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It is probably because a part of the oxygen produced from the reaction of KmnO4 and HCl is used up in oxidising the HCl to Cl2 gas
It would change your results because concentrated HCl is more acidic then H2SO4, therefore, there would be a larger change in pH quicker.
HNO3 is not used in redox titration because being a good oxidising ageant it oxidises the compound itself whereas HCL is a very volatile and it takes part in the reaction therefore H2SO4 is used in the reaction
KMnO4 will oxidize the HCl to Cl2 gas, a potentially hazardous vapor.
marri bhi yahi doubt se bhaI DUR KARAN ALE NE 10 Rs E NAAM
It is probably because a part of the oxygen produced from the reaction of KmnO4 and HCl is used up in oxidising the HCl to Cl2 gas
It would change your results because concentrated HCl is more acidic then H2SO4, therefore, there would be a larger change in pH quicker.
HNO3 is not used in redox titration because being a good oxidising ageant it oxidises the compound itself whereas HCL is a very volatile and it takes part in the reaction therefore H2SO4 is used in the reaction
KMnO4 will oxidize the HCl to Cl2 gas, a potentially hazardous vapor.
2 KMnO4 + 16 HCl = 5 Cl2 + 8 H2O + 2 KCl + 2 MnCl2
KMnO4 + HCl = Cl2 + H2O + KCl + MnCl2 After you balance it: 2KMnO4 + 16HCl = 5Cl2 + 8H2O + 2KCl + 2MnCl2
For preparation of standard solution of Mohr salt {FeSO4.(NH4)2SO4.6H2O}, it's necessary to add dilute H2SO4 to prevent the Fe2+ ions of Mohr salt solution from undergoing oxidation (to Fe3+). Just try to prepare the standard solution without adding this acid. You'll observe that your "Mohr solution" will become yellow in colour, i.e., it won't remain "Mohr salt solution" anymore, hence can't be used in titration. And while doing the titration of the Mohr salt solution with KMnO4 (or even with K2Cr2O7), you need to add dilute H2SO4. The reason is well explained by the chemical equation involved: reduction: (MnO4)- + 8H+ + 5e ----> Mn2+ + 4H2O oxidation: Fe2+ ----> Fe3+ + e net equation: (MnO4)- + 8H+ + 5Fe2+ ----> Mn2+ + 4H2O + 5Fe3+ There is involvement of H+ ions in this reaction. This redox titration requires acidic medium. Moreover, KMnO4 acts as a very good oxidizing agent in the presence of acidic medium, than in the basic and neutral medium. NOTE: Now a query may arise that for providing acidic medium, can HCl or HNO3 be used? (Let me tell you it's one of the favourite questions of external examiners) The answer is NO, because HNO3 is a very strong oxidizing agent. So, the Fe2+ present will be oxidized both by KMnO4 and HNO3, which will result in an error in determination of volume of KMnO4 reacting with Mohr salt solution. Also, HCl can't be used because Cl- from HCl will be oxidized by KMnO4: HCl (aq) ---> H+ (aq) +Cl- (aq) oxidation by KMnO4=> 2Cl- ----> Cl2 + 2e So, some extra KMnO4 will be used up because it will oxidize both- Cl- as well as Fe2+, => error in titration.
HCL is used to provide the acidic conditions required in the iodometeric titration.
Yaa, but not useful, because Hcl will release Cl whihc will oxidized by KMno4 and HNO3 is it self a good oxidizing acid.
Because sulphuric acid is non volatile and its sulphate ion is not interfering during the titration process while HCl is a volatile substance and its chloride ion interfere in the reaction as a reducing agent.
LiCl+H2SO4=LiHSO4+HCl