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Chapter 18: Problem 106

Which of the following barium salts should dissolve in a strong acid such as HCl: \(\mathrm{Ba}(\mathrm{OH})_{2}, \mathrm{BaSO}_{4},\) or \(\mathrm{BaCO}_{3} ?\)

Short Answer

Expert verified
Ba(OH)鈧� and BaCO鈧� dissolve in HCl, but BaSO鈧� does not.

Step by step solution

01

Identifying Potential Reactions

To determine which barium salts would dissolve in a strong acid like HCl, we need to consider how these compounds would react with HCl. Substances that contain basic anions that react with H鈦� ions will dissolve in the acid.
02

Assessing Basicity of Anions

Examine the anions present in each barium salt: - Ba(OH)鈧� contains OH鈦� ions, which readily react with H鈦� ions to form water. - BaSO鈧� contains SO鈧劼测伝 ions, which are not basic ions and do not react with H鈦� ions under normal conditions. - BaCO鈧� contains CO鈧兟测伝 ions, which react with H鈦� ions to form H鈧侰O鈧�, which decomposes into CO鈧� and water.
03

Reaction Outcomes

Considering possible reactions: - Ba(OH)鈧� + 2HCl 鈫� BaCl鈧� + 2H鈧侽. This dissolves because OH鈦� reacts with H鈦�. - BaSO鈧� + HCl 鈫� No significant reaction occurs, so it remains largely insoluble. - BaCO鈧� + 2HCl 鈫� BaCl鈧� + CO鈧� + H鈧侽. This dissolves because CO鈧兟测伝 reacts with H鈦� ions.
04

Conclusion on Solubility

Based on the reactions, Ba(OH)鈧� and BaCO鈧� are able to dissolve when reacted with HCl because they contain basic anions that react with the acid. BaSO鈧� does not dissolve significantly as its anion is not basic and does not react with H鈦� ions.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acid-Base Reaction
An acid-base reaction is a chemical process where an acid and a base interact. Strong acids like hydrochloric acid (HCl) are capable of donating protons (H鈦� ions) readily. Bases, on the other hand, can accept these protons. In the context of dissolving barium salts in HCl, we consider whether the anions in the salts can behave as a base.
  • For instance, hydroxide (OH鈦�) ions in barium hydroxide, \ \( \mathrm{Ba} (\mathrm{OH})_{2} \ \), accept H鈦� ions to form water.
  • Similarly, carbonate (CO鈧兟测伝) ions in barium carbonate, \ \( \mathrm{BaCO}_{3} \ \), react with H鈦� ions to produce carbonic acid, \ \( \mathrm{H}_2\mathrm{CO}_3 \ \), which then decomposes to carbon dioxide and water.
  • Barium sulfate, \ \( \mathrm{BaSO}_{4} \ \), however, contains sulfate ions (SO鈧劼测伝) that typically do not participate in acid-base reactions with strong acids.
Understanding this allows us to predict which barium salts might dissolve in a strong acid environment, based on active participation in an acid-base reaction.
Anion Basicity
Anion basicity refers to an anion's ability to accept protons (H鈦� ions) and participate in a reaction with acids. The basicity of an anion is crucial in understanding why some barium salts dissolve in hydrochloric acid (HCl), while others do not.
  • In \ \( \mathrm{Ba(OH)}_2 \ \), the OH鈦� anion is a strong base, readily reacting with H鈦� to form water, which facilitates dissolution.
  • In \ \( \mathrm{BaCO}_{3} \ \), the CO鈧兟测伝 anion is also basic. It reacts with H鈦� ions, eventually leading to the release of CO鈧� gas and water, making the salt soluble in acid.
  • On the other hand, SO鈧劼测伝 in \ \( \mathrm{BaSO}_{4} \ \) lacks basicity for meaningful reaction with H鈦�, rendering it largely insoluble in HCl.
Thus, analyzing the basicity of anions helps predict solubility trends of various salts in strong acids.
HCl Reaction
Reactions with hydrochloric acid (HCl) involve the interaction of its H鈦� ions with anions in compounds. Whether a barium salt dissolves in HCl depends heavily on this interaction.
  • Hydrochloric acid can effectively dissolve compounds containing anions that react to lower the free energy of the system, often via gas production or forming neutral molecules like water.
  • For \ \( \mathrm{Ba(OH)}_2 \ \), the reaction with HCl produces barium chloride (BaCl鈧�) and water, facilitating dissolution.
  • Similarly, \ \( \mathrm{BaCO}_{3} \ \) reacts with HCl to yield barium chloride, carbon dioxide (escaping as a gas), and water.
  • In contrast, \ \( \mathrm{BaSO}_{4} \ \) remains unchanged because sulfate ions do not efficiently bind with H鈦� ions.
By assessing the likely outcomes of HCl reactions, one can determine the extent to which each barium salt will dissolve in such an acidic environment.

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Most popular questions from this chapter

Name two insoluble salts of each of the following ions. (a) \(\mathrm{Cl}^{-}\) (b) \(\mathrm{Zn}^{2+}\) (c) \(\mathrm{Fe}^{2+}\)

Will a precipitate of \(\mathrm{Mg}(\mathrm{OH})_{2}\) form when \(25.0 \mathrm{mL}\) of \(0.010 \mathrm{M} \mathrm{NaOH}\) is combined with \(75.0 \mathrm{mL}\) of a \(0.10 \mathrm{M}\) solution of magnesium chloride?

Name two insoluble salts of each of the following ions. (a) \(\mathrm{SO}_{4}^{2-}\) (b) \(\mathrm{Ni}^{2+}\) (c) \(\mathrm{Br}^{-}\)

If the concentration of \(\mathrm{Zn}^{2+}\) in \(10.0 \mathrm{mL}\) of water is \(1.63 \times 10^{-4} \mathrm{M},\) will zinc hydroxide, \(\mathrm{Zn}(\mathrm{OH})_{2},\) precipitate when 4.0 mg of \(\mathrm{NaOH}\) is added?

Construct a rough plot of \(\mathrm{pH}\) versus volume of base for the titration of \(25.0 \mathrm{mL}\) of \(0.050 \mathrm{M} \mathrm{HCN}\) with \(0.075 \mathrm{M}\) \(\mathrm{NaOH}.\) (a) What is the pH before any \(\mathrm{NaOH}\) is added? (b) What is the pH at the halfway point of the titration? (c) What is the pH when \(95 \%\) of the required \(\mathrm{NaOH}\) has been added? (d) What volume of base, in milliliters, is required to reach the equivalence point? (e) What is the \(\mathrm{pH}\) at the equivalence point? (f) What indicator would be most suitable for this titration? (See Figure 18.10 .) (g) What is the pH when \(105 \%\) of the required base has been added?
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