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.
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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...
Suppose you need to standardize a sodium thiosulfate solution for a titration experiment. To do so,...
Suppose you need to standardize a sodium thiosulfate solution for a titration experiment. To do so, you will react it with a solution of iodine. You add a 1.00 mL aliquot of 0.0200 M KIO3 solution to a flask, followed by 3 mL of distilled water, 0.2 g of solid KI, and 1 mL H2SO4. You then titrate the solution with sodium thiosulfate solution in order to determine the exact concentration of Na2S2O3. The end point of the titration is...
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 solution of sodium thiosulfate, Na2S2O3, is 0.7707 M. 7.42 mL of this solution reacts with...
A solution of sodium thiosulfate, Na2S2O3, is 0.7707 M. 7.42 mL of this solution reacts with 24.81 mL of I2 solution. What is the molarity of the I2 solution? 2(Na2S2O3) + I2↔Na2S4O6 + 2(NaI) 20.28 mL of the I2 solution from above is required to titrate a sample containing As2O3. Calculate the mass of As2O3 (197.8 g/mol) in the sample. As2O3 + 5(H2O) + 2I2 → 2(H3AsO4) + 4HI
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:
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:
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