3.00 mL of bleach (NaOCl is the active ingredient) is mixed with KI and HCl to completely form triiodide (I, ) ions. The I, ions is titrated with a 0.1306 3. 3 M thiosulfate (S,0, ) solution. The endpoint is reached when 31.52 mL of the thiosulfate solution is added. 3. The moles of sodium thiosulfate used in the reaction is? Select one: а. 0.00389 b. 0.00412 С. 0.00327 O d. 0.00462

3.00 mL of bleach (NaOCl is the active ingredient) is mixed with KI and HCl to completely form triiodide (I, ) ions. The I, ions is titrated with a 0.1306 3. 3 M thiosulfate (S,0, ) solution. The endpoint is reached when 31.52 mL of the thiosulfate solution is added. 3. The moles of sodium thiosulfate used in the reaction is? Select one: а. 0.00389 b. 0.00412 С. 0.00327 O d. 0.00462

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.26QAP

See similar textbooks

Similar questions

A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
6g of impure NaOH were dissolved in water and the solution was completed to become 1L ,if 25ml of this solution were titrated with 18ml of 0.1 sulphuric acid ,the % of sodium hydroxide in the sample equals .... [NaOH=40g/m]
How many liters of pure water willbe required to dissolve the same amount of solid Lead Iodate (0.885g), if the water already intially contains .135M NaIO3?
A 100.0-mL sample of brackish water was made ammoniacal, and the sulfide it contained was titrated with 16.47 mL of 0.02310 M AgNO3. The chemical reaction is 2Ag+ + S2- -> Ag2S (s) Compute for the concentration of H2S in the water in parts per million, ppm.
A buffer is prepared by mixing 204 mL of 0.452 M HCl and0.500 L of 0.400 M sodium acetate. (a) What is the pH? (b) How many grams of KOH must be addedto 0.500 L of the buffer to change the pH by 0.15 units?
(a) Precipitation of the group 4 cations of Figure requiresa basic medium. Why is this so? (b) What is the mostsignificant difference between the sulfides precipitated ingroup 2 and those precipitated in group 3? (c) Suggest aprocedure that would serve to redissolve the group 3 cationsfollowing their precipitation.
A 250.0-mg sample of an organic weak acid is dissolved in an appropriate solvent and titrated with 0.0556 M NaOH, requiring 32.58 mL to reach the end point. Determine the compound’s equivalent weight.
Calculate the ratio of [Ca2+ ] to [Fe2+ ] in a lake in whichthe water is in equilibrium with deposits of both CaCO3 and FeCO3. Assume that the water is slightly basic andthat the hydrolysis of the carbonate ion can, therefore, beignored.
10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?
The graph below, which is related to a titration curve, shows the fraction (f) of the stoichiometric amount of acetic acid present as non-ionized CH3COOH and as acetate ion, CH3COO-, as a function of the pH of the solution containing these species. (Graph piture attached) Explain the significance of the point at which the two curves cross. What are the fractions and the pH at that point?
750 mL of buffer with pH 4.50 needs to be prepared. Solid sodium acetate (CH3COONa) and glacial acetic acid, which h is 99% by mass acetic acid and has a density of 1.05 g/mL are available to prepare this buffer. If the buffer is to be 0.15 M in acetic acid, determine: The mass in grams of CH3COONa that needs to be added. The volume in mL of glacial acetic acid that must be added.
A buffer of acetic acid and sodium acetate is prepared by mixing 10.0 mL of 0.50 M acetic acid with 0.41 grams of sodium acetate (molar mass = 82.0343 grams/mole). Calculate the concentration of acetic acid and acetate ion in the buffer (total volume of the solution is 100.0 mL). Additionally, the pH of the solution is 4.75. Explain why this is significant.