Home >
Community >
Why is lead 2 chloride less soluble in dilute HCl but extremely soluble in concentrated HCl?
Upvote
17
Downvote
+ Solubility
+ Chemistry
+ Hydrochloric acid
Posted by
Mathematics and Physics
Why is lead 2 chloride less soluble in dilute HCl but extremely soluble in concentrated HCl?
Well, likely, complex ion formation occurs, to give a species such as [math][PbCl_{4}]^{2-}[/math], the which is MORE water-soluble than [math]PbCl_{2}[/math]. The high concentration of chloride ions in the acid solution promotes such complexation.
Well, likely, complex ion formation occurs, to give a species such as [math][PbCl_{4}]^{2-}[/math], the which is MORE water-soluble than [math]PbCl_{2}[/math]. The high concentration of chloride ions in the acid solution promotes such complexation.
Lead(II) chloride reacts with aqueous chloride ion to form soluble complexes of trichloridoplumbate(II) and tetrachloridoplumbate(II). PbCl₂(s) + Cl⁻(aq) ⇌ [PbCl₃]⁻ PbCl₂(s) + 2Cl⁻(aq) ⇌ [PbCl₄]²⁻
When the concentration Cl⁻ increases, according to Le Chatelier's principle, the equilibrium position will shift to the right and thus increase the solubility of lead(II) chloride. Hence, lead(II) chloride is only slightly soluble in dilute HCl, but is very soluble in concentrated HCl.
Lead(II) chloride reacts with aqueous chloride ion to form soluble complexes of trichloridoplumbate(II) and tetrachloridoplumbate(II). PbCl₂(s) + Cl⁻(aq) ⇌ [PbCl₃]⁻ PbCl₂(s) + 2Cl⁻(aq) ⇌ [PbCl₄]²⁻
When the concentration Cl⁻ increases, according to Le Chatelier's principle, the equilibrium position will shift to the right and thus increase the solubility of lead(II) chloride. Hence, lead(II) chloride is only slightly soluble in dilute HCl, but is very soluble in concentrated HCl.
At high concentrations of chloride ion, i.e. such as pertain in conc. hydrochloric, complex ions, [math]PbCl_{3}^{-}[/math], and [math]PbCl_{4}^{2-}[/math] may form….
At high concentrations of chloride ion, i.e. such as pertain in conc. hydrochloric, complex ions, [math]PbCl_{3}^{-}[/math], and [math]PbCl_{4}^{2-}[/math] may form….
It is soluble, but I have only carried out the experiment with relatively strong HCl, where the blue solution turns a strong yellow due to the formation of cuprochloric acid. So, you may get some yellow coloration, or green.
It is soluble, but I have only carried out the experiment with relatively strong HCl, where the blue solution turns a strong yellow due to the formation of cuprochloric acid. So, you may get some yellow coloration, or green.
Concentrated HCl is more corrosive as compared to dilute acids. An acid is said to be diluted when the concentration of H3O+ ions per unit volume of the solution reduces. The hydronium ion or H3O+ ion is responsible for giving acids their acidic property including the property of corrosion. A concentrated acid has a higher concentration of H3O+ ions per unit volume as compared to its diluted counterpart. Thus, the natural answer is that concentrated HCl is more corrosive as compared to diluted HCl.
Concentrated HCl is more corrosive as compared to dilute acids. An acid is said to be diluted when the concentration of H3O+ ions per unit volume of the solution reduces. The hydronium ion or H3O+ ion is responsible for giving acids their acidic property including the property of corrosion. A concentrated acid has a higher concentration of H3O+ ions per unit volume as compared to its diluted counterpart. Thus, the natural answer is that concentrated HCl is more corrosive as compared to diluted HCl.
Dissolution of a metal in HCl actually means that the metal has displaced H+ ions and form its own salt. However, copper is unable to displace H sine copper lies below H in electropositive character series.HNO3 is a strong oxidising agent also. Hence it rather oxidises copper to Cu2+ ions and hence copper dissolves in HNO3.
Dissolution of a metal in HCl actually means that the metal has displaced H+ ions and form its own salt. However, copper is unable to displace H sine copper lies below H in electropositive character series.HNO3 is a strong oxidising agent also. Hence it rather oxidises copper to Cu2+ ions and hence copper dissolves in HNO3.
One way you can figure it out is by putting it on your hand. If it’s concentrated, it’ll start to hurt real bad, if it’s diluted it’ll just feel a little tingly.
Granted I wouldn’t recommend doing it this way, there are other ways like using a known concentration NaOH and measuring the pH levels, but if you don’t have any of those things putting it on your arm would work.
One way you can figure it out is by putting it on your hand. If it’s concentrated, it’ll start to hurt real bad, if it’s diluted it’ll just feel a little tingly.
Granted I wouldn’t recommend doing it this way, there are other ways like using a known concentration NaOH and measuring the pH levels, but if you don’t have any of those things putting it on your arm would work.
Well, likely, complex ion formation occurs, to give a species such as [math][PbCl_{4}]^{2-}[/math], the which is MORE water-soluble than [math]PbCl_{2}[/math]. The high concentration of chloride ions in the acid solution promotes such complexation.
Well, likely, complex ion formation occurs, to give a species such as [math][PbCl_{4}]^{2-}[/math], the which is MORE water-soluble than [math]PbCl_{2}[/math]. The high concentration of chloride ions in the acid solution promotes such complexation.
