1. Which salt will precipitate first upon addition of AgNO3 to a solution contai
ID: 947690 • Letter: 1
Question
1. Which salt will precipitate first upon addition of AgNO3 to a solution containing Cl- and I-?
A. AgCl, Ksp=1.8X10^-10
B. AgI, Ksp=8.5X10^-17
2.
The amount of chloride in a water sample was determined by potentiometric titration using AgNO3 as the titrant. 25.00 mL of the water sample was placed in a beaker. It took 18.90 mL of 0.08541 M AgNO3 to reach the equivalence point.
What is the net ionic equation for the precipitation reaction that takes place?
A. Ag+ (aq) + NO3- (aq) AgNO3 (s)
B Ag+ (aq) + Cl- (aq) AgCl (s)
3.
The amount of chloride in a water sample was determined by potentiometric titration using AgNO3 as the titrant. 25.00 mL of the water sample was placed in a beaker. It took 18.90 mL of 0.08541 M AgNO3 to reach the equivalence point.
Determine the concentration of Cl- in the water sample.
A. 0.08080M
B. 0.06457M
c. 0.1130M
D.1.34X10^-5M
Explanation / Answer
1) AgCl(s) <-------> Ag+(aq) + Cl-(aq)
Ksp = [Ag+]*[Cl-]
Thus, greater the Ksp value , slower it will precipitate
Thus, AgI will precipitate first.
2) The net ionic equation is :-
Ag+(aq) + Cl-(aq) ------> AgCl(s)
3) moles of Cl- = moles of AgNO3 used = molar concentration*volume of solution in litres = 0.08541*0.0189 = 0.00161
Thus, molar concentration of Cl- = moles/volume of water sample in litres = 0.00161/0.025 = 0.0646 M
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