If a 100.0 mL aliquot of a 0.05009 M KIO3 solution required 41.15 mL of a...
If a 100.0 mL aliquot of a 0.05009 M KIO3 solution required 41.15 mL of a sodium thiosulfate solution to titrate it, what is the molarity of the sodium thiosulfate solution? Clearly show any required calculations with proper units and significant digits.
Homework Answers
Request Answer!
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Add Answer to:
If a 100.0 mL aliquot of a 0.05009 M KIO3 solution required 41.15 mL of a...
A water supply was known to contain lead (II) ions. A 100.0 mL aliquot of the...
A water supply was known to contain lead (II) ions. A 100.0 mL
aliquot of the solution was pipetted, and its mass determined to be
100.53 g. The 100.0 mL aliquot was acidified, and 21.25 mL of a
0.01235 M potassium dichromate solution were required to oxidize
all of the lead (II) ions. Calculate (1) the molarity of the lead
(II) ions in the solution, and (2) the mass percent of the lead
(II) ions in the solution.
3. A...
A 10.00 ml sample of .0.0100 M KIO3 was titrated against a solution of sodium thiosulfate...
A 10.00 ml sample of .0.0100 M KIO3 was titrated against a solution of sodium thiosulfate to standardize it. The initial buret volume reading was 0.07 ml. The final buret reading was 6.54 ml. Calculate the [Na2S2O3].
3. A water supply was known to contain lead (II) ions. A 100.0 mL aliquot of...
3. A water supply was known to contain lead (II) ions. A 100.0 mL aliquot of the solution was pipetted. and its mass determined to be 100.53 g. The 100.0 mL aliquot was acidified, and 21.25 mL of a 0.01235 M potassium dichromate solution were required to oxidize all of the lead (I) ions, Calculate (1) the molarity of the lead (II) ions in the solution, and (2) the mass percent of the lead (II) ions in the solution.
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a...
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a standard solution containing 0.01500 M Ca2+ required 42.87 mL of EDTA to reach the endpoint. The molarity of the EDTA solution is: ________ M b) That same EDTA solution was then used to titrate an unknown hard water sample. A 40.00 mL aliquot of unknown hard water required 34.21 mL of EDTA solution to reach a distinct endpoint. The concentration of Ca2+ ions (assuming...
A 25-mL aliquot of a 0.0104 M KIO, solution is titrated to the end point with 17.27 mL of a sodium thiosulfate, Na,...
A 25-mL aliquot of a 0.0104 M KIO, solution is titrated to the end point with 17.27 mL of a sodium thiosulfate, Na,S,O3 , solution using a starch-iodide indicator. What is the molar concentration of the Na,S,O, solution?
balance: KIO3(aq) + KI(aq) + H2SO4(aq) -----> I2(aq) + K2SO4(aq) I2(aq) + Na2S2O3(aq) ------> NaI(aq) + Na2S4O6(aq) &nb
balance: KIO3(aq) + KI(aq) + H2SO4(aq) -----> I2(aq) + K2SO4(aq) I2(aq) + Na2S2O3(aq) ------> NaI(aq) + Na2S4O6(aq) Assume that 1.1 mL of the above potassium iodate solution is measured and that 2.20 mL of the unstandardized sodium thiosulfate is required to reach the endpoint. What is the molarity (M), now standardized, sodium thiosulfate?
A 15 ml aliquot of 1.00 M phosphoric acid is titrated with sodium hydroxide using phenolphthalein...
A 15 ml aliquot of 1.00 M phosphoric acid is titrated with sodium hydroxide using phenolphthalein as an indicator. If it takes 20.00 ml of sodium hydroxide to reach the endpoint, what is the molarity of the sodium hydroxide? Answer with appropriate significant digits. H3PO4 (aq) + NaOH (aq) --> H2O (l) + Na3PO4
A 24.34 mL aliquot of a Pb2 solution, containing excess Pb2+, was added to 11.50 mL...
A 24.34 mL aliquot of a Pb2 solution, containing excess Pb2+, was added to 11.50 mL of a 2,3-dimercapto-1-propanol (BAL) solution of unknown concentration, forming the 1:1 Pb2+-BAL complex. The excess Pb2+ was titrated with 0.0157 M EDTA, requiring 9.88 mL to reach the equivalence point. Separately, 39.89 mL of the EDTA solution was required to titrate 32.75 mL of the Pb2+ solution. Calculate the BAL concentration, in molarity, of the original 11.50 mL solution concentration:
In a titration, 41.00 mL of 0.200 M thiosulfate solution was used to titrate 35.00 mL...
