A 0.1530 g of pure KIO3 was dissolved in 50 mL distilled water. This was then added with KI and 6N H₂SO4. After allowing the said solution to stand in the dark for 3 minutes, this was then titrated to end point with 31.35 mL sodium thiosulfate solution, with starch as the indicator. What is the normality of the sodium thiosulfate solution? Atomic weights: K = 39.1 I = 126.9 O= 16.0

A 0.1530 g of pure KIO3 was dissolved in 50 mL distilled water. This was then added with KI and 6N H₂SO4. After allowing the said solution to stand in the dark for 3 minutes, this was then titrated to end point with 31.35 mL sodium thiosulfate solution, with starch as the indicator. What is the normality of the sodium thiosulfate solution? Atomic weights: K = 39.1 I = 126.9 O= 16.0

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter18: Chemical Equilibrium

Section: Chapter Questions

Problem 3E

See similar textbooks

Similar questions

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Calculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.
A solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?
A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?
A 2.190 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/mol) and potassium bicarbonate (MM=100.1154 g/mol) is dissolved in distilled water. A volume of 30.74 mL of a 0.778 M HCl standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K2CO3: ? wt% KHCO3: ? wt%
A 2.187 g sample of a solid mixture containing only potassium carbonate (MM = 138.2058 g/mol) and potassium bicarbonate ( MM 100.1154 g/mol) is dissolved in distilled water. A volume of 33.47 mL of a 0.749 M HCI standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K₂CO₂: KHCO,: wt% wt%
Please answer the wrong portion with clear steps and explanations
A 0.5123g sample (molar mass 204.23g/mol) of KHP was dissolved in about 25 mL of distilled water and titrated to the phenolphthalein end point with 28.75 mL of a sodium hydroxide solution. Calculate the molar concentration of the hydroxide solution.
4pts) 2.80g of a mixture of Barium Nitrate, Ba(NO3)2 (MM = 261.35 g/mol) and Potassium Bromide, KBr (MM-119.01 g/mol) was dissolved in 200 mL of hot H₂0. Enough Ammonium Phosphate, (NH4)3PO4 (MM = 149.12 g/mol), was added to the solution to precipitate ALL the Barium as Barium Phosphate, Ba3(PO4)2 (s) (MM = 601.93 g/mol). The precipitate was filtered, dried, and weighed to a constant mass of 1.83 g. Determine the percentage by mass of Potassium Bromide, KBr in the original mixture.
A 1.000g sample of a mixture which contains only NaCl and KCl gave a precipitate of AgCl which weighed 2.000g. What are the percentages of Na and K in the mixture? Molar masses: AgCl = 143.3; KCl = 74.55; NaCl = 58.45; Na = 23.0; K = 39.0 * 3/3
The apparent solubility products of AgCN and PBF2 at 25°C are 6.0x10¬1/ and 3.3x10-8, respectively. Calculate the solubility (g/100. g of solution) of these compounds. (Assume each solution has a density of 0.99705 g·cm-3.) solubility of AgCN 4.0 g/100. g of solution solubility of PbF2 4.0 g/100. g of solution
Chemistry A 2.139 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/mol) and potassium bicarbonate (MM=100.1154 g/mol) is dissolved in distilled water. A volume of 30.57 mL of a 0.752 M HCl standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K2CO3: ? WT% KHCO3: ? WT%.

SEE MORE QUESTIONS

Recommended textbooks for you

Introductory Chemistry: An Active Learning Approa…

Chemistry

ISBN:

9781305079250

Author:

Mark S. Cracolice, Ed Peters

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Introductory Chemistry For Today

Chemistry

ISBN:

9781285644561

Author:

Seager

Publisher:

Cengage

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Introductory Chemistry: An Active Learning Approa…

Chemistry

ISBN:

9781305079250

Author:

Mark S. Cracolice, Ed Peters

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Introductory Chemistry For Today

Chemistry

ISBN:

9781285644561

Author:

Seager

Publisher:

Cengage

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS