A 0.601 g sample of bleach was treated with an excess of KI. The iodine liberated...
A 0.601 g sample of bleach was treated with an excess of KI. The iodine liberated required 12.34 mL of 0.0692 M Na2S2O3 for titration. What is the percentage of KOCl in the bleach?
And can we use NaI to replace KI in the titration? Why?
Homework Answers
reaction between NaI and NaOCl
no new products are obtained in other words they don't react hence
NaI is not used
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A 0.601 g sample of bleach was treated with an excess of KI. The
iodine liberated...
A 0.601 g sample of bleach was treated with an excess of Kl. The lodine liberated...
A 0.601 g sample of bleach was treated with an excess of Kl. The lodine liberated required 12.34 mL of 0.0692 M Na2S203 for titration What is the percentage of KOCI in the bleach? And can we use Nal to replace Kl in the titration? Why?
Please help me with step by step solution. Thank you. A 0.601 g sample of bleach...
Please help me with step by step solution. Thank
you.
A 0.601 g sample of bleach was treated with an excess of Kl. The iodine liberated required 12.34 mL of 0.0692 M Na2S203 for titration. What is the percentage of KOCI in the bleach? And can we use Nal to replace Kl in the titration? Why? For the toolbar, press ALT+F10 (PC) or ALT+FN+F 10 (Mac).
A 2.50 g sample of a household bleach containing sodium hypochlorite (NaClO) is treated with excess...
A 2.50 g sample of a household bleach containing sodium hypochlorite (NaClO) is treated with excess KI solution. The iodine liberated requires 18.0 mL of 0.0200 M Na2S2O3 solution for complete titration. What is the weight percentage of NaClO in the household bleach? (The redox couples are: ClO-/Cl- ; I2/I- ; S2O32-/ S4O62-) *I need the answer step by step with explaination
2. A 0.1000 g sample of KBrO3 was dissolved in dilute acid and treated with an...
2. A 0.1000 g sample of KBrO3 was dissolved in dilute acid and treated with an excess of KI. BrO3 +91 +6H+ → Brº+ 313 + 3H20 The generated 13. required 11.92 mL of a Na2S2O3 solution to reduce it to 1. Use the above balanced equation and those found in the introduction to determine the molarity of the Na2S2O3 solution. 3. The following data was obtained for an iodometric titration of an ascorbic acid tablet. Mass of tablet: 1.2191...
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g...
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g of sodium hypochlorite present What is the percent of sodium hypochlorite in the bleach sample? Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000157 mol KIO, were titrated with an unknown solution of Na2S2O3 and the endpoint was reached after 14.63 mL What is the concentration of the Na2S2O3 solution, in M? Suppose, in an experiment to determine the...
When doing a titration of a 2.310 g sample of bleach, 11.12 mL of a 0.1117...
When doing a titration of a 2.310 g sample of bleach, 11.12 mL of a 0.1117 M Na2S2O3 solution was used. How many moles of I2 reacted with the Na2S2O3? How many grams of NaOCl must have been present in the solution? (Hint: calculate moles of NaOCl that had to have been present based on the moles of I2 that were found and convert that to grams.) What is the percent by mass of the NaOCl in the bleach
(a) Potassium iodate solution was prepared by dissolving 1.022 g of KIO3 (FM 214.00) in a...
(a) Potassium iodate solution was prepared by dissolving 1.022 g of KIO3 (FM 214.00) in a 500 mL volumetric flask. Then 50.00 mL of the solution was pipetted into a flask and treated with excess KI (2 g) and acid (10 mL of 0.5 M H2SO4). How many millimoles of I3− are created by the reaction? (b) The triiodide from part (a) reacted with 37.54 mL of Na2S2O3 solution. What is the concentration of the Na2S2O3 solution? (c) A 1.223...
a) A 3.071-g portion of a copper(II) salt was dissolved in a 250-mL volumetric flask. A...
a) A 3.071-g portion of a copper(II) salt was dissolved in a 250-mL volumetric flask. A 50.0-mL aliquot was analyzed by adding 1 g of KI and titrating the liberated iodine with 23.80 mL of 0.04684 M Na2S2O3. Find the weight percent of Cu in the salt. b) Should starch indicator be added to this titration at the beginning or just before the end point?
1. A sample contains an unknown amount of tartaric acid, H2C4H4O6. If 0.3888 g of the...
1. A sample contains an unknown amount of tartaric acid, H2C4H4O6. If 0.3888 g of the sample requires 37.74 mL of 0.1000 M NaOH to neutralize the H2C4H4O6 completely, what is the percentage of H2C4H4O6 in the sample? The molar mass of H2C4H4O6 is 150.09 g/mol. The balanced equation for the reaction is: H2C4H4O6 + 2 NaOH → 2 H2O + Na2C4H4O6 2. Sodium thiosulfate, Na2S2O3, is an important reagent for titrations. Its solutions can be standardized by titrating the...
A sample of a new cleaning product, "Joe's Famous Bleach Cleaner," with a mass of 54.0...
A sample of a new cleaning product, "Joe's Famous Bleach Cleaner," with a mass of 54.0 g , was diluted with an acetic acid solution containing excess I−. A small amount of starch indicator solution was then added, turning the solution a deep bluish-purple. The solution was then titrated with 0.180 M sodium thiosulfate, Na2S2O3, containing the ion S2O32−. A volume of 41.0 mL of sodium thiosulfate, the titrant, was needed to turn the solution colorless. What is the percentage...
A 0.601 g sample of bleach was treated with an excess of Kl. The lodine liberated required 12.34 mL of 0.0692 M Na2S203 for titration What is the percentage of KOCI in the bleach? And can we use Nal to replace Kl in the titration? Why?
Please help me with step by step solution. Thank
you.
A 0.601 g sample of bleach was treated with an excess of Kl. The iodine liberated required 12.34 mL of 0.0692 M Na2S203 for titration. What is the percentage of KOCI in the bleach? And can we use Nal to replace Kl in the titration? Why? For the toolbar, press ALT+F10 (PC) or ALT+FN+F 10 (Mac).
2. A 0.1000 g sample of KBrO3 was dissolved in dilute acid and treated with an excess of KI. BrO3 +91 +6H+ → Brº+ 313 + 3H20 The generated 13. required 11.92 mL of a Na2S2O3 solution to reduce it to 1. Use the above balanced equation and those found in the introduction to determine the molarity of the Na2S2O3 solution. 3. The following data was obtained for an iodometric titration of an ascorbic acid tablet. Mass of tablet: 1.2191...
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g of sodium hypochlorite present What is the percent of sodium hypochlorite in the bleach sample? Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000157 mol KIO, were titrated with an unknown solution of Na2S2O3 and the endpoint was reached after 14.63 mL What is the concentration of the Na2S2O3 solution, in M? Suppose, in an experiment to determine the...
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