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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

Laundry bleach is a solution of sodium hypochlorite (NaClO). To determine the hypochlorite (ClO \(^{-}\) ) content of bleach (which is responsible for its bleaching action), sulfide ion is added in basic solution. The balanced equation for the reaction is $$ \mathrm{ClO}^{-}(a q)+\mathrm{S}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{Cl}^{-}(a q)+\mathrm{S}(s)+2 \mathrm{OH}^{-}(a q) $$ The chloride ion resulting from the reduction of HClO is precipitated as \(\mathrm{AgCl}\). When \(50.0 \mathrm{~mL}\) of laundry bleach \(\left(d=1.02 \mathrm{~g} / \mathrm{cm}^{3}\right)\) is treated as described above, \(4.95 \mathrm{~g}\) of \(\mathrm{AgCl}\) is obtained. What is the mass percent of \(\mathrm{NaClO}\) in the bleach?

Consider the reaction between silver and nitric acid for which the unbalanced equation is $$ \mathrm{Ag}(s)+\mathrm{H}^{+}(a q)+\mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{Ag}^{+}(a q)+\mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O} $$ (a) Balance the equation. (b) If \(42.50 \mathrm{~mL}\) of \(12.0 \mathrm{M}\) nitric acid furnishes enough \(\mathrm{H}^{+}\) to react with silver, how many grams of silver react?

Write net ionic equations for the formation of (a) a precipitate when solutions of magnesium nitrate and potassium hydroxide are mixed. (b) two different precipitates when solutions of silver(I) sulfate and barium chloride are mixed.

Mssign oxidation numbers to each element in (a) \(\mathrm{HIO}_{3}\) (b) \(\mathrm{NaMnO}_{4}\) (c) \(\mathrm{SnO}_{2}\) (d) NOF (e) \(\mathrm{NaO}_{2}\)

Assign oxidation numbers to each element in (a) nitrogen oxide (b) ammonia (c) potassium peroxide (d) chlorate ion \(\left(\mathrm{ClO}_{3}^{-}\right)\)
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