Enter a balanced net ionic equation to describe the reactions indicated. Enter NR if no reaction occurred.
Suppose you determine a pH of 0 to 1 for an unknown solution. When mixed in equal volumes, which of the following solutions could have generated an unknown solution consistent with this pH measurement?
a) NH4Br and AgNO3
b) CuSO4 and BaCl2
c) LiOH and HCl
d) HCl and NH4Br
e) K2CO3 and Na2S
Net ionic reactions are written for those whose products gives solid precipitates.
a) Ag+(aq) + Br- (aq)---------------------> AgBr(s)
b) Ba2+(aq) + SO42-(aq) -------------------> BaSO4(s)
c) NR
d) NR
e) NR
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The pH of the resultant solution is given as 0 to 1 which means it should be strongly acidic solution. Only the the mixture of HCl and NH4Br produces the pH shown/ required. Since the Hydrobromic acid produced in option d is very strong acid.
HCl(aq) + NH4Br(aq) -------------------------> HBr(aq) + NH4Cl (aq)
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The rest of the mixtures produces insignificant inorganic salts which are not capable enough to yield a an unknown solution of pH 0 to 1
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The option c can be a neutral solution , since it is a combination of base and acid.
The option e can be a basic solution.
options a and b are insignificant in yielding acidic solutions of pH range 0 to 1
Enter a balanced net ionic equation to describe the reactions indicated. Enter NR if no reaction...
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