Question
In: Chemistry
Suppose that a 10-mL sample of a solution is to be tested for I− ion by...
Suppose that a 10-mL sample of a solution is to be tested for I− ion by addition of 1 drop (0.2 mL) of 0.10 M Pb(NO3)2.
What is the minimum number of grams of I− that must be present in order for PbI2(s) (Ksp=8.49×10−9) to form?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Suppose that a 10-mL sample of a solution is to be tested for I− ion by...
Suppose that a 10-mL sample of a solution is to be tested for I−
ion by addition of 1 drop (0.2 mL) of 0.14 M Pb(NO3)2. What is the
minimum number of grams of I− that must be present in order for
PbI2(s) (Ksp=8.49×10−9) to form?
The tetraborate ion present in a 5.00 mL sample of a saturated borax solution is titrated...
The tetraborate ion present in a 5.00 mL sample of a saturated
borax solution is titrated with 4.78 mL of 0.209 M HCl. Express all
calculations with the correct units and number of significant
figures.
a. How many moles of
B4O5(OH)42- are present
in the sample?
b. What is the molar concentration of
B4O5(OH)42- in the
sample?
c. What is the Ksp of the dissolution of borax at
this temperature?
10 mL sample solution that contains arsenic each is filled into 5 100 mL-volumetric flasks. Then...
10 mL sample solution that contains arsenic each is filled into
5 100 mL-volumetric flasks. Then into the second volumetric flask
until the fifth volumetric flask each added 5, 10, 15, and 20 mL
standard solution 22.1 ppm of arsenic. Then water is added to all
volumetric flasks until the volume reached the 100 mL mark. Then
the absorbance of each solution is measured, with the data below.
Calculate the content of As in sample.
Standard (mL)
Absorbance
0.00
0.156...
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?
A 130.0 −mL sample of a solution that is 3.0×10−3 M in AgNO3 is mixed with...
A 130.0 −mL sample of a solution that is 3.0×10−3 M in AgNO3 is
mixed with a 225.0 −mL sample of a solution that is 0.12 M in NaCN.
After the solution reaches equilibrium, what concentration of
Ag+(aq) remains?
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