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Chapter 4: Problem 19

Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueous solution of this compound? Write the chemical equation for the ionization of HCOOH.

Short Answer

Expert verified
The solutes present in an aqueous solution of formic acid (HCOOH) are H+ and HCOO- ions. The chemical equation for the ionization of HCOOH is: HCOOH \(\rightleftharpoons\) H+ + HCOO-

Step by step solution

01

Identify the ions present in formic acid

Formic acid (HCOOH) is a weak acid, and when it ionizes in water, it will lose one hydrogen ion (H+) and form a formate ion (HCOO-). So the solutes present in an aqueous solution of formic acid are H+ and HCOO- ions.
02

Write the chemical equation for the ionization of formic acid

Now that we have identified the ions present in formic acid, we can write the equation for its ionization. Since it's a weak electrolyte, we will use a double arrow to indicate the partial ionization. The chemical equation for the ionization of formic acid (HCOOH) in water is: HCOOH \(\rightleftharpoons\) H+ + HCOO-

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Most popular questions from this chapter

Uranium hexafluoride, \(\mathrm{UF}_{6}\), is processed to produce fuel for nuclear reactors and nuclear weapons. \(\mathrm{UF}_{6}\) is made from the reaction of elemental uranium with \(\mathrm{ClF}_{3}\), which also produces \(\mathrm{Cl}_{2}\) as a by-product. (a) Write the balanced molecular equation for the conversion of \(\mathrm{U}\) and \(\mathrm{ClF}_{3}\) into \(\mathrm{UF}_{6}\) and \(\mathrm{Cl}_{2}\). (b) Is this a metathesis reaction? (c) Is this a redox reaction?

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) \(\begin{aligned} \mathrm{P}_{4}(s)+10 \mathrm{HClO}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow & \longrightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+10 \mathrm{HCl}(a q) \end{aligned}\) (b) \(\mathrm{Br}_{2}(l)+2 \mathrm{~K}(s) \longrightarrow 2 \mathrm{KBr}(s)\) (c) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)\) (d) \(\mathrm{ZnCl}_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow \mathrm{Zn}(\mathrm{OH})_{2}(s)+\) \(2 \mathrm{NaCl}(a q)\)

Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a), how could you distinguish any of the three magnesium substances from the other two?

Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF, (b) acetonitrile, \(\mathrm{CH}_{3} \mathrm{CN}\), (c) \(\mathrm{NaClO}_{4}\), (d) \(\mathrm{Ba}(\mathrm{OH})_{2}\).

You want to analyze a silver nitrate solution. (a) You could add \(\mathrm{HCl}(a q)\) to the solution to precipitate out \(\operatorname{AgCl}(s)\). What volume of a \(0.150 \mathrm{M} \mathrm{HCl}(a q)\) solution is needed to precipitate the silver ions from \(15.0 \mathrm{~mL}\) of a \(0.200 \mathrm{M} \mathrm{AgNO}_{3}\) solution? (b) You could add solid \(\mathrm{KCl}\) to the solution to precipitate out \(\mathrm{AgCl}(s)\). What mass of \(\mathrm{KCl}\) is needed to precipitate the silver ions from \(15.0 \mathrm{~mL}\) of \(0.200 \mathrm{MAgNO}_{3}\) solution? (c) Given that a \(0.150 \mathrm{M}\) \(\mathrm{HCl}(a q)\) solution costs \(\$ 39.95\) for \(500 \mathrm{~mL}\), and that \(\mathrm{KCl}\) costs \(\$ 10 /\) ton, which analysis procedure is more cost-effective?
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