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In which of the following solvents, AgBr will have the highest solubility ? [1992]
- a)10-3 M NaBr
- b)10-3 M NH4 OH
- c)Pure water
- d)10-3 M HBr
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
In which of the following solvents, AgBr will have the highest solubil...
AgBr has the highest solubility in 10-3 M NH4OH . All other solven ts will dissolve AgBr poorly. Moreover bromides of Ag+, Hg22+ and Cu22+ are water insoluble
Most Upvoted Answer
In which of the following solvents, AgBr will have the highest solubil...
Explanation:
To determine which solvent will have the highest solubility for AgBr, we need to consider the solubility rules and the effect of the solvent on the dissociation of AgBr.
Solubility Rules:
- Most nitrate (NO3-) salts are soluble.
- Most salts containing Group 1 metals (Li+, Na+, K+, etc.) and ammonium (NH4+) are soluble.
- Most chloride (Cl-), bromide (Br-), and iodide (I-) salts are soluble.
- Most sulfate (SO42-) salts are soluble.
- Most hydroxide (OH-) salts are slightly soluble.
- Most sulfide (S2-) and carbonate (CO32-) salts are insoluble.
Effect of Solvent:
The solubility of a solute is influenced by the nature of the solvent. In this case, we are comparing four different solvents:
a) 10-3 M NaBr
b) 10-3 M NH4 OH
c) Pure water
d) 10-3 M HBr
Explanation of Options:
a) 10-3 M NaBr:
- NaBr is a soluble salt according to the solubility rules.
- However, the presence of a high concentration of Na+ ions may cause AgBr to precipitate due to the common ion effect. Therefore, the solubility of AgBr may not be very high in this solvent.
b) 10-3 M NH4 OH:
- NH4OH is a weak base and a weak electrolyte. It partially dissociates into NH4+ and OH- ions.
- AgBr is a slightly soluble salt according to the solubility rules.
- The presence of OH- ions in the solution can react with Ag+ ions to form AgOH, which is even less soluble than AgBr.
- This reaction helps to shift the equilibrium towards the dissociation of AgBr, increasing its solubility.
c) Pure water:
- Pure water is a neutral solvent and does not contain any ions.
- AgBr is a slightly soluble salt according to the solubility rules.
- The solubility of AgBr in pure water will be lower compared to the solvent in option b) because there are no ions present to help with the dissociation.
d) 10-3 M HBr:
- HBr is a strong acid and a strong electrolyte. It completely dissociates into H+ and Br- ions.
- AgBr is a slightly soluble salt according to the solubility rules.
- The presence of a high concentration of Br- ions may cause AgBr to precipitate due to the common ion effect. Therefore, the solubility of AgBr may not be very high in this solvent.
Conclusion:
Among the given options, option b) 10-3 M NH4 OH will have the highest solubility for AgBr because the presence of OH- ions will help to shift the equilibrium towards the dissociation of AgBr.
To determine which solvent will have the highest solubility for AgBr, we need to consider the solubility rules and the effect of the solvent on the dissociation of AgBr.
Solubility Rules:
- Most nitrate (NO3-) salts are soluble.
- Most salts containing Group 1 metals (Li+, Na+, K+, etc.) and ammonium (NH4+) are soluble.
- Most chloride (Cl-), bromide (Br-), and iodide (I-) salts are soluble.
- Most sulfate (SO42-) salts are soluble.
- Most hydroxide (OH-) salts are slightly soluble.
- Most sulfide (S2-) and carbonate (CO32-) salts are insoluble.
Effect of Solvent:
The solubility of a solute is influenced by the nature of the solvent. In this case, we are comparing four different solvents:
a) 10-3 M NaBr
b) 10-3 M NH4 OH
c) Pure water
d) 10-3 M HBr
Explanation of Options:
a) 10-3 M NaBr:
- NaBr is a soluble salt according to the solubility rules.
- However, the presence of a high concentration of Na+ ions may cause AgBr to precipitate due to the common ion effect. Therefore, the solubility of AgBr may not be very high in this solvent.
b) 10-3 M NH4 OH:
- NH4OH is a weak base and a weak electrolyte. It partially dissociates into NH4+ and OH- ions.
- AgBr is a slightly soluble salt according to the solubility rules.
- The presence of OH- ions in the solution can react with Ag+ ions to form AgOH, which is even less soluble than AgBr.
- This reaction helps to shift the equilibrium towards the dissociation of AgBr, increasing its solubility.
c) Pure water:
- Pure water is a neutral solvent and does not contain any ions.
- AgBr is a slightly soluble salt according to the solubility rules.
- The solubility of AgBr in pure water will be lower compared to the solvent in option b) because there are no ions present to help with the dissociation.
d) 10-3 M HBr:
- HBr is a strong acid and a strong electrolyte. It completely dissociates into H+ and Br- ions.
- AgBr is a slightly soluble salt according to the solubility rules.
- The presence of a high concentration of Br- ions may cause AgBr to precipitate due to the common ion effect. Therefore, the solubility of AgBr may not be very high in this solvent.
Conclusion:
Among the given options, option b) 10-3 M NH4 OH will have the highest solubility for AgBr because the presence of OH- ions will help to shift the equilibrium towards the dissociation of AgBr.
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In which of the following solvents, AgBr will have the highest solubility ? [1992]a)10-3 M NaBrb)10-3 M NH4 OHc)Pure waterd)10-3 M HBrCorrect answer is option 'B'. Can you explain this answer?
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