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Chapter 4: Problem 30

Identify the following as a weak or strong acid or base: (a) \(\mathrm{NH}_{3},\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{4},\) (c) \(\mathrm{LiOH}\), (d) \(\mathrm{HCOOH}\) (formic acid), (e) \(\mathrm{H}_{2} \mathrm{SO}_{4},\) (f) \(\mathrm{HF},(\mathrm{g}) \mathrm{Ba}(\mathrm{OH})_{2}\).

Short Answer

Expert verified
(a) \(\mathrm{NH}_{3}\) - weak base, (b) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) - weak acid, (c) \(\mathrm{LiOH}\) - strong base, (d) \(\mathrm{HCOOH}\) - weak acid, (e) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) - strong acid, (f) \(\mathrm{HF}\) - weak acid, (g) \(\mathrm{Ba}(\mathrm{OH})_{2}\) - strong base.

Step by step solution

01

Identify the nature of \(\mathrm{NH}_{3}\)

Ammonia, \(\mathrm{NH}_{3}\), is a base because it accepts protons (H+) from water to form ammonium ions (\(\mathrm{NH}_{4}^{+}\)). However, it doesn't dissociate completely in water, so it is considered a weak base.
02

Identify the nature of \(\mathrm{H}_{3} \mathrm{PO}_{4}\)

Phosphoric acid, \(\mathrm{H}_{3}\mathrm{PO}_{4}\), is an acid because it donates protons (H+) to water. But it doesn't fully ionize in water, so it's a weak acid.
03

Identify the nature of \(\mathrm{LiOH}\)

Lithium hydroxide, \(\mathrm{LiOH}\), is a base. It completely dissociates in water to form Li+ and OH− ions, hence it is categorized as a strong base.
04

Identify the nature of \(\mathrm{HCOOH}\)

Formic acid, \(\mathrm{HCOOH}\), is an acid. It donates protons (H+) to water, but doesn't do so fully, therefore it's a weak acid.
05

Identify the nature of \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

Sulfuric acid, \(\mathrm{H}_{2}\mathrm{SO}_{4}\), is a strong acid because it donates protons (H+) and fully ionizes in water.
06

Identify the nature of \(\mathrm{HF}\)

Hydrofluoric acid, \(\mathrm{HF}\), is an acid, but it doesn't fully ionize in water, so it is a weak acid.
07

Identify the nature of \(\mathrm{Ba}(\mathrm{OH})_{2}\)

Barium hydroxide, \(\mathrm{Ba}(\mathrm{OH})_{2}\), is a strong base. This is because it fully dissociates in water to produce Ba2+ and OH− ions.

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Most popular questions from this chapter

A \(35.2-\mathrm{mL}, 1.66 M \mathrm{KMnO}_{4}\) solution is mixed with \(16.7 \mathrm{~mL}\) of \(0.892 \mathrm{M} \mathrm{KMnO}_{4}\) solution. Calculate the concentration of the final solution.

Sodium carbonate \(\left(\mathrm{Na}_{2} \mathrm{CO}_{3}\right)\) is available in very pure form and can be used to standardize acid solutions. What is the molarity of a HCl solution if \(28.3 \mathrm{~mL}\) of the solution are required to react with \(0.256 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{CO}_{3} ?\)

On standing, a concentrated nitric acid gradually turns yellow. Explain. (Hint: Nitric acid slowly decomposes. Nitrogen dioxide is a colored gas.)

Classify the following redox reactions. (a) \(2 \mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}\) (b) \(\mathrm{Mg}+2 \mathrm{AgNO}_{3} \longrightarrow \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}+2 \mathrm{Ag}\) (c) \(\mathrm{NH}_{4} \mathrm{NO}_{2} \longrightarrow \mathrm{N}_{2}+2 \mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{H}_{2}+\mathrm{Br}_{2} \longrightarrow 2 \mathrm{HBr}\)

A 5.012 -g sample of an iron chloride hydrate was dried in an oven. The mass of the anhydrous compound was \(3.195 \mathrm{~g}\). The compound was then dissolved in water and reacted with an excess of \(\mathrm{AgNO}_{3} .\) The AgCl precipitate formed weighed 7.225 g. What is the formula of the original compound?
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