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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

1) Determine the solubility product constant (Ksp) of borax, a slightly soluble sodium salt, in water at two different temperatures and evaluate the enthalpy, entropy and Gibbs free energy change for dissolving borax in water. Materials and reagents: Borax (Na2B4O5(OH)4· 10H2O) Na2CO3 0.1 M HCl solution Bromocresol green indicator Bromothymol blue indicator 500 ml Erlenmeyer flasks (10 per student) Beakers (2 per student) Magnetic stirrer and bar (1 per student) Distilled water Ice-water bath Thermometer (1 per student) 50 ml burette (1 per student) Procedure: Preparation of the Borax-Borate Equilibrium Mixtures: These solutions will be prepared beforehand. Take about 60 mL of each solution. Make sure each student performs at least one titration. To two separate 500mL Erlenmeyer flasks containing magnetic stirring bars add about 20g of borax and 400mL of distilled water. Designate one flask as the room temperature system and one as the ice-water system. Stir the room…
Can solid Mg(OH)2 precipitate when 20.0 mL of 2.4 x 10-4 M of MgCl2 solution is mixed with 10.0 mL of 3.6 x 10-4 M of NaOH solution? Ksp of Mg(OH)2 = 7.2 x 10-12
Two homogeneous solutions 1.5 x 10-2 M Pb(NO3)2 and 2.5 x 10-4 M (NH4)2SO4 are combined. Does PbSO4 (s) (Ksp = 1.8 x 10-7) precipitate from the solution? Please explain so I can understand- thank you!
The apparent solubility products of AgCN and PbF2 at 25°C are 6.0x10-1/ and 3.3×10¬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.) 4.0 solubility of A9CN g/100. g of solution solubility of PBF2 4.0 g/100. g of solution
Calculate the solubility of KHC₂O4 in moles per liter given that Ksp = 3.72 x 10². (The dissolution products are K + HC₂O4)
The solubility product (Kgp) for MnCO3 in pure water at 25 °C is 1.8 x 1011. Calculate the molar solubility of MnCO3. O4.2 x 10-6 M 3.2 x 10-22 M 9.0 x 10-12 M O 4.5 x 10-12 M 1.8 x 10-11 M
The solubility of Ag₂ CrO4 in water at 25 °C is measured to be 0.022 L Round your answer to 2 significant digits. 0 x10 × Ś I Use this information to calculate Kp for Ag₂ CrO4. sp
One gram of sodium hydroxide (NaOH) is used to adjust the pH of an aqueous solution (200 gallons) thatcontains 10 lbs of finely ground rhodochrosite (MnCO3) ore. Does the NaOH raise or lower the solutionpH? What is the amount of NaOH added in lbs/ton? What is the molarity (mol/l) of the system? Assumingthe NaOH is completely soluble and the system is at room temperature, what is the solid-to-liquid ratio(wt%) of the system?
Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Moles of OCl– in the diluted bleach titrated. ?
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca² +(aq) and 0.0210 M Ag+ (aq). What will be the concentration of Ca² +(aq) when Ag₂SO4(s) begins to precipitate? Solubility-product constants, K₁p, can be found in the chempendix. [Ca²+] = What percentage of the Ca² +(aq) can be precipitated from the Ag+ (aq) by selective precipitation? percentage: M %
Calculate the solubility of zinc (II) hydroxide in a solution maintained at (i) pH= 5.3(ii) pH= 8.2. Ksp = 2.0 x 10-17
A sample containing calcium was analyzed by gravimetry, converting all calcium to calcium oxalate monohydrate (CaC2O4 • H2O). The sample weighing 0.2654 g was dissolved by adding 6M HCl, and then ammonium oxalate solution was added to precipitate all the calcium. The precipitate was suction filtered and dried in an oven at 95 °C for one hour. The solid obtained weighed 0.3216 grams.Calculate:A) The percentage of CaCO3B) The percentage of Ca C) The percentage of CaO