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Chapter 17: Problem 61

Both \(\mathrm{KCl}\) and \(\mathrm{NH}_{4} \mathrm{Cl}\) are white solids. Suggest one reagent that would enable you to distinguish between these two compounds.

Short Answer

Expert verified
The reagent that can be used to distinguish between KCl and NH4Cl is sodium hydroxide (NaOH). When mixed with the compounds, NH4Cl reacts to form NH3 gas with a strong smell, whereas KCl remains unreactive.

Step by step solution

01

Understanding the properties of KCl and NH4Cl

Potassium Chloride (KCl) and Ammonium Chloride (NH4Cl) are both Chlorides but have different cations. KCl consists of K+ and Cl- ions. NH4Cl consists of NH4+ and Cl- ions. The primary difference between them lies in their cations.
02

Choosing the right reagent

When considering a reagent to distinguish between these two compounds, we need to think of a reagent that would react differently with NH4+ and K+. One possible reagent is NaOH (Sodium Hydroxide).
03

Explaining the action of the reagent

When Sodium Hydroxide (NaOH) is added to these compounds, it will react differently. NH4Cl reacts with NaOH to release ammonia gas (NH3), which has a distinct sharp, pungent smell. On the other hand, KCl does not react with NaOH, and there would be no gas evolved.

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Most popular questions from this chapter

What are the criteria for choosing an indicator for a particular acid-base titration?

Calculate the concentration of ions in these saturated solutions: (a) \(\left[\mathrm{I}^{-}\right]\) in AgI solution with \(\left[\mathrm{Ag}^{+}\right]=9.1 \times 10^{-9} \mathrm{M}\) (b) \(\left[\mathrm{Al}^{3+}\right]\) in \(\mathrm{Al}(\mathrm{OH})_{3}\) with \(\left[\mathrm{OH}^{-}\right]=2.9 \times 10^{-9} \mathrm{M}\)

Define solubility, molar solubility, and solubility product. Explain the difference between solubility and the solubility product of a slightly soluble substance such as \(\mathrm{BaSO}_{4}\) .

The amount of indicator used in an acid-base titration must be small. Why?

Acid-base reactions usually go to completion. Confirm this statement by calculating the equilibrium constant for each of the following cases: (a) a strong acid reacting with a strong base, (b) a strong acid reacting with a weak base \(\left(\mathrm{NH}_{3}\right),\) (c) a weak acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\) reacting with a strong base, \((\mathrm{d})\) a weak acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\) reacting with a weak base \(\left(\mathrm{NH}_{3}\right)\) (Hint: Strong acids exist as \(\mathrm{H}^{+}\) ions and strong bases exist as \(\mathrm{OH}^{-}\) ions in solution. You need to look up the \(K_{\mathrm{a}}, K_{\mathrm{b}}\), and \(K_{\mathrm{w}}\) values.)
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