In a titration, 41.00 mL of 0.200 M thiosulfate solution was used to titrate 35.00 mL of iodine solution in CH2CI2. What is the molarity of the iodine solution? 5.
If 27.7 mL of the barium hydroxide solution was needed to neutralize a 7.44 mL aliquot...
If 27.7 mL of the barium hydroxide solution was needed to
neutralize a 7.44 mL aliquot of the perchloric acid solution, what
is the concentration of the acid?
Question 63 of 65 > Attempt 1 A barium hydroxide solution is prepared by dissolving 2.97 g of Ba(OH), in water to make 73.4 mL of solution. What is the concentration of the solution in units of molarity? concentration: 0.24 M The barium hydroxide solution is used to titrate a perchloric acid...
A water supply was known to contain lead (II) ions. A 100.0 mL
aliquot of the solution was pipetted, and its mass determined to be
100.53 g. The 100.0 mL aliquot was acidified, and 21.25 mL of a
0.01235 M potassium dichromate solution were required to oxidize
all of the lead (II) ions. Calculate (1) the molarity of the lead
(II) ions in the solution, and (2) the mass percent of the lead
(II) ions in the solution.
3. A...
3. A water supply was known to contain lead (II) ions. A 100.0 mL aliquot of the solution was pipetted. and its mass determined to be 100.53 g. The 100.0 mL aliquot was acidified, and 21.25 mL of a 0.01235 M potassium dichromate solution were required to oxidize all of the lead (I) ions, Calculate (1) the molarity of the lead (II) ions in the solution, and (2) the mass percent of the lead (II) ions in the solution.
A 25-mL aliquot of a 0.0104 M KIO, solution is titrated to the end point with 17.27 mL of a sodium thiosulfate, Na,S,O3 , solution using a starch-iodide indicator. What is the molar concentration of the Na,S,O, solution?
A 24.34 mL aliquot of a Pb2 solution, containing excess Pb2+, was added to 11.50 mL of a 2,3-dimercapto-1-propanol (BAL) solution of unknown concentration, forming the 1:1 Pb2+-BAL complex. The excess Pb2+ was titrated with 0.0157 M EDTA, requiring 9.88 mL to reach the equivalence point. Separately, 39.89 mL of the EDTA solution was required to titrate 32.75 mL of the Pb2+ solution. Calculate the BAL concentration, in molarity, of the original 11.50 mL solution concentration:
In a titration, 41.00 mL of 0.200 M thiosulfate solution was used to titrate 35.00 mL of iodine solution in CH2CI2. What is the molarity of the iodine solution? 5.
If 27.7 mL of the barium hydroxide solution was needed to
neutralize a 7.44 mL aliquot of the perchloric acid solution, what
is the concentration of the acid?
Question 63 of 65 > Attempt 1 A barium hydroxide solution is prepared by dissolving 2.97 g of Ba(OH), in water to make 73.4 mL of solution. What is the concentration of the solution in units of molarity? concentration: 0.24 M The barium hydroxide solution is used to titrate a perchloric acid...
Most questions answered within 3 hours.
-
The manufacturers of Oriental Spice Sauce are concerned that the
sodium levels in their product vary...
asked 32 minutes ago -
PLEASE DON'T ANSWER IF YOU CAN'T ANSWER ALL OF THE QUESTIONS. I
DESPERATELY NEED HELP
Consider...
asked 38 minutes ago -
DO NOT ANSWER IF YOU ARE UNSKILLED IN THIS AREA! TYPE OR WRITE
EACH ANSWER CLEARLY!!...
asked 33 minutes ago -
how many moles of sodium are there in 3.41 moles of the
following compounds
NaCl
Na2SO4...
asked 34 minutes ago -
1.1: Draw a position vs. time graph for a sprinter
running a 100 m dash. Label...
asked 33 minutes ago -
A uniform electric field exists in a region between two
oppositely charged plates. An electron is...
asked 41 minutes ago -
The energy levels of a quantum mechanical system are given by
the equation: En = -hfo/√n^2+9....
asked 1 hour ago -
Calculate the molality of an aqueous solution of iron (II)
nitrate with a solute mole fraction...
asked 1 hour ago -
Use the adjusted trial balance for Stockton Company. Determine
the current asset.
Stockton Company
Adjusted Trial...
asked 1 hour ago -
Mry has net and taxable income of $55000; her claim for
charitable donation is $4000. How...
asked 1 hour ago -
Independent random samples were selected from two binomial
populations, with sample sizes and the number of...
asked 1 hour ago -
Calculate the wavelength of light (in nanometers) emitted from a
hydrogen atom if the electron is...
asked 1 hour ago