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 0.14 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?

Solutions

Expert Solution


Related 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 0.10 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?
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?
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT