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Chapter 4: Problem 35

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,\(\mathrm{CH}_{3} \mathrm{CN},(\mathbf{c}) \mathrm{NaClO}_{4},(\mathbf{d}) \mathrm{Ba}(\mathrm{OH})_{2} .\)

Short Answer

Expert verified
(a) HF is an acid, existing as a mixture of molecules and ions in aqueous solution. (b) Acetonitrile (CH₃CN) is none of the above and exists almost entirely in molecular form in an aqueous solution. (c) NaClO₄ is a salt, existing as ions in an aqueous solution. (d) Ba(OH)₂ is a strong base, existing as ions in an aqueous solution.

Step by step solution

01

(a) HF

Hydrogen Fluoride (HF) is a binary compound of hydrogen and a halogen (fluorine). HF is an acid, specifically a hydrohalic acid. In an aqueous solution, it forms hydrogen ions (H+) and fluoride ions (F−). Therefore, HF exists in aqueous solution as a mixture of molecules and ions.
02

(b) Acetonitrile (CH₃CN)

Acetonitrile (CH₃CN) is an organic compound which does not contain any ionizable hydrogen or hydroxide ions. It is not an acid, a base, or a salt. In an aqueous solution, it exists almost entirely in molecular form, as the interaction with water molecules is weak.
03

(c) NaClO₄

Sodium perchlorate (NaClO₄) is a compound consisting of a metal (sodium) and a nonmetal polyatomic ion (perchlorate). Thus, it is classified as a salt. In an aqueous solution, NaClO₄ dissociates completely into sodium ions (Na⁺) and perchlorate ions (ClO₄⁻), making it exist as ions in solution.
04

(d) Ba(OH)₂

Barium hydroxide (Ba(OH)₂) is a compound composed of a metal (barium) and hydroxide ions (OH⁻). It is a strong base. In an aqueous solution, it dissociates completely into barium ions (Ba²⁺) and hydroxide ions (OH⁻), so it exists as ions in aqueous solution.

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Most popular questions from this chapter

Predict whether each of the following compounds is soluble in water: \((\mathbf{a})\mathrm{AgI},(\mathbf{b}) \mathrm{Na}_{2} \mathrm{CO}_{3},(\mathbf{c}) \mathrm{BaCl}_{2},(\mathbf{d}) \mathrm{Al}(\mathrm{OH})_{3}$$(\mathbf{e})\mathrm{Zn}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\).

The mass percentage of chloride ion in a 25.00 -mL. sample of seawater was determined by titrating the sample with silver nitrate, precipitating silver chloride. It took 42.58 \(\mathrm{mL}\) of 0.2997 M silver nitrate solution to reach the equivalence point in the titration. What is the mass percentage of chloride ion in seawater if its density is 1.025 \(\mathrm{g} / \mathrm{mL}\) ?

The U.S. standard for arsenate in drinking water requires that public water supplies must contain no greater than 10 parts per billion \((\mathrm{ppb})\) arsenic. If this arsenic is present as arsenate, AsO \(_{4}^{3-},\) what mass of sodium arsenate would be present in a 1.00 -L sample of drinking water that just meets the standard? Parts per billion is defined on a mass basis as $$\mathrm{ppb}=\frac{\text { g solute }}{\mathrm{g} \text { solution }} \times 10^{9}$$

Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the aqueous HCl in the stomach and each of the following substances used in various antacids: (a) \(\mathrm{Al}(\mathrm{OH})_{3}(\mathrm{s}),\) (b) \(\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s})\), \((\mathbf{c}) \mathrm{MgCO}_{3}(s)\), \((\mathbf{d}) \mathrm{NaAl}\left(\mathrm{CO}_{3}\right)(\mathrm{OH})_{2}(s),\) (e) \(\mathrm{CaCO}_{3}(\mathrm{s}).\)

A solid sample of \(\mathrm{Zn}(\mathrm{OH})_{2}\) is added to 0.350 \(\mathrm{L}\) of 0.500 \(\mathrm{M}\) aqueous HBr. The solution that remains is still acidic. It is then titrated with 0.500 \(\mathrm{MNaOH}\) solution, and it takes 88.5 mL of the NaOH solution to reach the equivalence point. What mass of \(\mathrm{Zn}(\mathrm{OH})_{2}\) was added to the HBr solution?
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