Assuming that no equilibria other than dissolution are involved, calculate the concentration (in M) of all solute species in each of the following solutions of salts in contac with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected under the 5% rule. (See the Solubility-Pr Constants table. Assume K = 1.01 x 10-14.) (a) TIBr in 1.320 M HBr [TI+] [Br] [H] % error due to approximation (b) PbI₂ in 0.0368 M MgI2 [Pb2+] [I] [Mg2+] M M M % M M M 0
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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.
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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
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Assuming that no equilibria other than dissolution are involved, calculate the concentration (in M) of all solute species in each of the following solutions of salts in contact
with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected under the 5% rule. (See the Solubility-Prom
Constants table. Assume Kw = 1.01 x 10-14.)
(a) TIBr in 1.320 M HBr
[TI+]
[Br]
[H+]
% error due to approximation
(b) PbI, in 0.0368 M MgI₂
[Pb²+]
[I]
[Mg²+]
% error due to approximation
M
]
M
[OH ]
% error due to approximation
M
%
M
(c) Ag₂ CrO4 in 0.230 L of a solution containing 0.876 g of K₂ CrO 4
[Ag+]
[Cro42-]
[K+]
% error due to approximation
M
M
%
M
(d) Co(OH)₂ in a solution buffered at a pH of 10.975
[Co²+
M
M
%
M
M
%
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