NO3-, (e) HC3H5O3 → H+ + C3H5O3-

Step by step solution

01

(a) Perchloric Acid

Perchloric acid has the chemical formula HClO4. In an acid-base reaction, the acid loses a proton (H+), leaving the conjugate base. In this case, after losing a proton, perchloric acid becomes the perchlorate ion (ClO4-). The reacting species in the reaction is: HClO4 → H+ + ClO4-
02

(b) Hydriodic Acid

Hydriodic acid is represented by the chemical formula HI. During an acid-base reaction, the acid will lose a hydrogen ion (H+), resulting in iodide ion (I-) remaining. The reacting species in the reaction is: HI → H+ + I-
03

(c) Nitrous Acid

Nitrous acid has the chemical formula HNO2. In an acid-base reaction, the acid loses a proton (H+), leaving the nitrite ion (NO2-) as the conjugate base. The reacting species in the reaction is: HNO2 → H+ + NO2-
04

(d) Nitric Acid

Nitric acid is represented by the chemical formula HNO3. During an acid-base reaction, the acid will lose a hydrogen ion (H+), resulting in the nitrate ion (NO3-) remaining. The reacting species in the reaction is: HNO3 → H+ + NO3-
05

(e) Lactic Acid

Lactic acid has the chemical formula HC3H5O3. In an acid-base reaction, the acid loses a proton (H+) from its hydroxyl group (OH), leaving the lactate ion (C3H5O3-) as the conjugate base. The reacting species in the reaction is: HC3H5O3 → H+ + C3H5O3-

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Most popular questions from this chapter

Assign oxidation numbers to each element in (a) \(\mathrm{P}_{2} \mathrm{O}_{5}\) (b) \(\mathrm{NH}_{3}\) (c) \(\mathrm{CO}_{3}{ }^{2-}\) (d) \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\) (e) \(\mathrm{N}_{2} \mathrm{H}_{4}\)

What is the volume of \(1.222 \mathrm{M}\) sodium hydroxide required to react with (a) \(32.5 \mathrm{~mL}\) of \(0.569 \mathrm{M}\) sulfurous acid? (One mole of sulfurous acid reacts with two moles of hydroxide ion.) (b) \(5.00 \mathrm{~g}\) of oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) ? (One mole of oxalic acid reacts with two moles of hydroxide ion.) (c) \(15.0 \mathrm{~g}\) of concentrated acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)\) that is \(88 \%\) by mass pure?

A capsule of vitamin \(\mathrm{C}\), a weak acid, is analyzed by titrating it with \(0.425 M\) sodium hydroxide. It is found that \(6.20 \mathrm{~mL}\) of base is required to react with a capsule weighing \(0.628 \mathrm{~g}\). What is the percentage of vitamin \(\mathrm{C}\) \(\left(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{6}\right)\) in the capsule? (One mole of vitamin \(\mathrm{C}\) reacts with one mole of hydroxide ion.)

A student is asked to identify the metal nitrate present in an aqueous solution. The cation in the solution can either be \(\mathrm{Na}^{+}, \mathrm{Ba}^{2+}, \mathrm{Ag}^{+}\), or \(\mathrm{Ni}^{2+}\). Results of solubility experiments are as follows: unknown + chloride ions-no precipitate unknown + carbonate ions-precipitate unknown + sulfate ions-precipitate What is the cation in the solution?

An artificial fruit beverage contains \(12.0 \mathrm{~g}\) of tartaric acid, \(\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{O}_{6}\) to achieve tartness. It is titrated with a basic solution that has a density of \(1.045 \mathrm{~g} / \mathrm{cm}^{3}\) and contains \(5.00\) mass percent \(\mathrm{KOH}\). What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
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