suppose that 0.3562 g of na2c2o4 is dissolved in a 250
mL volumetric flask. if 10...
suppose that 0.3562 g of na2c2o4 is dissolved in a 250
mL volumetric flask. if 10 mL of this solution required 48.36 mL of
kmno4 to reach the endpoint what is the molarity of the
permanganate solution
0.1200 g of potassium dichromate primary standard is dissolved,
quantitatively transferred into a 250-mL volumetric flask and
diluted to volume. 0.3000 g an unknown iron ore sample was
dissolved in hydrochloric acid, treated with stanous chloride and
mercury(II) chloride, quantitatively transferred to a 100-mL
volumetric flask and diluted to volume. 25.00 mL of the unknown
iron(II) solution was pipetted into 500-mL Erlenmyer flask and
titrated with the potassium dichromate solution. 28.00 mL of
potassium dichromate is required to reach the...
A compound with molecular mass = 292.16 g/mol was dissolved in a
5.000 mL volumetric flask. A 1.000 mL aliquot was withdrawn, placed
in a 10.000 mL flask and diluted to volume. The apparent absorbance
of the diluted solution at 340 nm was 0.827 in a 1.000 cm cuvette.
To check for a possible stray light effect, this sample was diluted
by exactly a factor of 2; the apparent absorbance was now 0.421. A
reagent blank showed negligible absorbance. The...
A 2.2222 gram sample containing soda ash is dissolved in a 100
mL volumetric flask. A 24.98 mL aliquot is analyzed and required
45.67 mL of 0.1234 M HCl, before it was boiled, cooled, and
back-titrated with 8.88 mL of 0.0987 M NaOH. What is the percent
Na2CO3?
1.25-g of BaCl2 is placed in a 4.000 L volumetric flask. Then
the volumetric flask is filled with D.I. water to the 4.000 L mark.
All the BaCl2 goes into the solution. Assume the density of the
solution is 1.00 g/mL.
What is the mass/mass (m/m) % and the mass/volume (m/v) of the
solution?
10 mL of bleach with an unknown concentration is added to a
100mL volumetric flask. The solution is then finished with
deionized water. 10 mL of this diluted bleach solution is then
added to an erlenmeyer flask along with 1 scoop of KI, and 5 L of
2M HCl. This solution is then titrated with Na2S2O3 until it is a
pale yellow color, then a starch indicator is added and titration
is completed until the solution is clear. If 43...
Suppose a 250.mL flask is filled with 2.0mol of O2 and 1.6mol of
NO . The following reaction becomes possible: N2g+O2g =2NOg The
equilibrium constant K for this reaction is 0.469 at the
temperature of the flask. Calculate the equilibrium molarity of N2
. Round your answer to one decimal place.
Suppose a 250.mL flask is filled with 0.20mol of N2 and 1.4mol
of O2 . The following reaction becomes possible: N2(g)+O2(g)= 2NO(g
)The equilibrium constant K for this reaction is 4.94 at the
temperature of the flask. Calculate the equilibrium molarity of O2
. Round your answer to two decimal places.
A 10.0 mL sample of liquid bleach is diluted to 100. mL in a
volumetric flask. A 25.0 mL aliquot of this solution is analyzed
using the procedure in this experiment. If 10.4 mL of 0.30 M
Na2S2O3 is needed to reach the equivalence point, what is the
percent by mass NaClO in the bleach? Hint: Percent by mass is grams
of NaClO / mass of bleach. Presume a density for the bleach of 1.00
g/mL.
If 4.90 g of Na2CO3 is dissolved in enough
water to make 250. mL of solution, what is the molar concentration
of the sodium carbonate?
Molar concentration of Na2CO3 =
______M
What are the molar concentrations of the Na+ and
CO32- ions?
Molar concentration of Na+ = ______M
Molar concentration of CO32- =
_______M
Suppose a 250.mL flask is filled with 0.90mol of Br2 , 0.60mol
of BrOCl and 1.9mol of BrCl . The following reaction becomes
possible: Br2(g)+OCl2(g) +BrOCl(g)+BrCl(g) The equilibrium constant
K for this reaction is 0.571 at the temperature of the flask.
Calculate the equilibrium molarity of OCl2 . Round your answer to
two decimal places.