Give the group number where the cation belongs 1. Mercurous(Hg2-) ion gives a white precipitate with 0.1 MHCI- 2. Bismuth (Bi3-) ion does not give a precipitate with HCI but gives a black precipitate with thioacetamide in the presence of HCI. 3. Ammonium (NH4*) ion does not give precipitate with any precipitating agent. 4. Magnesium (Mg²+) ion does not give a precipitate with HCI or thioacetamide but give a white solid product with NazCOa. 5. Cobalt (Co2+) ion does not give a solid product with HCl and thioacetamide unless the solution is treated with excess NH4OH.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![Give the group number where the cation belongs
1. Mercurous(Hg2+) ion gives a white precipitate with 0.1 MHGI.
2. Bismuth (Bi3-) ion does not give a precipitate with HCI but gives a black
precipitate with thioacetamide in the presence of HCI.
3. Ammonium (NHe*) ion does not give precipitate with any precipitating
agent.
4. Magnesium (Mg2+) ion does not give a precipitate with HCI or
thioacetamide but give a white solid product with Na2COa.
5. Cobalt (Co2+) ion does not give a solid product with HCI and
thioacetamide unless the solution is treated with excess NH4OH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbd17d91e-1dd9-4cc8-a115-13afbacebf88%2F5f3bc641-f5d1-4bc0-b0a9-e01d5413863d%2F4yv1qyk_processed.png&w=3840&q=75)
![Group I (Ag+, Pb2+, Hg2+) cations produce insoluble chlorides so they can be
precipitated with dilute HCI, while all other cations remain in solution.
Group II (Cu2+, Bi3+, Cd2+, Hg2+, As3+, Sb3+, Sn4+) cations produce very insoluble
sulfides (Ksp values less than 10-30) so they can be precipitated by low amounts of
sulfide ion; this can be achieved by adding an acidic solution of H2S.
Group III (A13+, Cr3+, Fe3+, Zn2+, Ni2+, Co2+, Mn2+) cations produce slightly soluble
sulfides (Ksp values more than 10-20) so they can be precipitated by relatively high
amounts of sulfide ion; this can be achieved by adding a basic solution of H2S.
Group IV (Mg2+, Ca2+, Sr2+, Ba2+) cations, as well as all of the above groups,
produce insoluble carbonates so they can be precipitated by the addition of carbonate
once the ions of the first three groups have been removed.
Group V (Na+, K+, NH4 +) cations do not precipitate with any of the above reagents.
Moreover, you can supplement your knowledge on this by reading or researching about
solubility rules.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbd17d91e-1dd9-4cc8-a115-13afbacebf88%2F5f3bc641-f5d1-4bc0-b0a9-e01d5413863d%2Fqlhkhw_processed.png&w=3840&q=75)
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