More
VOTE
Lead(II) chloride reacts with aqueous chloride ion to form soluble complexes of trichloridoplumbate(II) and tetrachloridoplumbate(II).
PbCl₂(s) + Cl⁻(aq) ⇌ [PbCl₃]⁻
PbCl₂(s) + 2Cl⁻(aq) ⇌ [PbCl₄]²⁻
When the concentration Cl⁻ increases, according to Le Chatelier's principle, the equilibrium position will shift to the right and thus increase the solubility of lead(II) chloride. Hence, lead(II) chloride is only slightly soluble in dilute HCl, but is very soluble in concentrated HCl.
Lead(II) chloride reacts with aqueous chloride ion to form soluble complexes of trichloridoplumbate(II) and tetrachloridoplumbate(II).
PbCl₂(s) + Cl⁻(aq) ⇌ [PbCl₃]⁻
PbCl₂(s) + 2Cl⁻(aq) ⇌ [PbCl₄]²⁻
When the concentration Cl⁻ increases, according to Le Chatelier's principle, the equilibrium position will shift to the right and thus increase the solubility of lead(II) chloride. Hence, lead(II) chloride is only slightly soluble in dilute HCl, but is very soluble in concentrated HCl.
More
VOTE
Well lead chloride is moderately insoluble in aqueous solution…
[math]Pb^{2+} + 2Cl^{-} ightarrow PbCl_{2}(s)downarrow[/math]
At high concentrations of chloride ion, i.e. such as pertain in conc. hydrochloric, complex ions, [math]PbCl_{3}^{-}[/math], and [math]PbCl_{4}^{2-}[/math] may form….
[math]PbCl_{2}(s)uparrow + 2Cl^{-} ightarrow [PbCl_{4}]^{2-}[/math]
Well lead chloride is moderately insoluble in aqueous solution…
[math]Pb^{2+} + 2Cl^{-} ightarrow PbCl_{2}(s)downarrow[/math]
At high concentrations of chloride ion, i.e. such as pertain in conc. hydrochloric, complex ions, [math]PbCl_{3}^{-}[/math], and [math]PbCl_{4}^{2-}[/math] may form….
[math]PbCl_{2}(s)uparrow + 2Cl^{-} ightarrow [PbCl_{4}]^{2-}[/math]
More
VOTE
It is soluble, but I have only carried out the experiment with relatively strong HCl, where the blue solution turns a strong yellow due to the formation of cuprochloric acid. So, you may get some yellow coloration, or green.
It is soluble, but I have only carried out the experiment with relatively strong HCl, where the blue solution turns a strong yellow due to the formation of cuprochloric acid. So, you may get some yellow coloration, or green.
More
VOTE
Concentrated HCl is more corrosive as compared to dilute acids. An acid is said to be diluted when the concentration of H3O+ ions per unit volume of the solution reduces. The hydronium ion or H3O+ ion is responsible for giving acids their acidic property including the property of corrosion. A concentrated acid has a higher concentration of H3O+ ions per unit volume as compared to its diluted counterpart. Thus, the natural answer is that concentrated HCl is more corrosive as compared to diluted HCl.
Concentrated HCl is more corrosive as compared to dilute acids. An acid is said to be diluted when the concentration of H3O+ ions per unit volume of the solution reduces. The hydronium ion or H3O+ ion is responsible for giving acids their acidic property including the property of corrosion. A concentrated acid has a higher concentration of H3O+ ions per unit volume as compared to its diluted counterpart. Thus, the natural answer is that concentrated HCl is more corrosive as compared to diluted HCl.
More
VOTE
VOTE
Because it forms a complex, in concentrated acid!
PbCl2 + HCl → H2PbCl4.
Or PbCl2 +(2Cl-)–> [PbCl4]2-
In case of PbCl2, diluted hydrochloric acid suppresses it's solubity according to le Chatilier's principle.
Pb2+ + 2Cl- →PbCl2↓(s)
Because it forms a complex, in concentrated acid!
PbCl2 + HCl → H2PbCl4.
Or PbCl2 +(2Cl-)–> [PbCl4]2-
In case of PbCl2, diluted hydrochloric acid suppresses it's solubity according to le Chatilier's principle.
Pb2+ + 2Cl- →PbCl2↓(s)
More
VOTE
2 different aspects.
BaSO4 didn't dissolve in water due to extremely high lattice energy.
BaSO4 is actually reacting with PbCl2, mistakenly you call it soluble!
BaSO4 + PbCl2–> BaCl2+ PbSO4↓
2 different aspects.
BaSO4 didn't dissolve in water due to extremely high lattice energy.
BaSO4 is actually reacting with PbCl2, mistakenly you call it soluble!
BaSO4 + PbCl2–> BaCl2+ PbSO4↓
More
VOTE
One way you can figure it out is by putting it on your hand. If it’s concentrated, it’ll start to hurt real bad, if it’s diluted it’ll just feel a little tingly.
Granted I wouldn’t recommend doing it this way, there are other ways like using a known concentration NaOH and measuring the pH levels, but if you don’t have any of those things putting it on your arm would work.
One way you can figure it out is by putting it on your hand. If it’s concentrated, it’ll start to hurt real bad, if it’s diluted it’ll just feel a little tingly.
Granted I wouldn’t recommend doing it this way, there are other ways like using a known concentration NaOH and measuring the pH levels, but if you don’t have any of those things putting it on your arm would work.
More
VOTE