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Chapter 18: Problem 32

(A) All sulphates give white precipitate with \(\mathrm{BaCl}_{2}\) solution. (R) \(\mathrm{BaSO}_{4}\) is insoluble in water.

Short Answer

Expert verified
R correctly explains A; both are true.

Step by step solution

01

Understanding the Assertion

The Assertion (A) states that when sulphates are mixed with barium chloride solution, they form a white precipitate. This implies that there is a chemical reaction between sulphates and barium chloride, resulting in a solid product that does not dissolve in the solution, hence appearing as a white precipitate.
02

Understanding the Reason

The Reason (R) provided is that barium sulphate (\(\mathrm{BaSO}_{4}\)) is insoluble in water. This implies that when barium ions (\(\mathrm{Ba}^{2+}\)) from barium chloride react with sulphate ions (\(\mathrm{SO}_{4}^{2-}\)), they form barium sulphate which precipitates out of the solution because it does not dissolve in water.
03

Evaluating the Connection between A and R

To decide if R is a correct explanation of A, check if the solubility of \(\mathrm{BaSO}_{4}\) is indeed the reason for the precipitate described in A. Since \(\mathrm{BaSO}_{4}\) forms by the reaction of \(\mathrm{BaCl}_{2}\) with sulphates and is insoluble, it accounts for the formation of the white precipitate. Thus, R correctly explains A.

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Key Concepts

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

Barium Sulfate Insolubility
Barium sulfate, denoted as \(\mathrm{BaSO}_4\), is a compound known for its remarkable insolubility in water. When barium ions \((\mathrm{Ba}^{2+})\) interact with sulfate ions \((\mathrm{SO}_4^{2-})\), they form barium sulfate, which does not dissolve in water because of its strong ionic lattice structure.

This insoluble characteristic means that, once formed, barium sulfate will remain as a solid within a solution, rather than dissolving.
  • Insoluble Characteristic: Barium sulfate retains a solid form in water.
  • Practical Applications: This insolubility is leveraged in various medical and industrial applications, such as in radiographic imaging, where it is used as a contrast agent due to its opacity to X-rays.
Understanding its insolubility is crucial, as it explains why a white precipitate forms in reactions involving sulfate ions and barium ions.
Sulfate Ions
Sulfate ions, represented by \((\mathrm{SO}_4^{2-})\), are common anions found in many chemical compounds. They consist of one sulfur atom covalently bonded to four oxygen atoms, and they carry a 2- charge.

These ions are prevalent in a variety of chemical reactions and can form insoluble compounds, such as barium sulfate, when they meet barium ions.
  • Charge and Structure: The tetrahedral arrangement gives the sulfate ion its distinct shape and charge.
  • Role in Precipitates: Sulfate ions readily combine with multiple cations to form various precipitates; their interaction with barium ions is a classic example of a precipitation reaction.
The understanding of sulfate ions is essential for predicting and explaining the outcomes of chemical reactions involving sulfate compounds.
Chemical Reaction Explanation
When barium chloride \((\mathrm{BaCl}_2)\) solution is mixed with a sulfate compound in water, a significant chemical reaction occurs. In this reaction, barium ions \((\mathrm{Ba}^{2+})\) from the barium chloride combine with sulfate ions \((\mathrm{SO}_4^{2-})\) from the sulfate compound.

The result is the formation of barium sulfate \((\mathrm{BaSO}_4)\), a solid white precipitate that does not dissolve in the solution.

Steps of the Reaction:
  • The sulfate ions in the solution are attracted to the barium ions.
  • This attraction leads to the formation of an insoluble compound: \(\mathrm{BaSO}_4\).
  • Due to the insolubility, the newly formed barium sulfate settles as a white precipitate.
Such precipitation reactions are pivotal in analytical chemistry for identifying and quantifying the presence of specific ions in a solution.

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Most popular questions from this chapter

\(0.1435 \mathrm{~g}\) of \(\mathrm{AgCl}\) is obtained from \(20 \mathrm{~mL} \mathrm{HCl}^{*}\). What is the normality of the acid ? (a) \(0.5 \mathrm{~N}\) (b) \(0.1 N\) (c) \(0.05 N\) (d) \(1.0 \mathrm{~N}\)

Potassium iodide is added to freshly precipitated mercury (II) iodide. Which is/are the correct statement/s ? (a) The precipitate will dissolve (b) The solution possesses the anion \(\left[\mathrm{Hgl}_{4}\right]^{2-}\) (c) The solution can be used for the test of ammonium ion (d) All the above statements are wrong

Compound ' \(A\) ' gives white ppt. with \(\mathrm{HgCl}_{2}\). The name of white compound is : (a) Calomel (b) Corrosive sublimate (c) Vermilon (d) Millon's base

When a pinch of a salt is added to dilute acid, it evolves a gas that turns acidified \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) green. The sulphide precipitate in fourth group is dissolved in aquaregia. The solution when shaken with sodium bicarbonate and bromine water develops apple green colour. The basic and acidic radicals of the salt are : (a) \(\mathrm{Ni}^{2+}, \mathrm{SO}_{3}^{2-}\) (b) \(\mathrm{Co}^{2+}, \mathrm{SO}_{3}^{2-}\) (c) \(\mathrm{Ni}^{2+}, \mathrm{S}^{2-}\) (d) \(\mathrm{Co}^{2+}, \mathrm{SO}_{4}^{2-}\)

Haemoglobin contains \(0.33 \%\) iron by mass. If the molecular mass of haemoglobin is 68000 , how many iron atoms are present in each molecule of haemoglobin ? (a) 1 (b) 2 [ (c) 3 (d) 4
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