Question
In: Chemistry
A mixture of 107.0 mL of 0.0866 M AgNO3 is mixed with 0.0377 M K2CO3. What...
A mixture of 107.0 mL of 0.0866 M AgNO3 is mixed with 0.0377 M K2CO3. What volume (in mL) of K2CO3 needs to be added to precipitate all of the silver ions as Ag2CO3?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
1) 20.0 mL of 0.01 M AgNO3 and 30.0 mL of 0.010 M K2CrO4 are mixed...
1) 20.0 mL of 0.01 M AgNO3 and 30.0 mL of 0.010 M K2CrO4 are
mixed together and allowed to react. Will a precipitate form? What
will be the molarities of the silver ion and chromate ion at
equilibrium?
2) Tooth enamel is composed of hydroxyapatite, whose simplest
formula is Ca5(PO4)3OH and whose corresponding Ksp = 6.8 x 10^-27.
As discussed, fluoride in fluorinated water or in toothpaste reacts
with the hydroxyapatite to form fluoroapatite, Ca5(PO4)3F whose Ksp
= 1.0...
50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of 0.050 M NaCl. Calculate...
50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of
0.050 M NaCl. Calculate the concentration of Ag + and Cl- in the
resulting solution, assuming the volumes are additive.
Ksp(AgCl) = 1.82*10-10
50 mL of 0.060 M K2CrO4 is mixed with 50 mL of 0.080 M AgNO3. Calculate...
50 mL of 0.060 M K2CrO4 is mixed with 50
mL of 0.080 M AgNO3. Calculate the following:
a. The solubility of Ag2CrO4
(Ksp = 1.9 X 10-12) in the solution in moles
per liter.
b. The concentrations of the following ions Ag+,
CrO4-2, K+, and
NO3-.
50 mL of 0.060 M K2CrO4 is mixed with 50 mL of 0.080 M AgNO3. Calculate...
50 mL of 0.060 M K2CrO4 is mixed with 50
mL of 0.080 M AgNO3. Calculate the following:
a. The solubility of Ag2CrO4
(Ksp = 1.9 X 10-12) in the solution in moles
per liter.
b. The concentrations of the following ions Ag+,
CrO4-2, K+, and
NO3-.
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.
A 115.0 −mL sample of a solution that is 2.6×10−3 M in AgNO3 is mixed with...
A 115.0 −mL sample of a solution that is 2.6×10−3 M
in AgNO3 is mixed with a 230.0 −mL sample of a solution that is
0.10 M in NaCN.
After the solution reaches equilibrium, what concentration of
Ag+(aq) remains?
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