Question
In: Chemistry
You mix 5.00 mL of 1.0 x 10-5M AgNO3 with 10.00mL of 2.00M NH3 solution resulting...
You mix 5.00 mL of 1.0 x 10-5M AgNO3 with 10.00mL of 2.00M NH3 solution resulting in the formation of the diamminesilver(I) complex ion, [Ag(NH3)2]+. (Assume volumes are additive.)
a) Write the net-ionic equilibrium equation for the formation of this complex ion.
b) Calculate the concentration of the complex ion in the reaction mixture.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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1. If you mix a 10 mL of a 0.1 solution of glucose with a 10 mL
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3. How does the conductance of a weak electrolyte change as the
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adding 50.0 mL of 1.0 x 10^-3 M Sr(NO3)2 and 50.0 mL of 1.0 x 10^-3...
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ksp of SrCO3 = 1.1 x 10^-10
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After mixing 5.00 mL of the 5.0×10–5 M crystal violet solution
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OH– is much greater than that of CV+? Why is this an important
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A student mixes 5.00 mL of 2.00 x 10‐3 M Fe(NO3)3 with 5.00 mL 2.00 x...
A student mixes 5.00 mL of 2.00 x 10‐3 M Fe(NO3)3 with 5.00 mL
2.00 x 10‐3 M KSCN. She finds that in the equilibrium mixture the
concentration of FeSCN+2 is 1.40 x 10‐4 M.
What is the initial concentration in solution of the Fe+3 and
SCN‐?
What is the equilibrium constant for the reaction?
What happened to the K+ and the NO3‐ ions in this solution?
You make two dilutions. You take 82.19 mL of the stock solution (8.1×10-5M) and dilute to...
You make two dilutions. You take 82.19 mL of the stock solution
(8.1×10-5M) and dilute to 500.0 mL to
make Solution #1. You then add 66.26 mL of Solution #1 to 30.11 mL
of water to make Solution #2.
What is the concentration of the Solution #1 in terms of
molarity?
What is the concentration of the Solution #2 in terms of
molarity?
A 130.0 mL sample of a solution that is 2.7×10−3 M in AgNO3 is mixed with...
A 130.0 mL sample of a solution that is 2.7×10−3 M in
AgNO3 is mixed with a 230.0 mL sample of a solution that
is 0.14 M in NaCN.
After the solution reaches equilibrium, what concentration of
Ag+(aq) remains?
A 130.0 mL sample of a solution that is 2.7×10−3 M in AgNO3 is mixed with...
A 130.0 mL sample of a solution that is 2.7×10−3 M in
AgNO3 is mixed with a 230.0 mL sample of a solution that
is 0.14 M in NaCN.
After the solution reaches equilibrium, what concentration of
Ag+(aq) remains?
A 125.0 −mL sample of a solution that is 2.9×10−3 M in AgNO3 is mixed with...
A 125.0 −mL sample of a solution that is 2.9×10−3 M in AgNO3 is
mixed with a 230.0 −mL sample of a solution that is 0.12 M in NaCN.
After the solution reaches equilibrium, what concentration of
Ag+(aq) remains? Answer in M Express your answer using two
significant figures. PS: the answer is not 2.9*10^{-20}
A 125.0 −mL sample of a solution that is 3.0×10^−3 M in AgNO3 is mixed with...
A 125.0 −mL sample of a solution that is 3.0×10^−3 M in AgNO3 is
mixed with a 230.0 −mL sample of a solution that is 0.12 M in
NaCN.
After the solution reaches equilibrium, what concentration of
Ag+(aq) remains?
A 125.0 −mL sample of a solution that is 3.0×10−3 M in AgNO3 is mixed with...
A 125.0 −mL sample of a solution that is 3.0×10−3 M in AgNO3 is
mixed with a 230.0 −mL sample of a solution that is 0.12 M in NaCN.
After the solution reaches equilibrium, what concentration of
Ag+(aq) remains?
Express your answer using two significant figures.
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