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Author Question: The concentration of an aqueous solution of NaOCl can be determined by a redox titration with iodide ... (Read 135 times)

genevieve1028

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Question 1

Assume that an aqueous solution of hydroxide ion, OH-, represented by unshaded spheres, is allowed to mix with a solution of an acid, HnA, represented by gray spheres. Three possible outcomes are represented by boxes (a)-(c), where the black spheres represent An-, the anion of the acid. For clarity H2O molecules are not shown.




Which outcome corresponds to the reaction:
H3AsO4 + 3 OH- → 3 H2O + AsO43-?
◦ box (a)
◦ box (b)
◦ box (c)
◦ None of these

Question 2




The concentration of an aqueous solution of NaOCl can be determined by a redox titration with iodide ion in acidic solution:

OCl- (aq) + 2 I- (aq) + 2 H⁺ (aq) → Cl⁻ (aq) + I2 (aq) + H2O (l)


Assume that the black spheres in the buret represent I⁻ ions, the gray spheres in the flask represent OCl⁻ ions, the concentration of the I⁻ ions in the buret is 0.120 M, and the volumes in the buret and the flask are identical. What is the concentration of the NaOCl in the flask, and what fraction of the I⁻ solution in the buret must be added to the flask to react with all the OCl⁻ ions?
◦ 0.0600 M NaOCl; 2/3 of the I⁻ must be added.
◦ 0.0600 M NaOCl; 1/3 of the I⁻ must be added.
◦ 0.0400 M NaOCl; 2/3 of the I⁻ must be added.
◦ 0.0400 M NaOCl; 1/3 of the I⁻ must be added.


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Marked as best answer by genevieve1028 on Feb 15, 2020

bblaney

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genevieve1028

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Reply 2 on: Feb 15, 2020
Gracias!


tandmlomax84

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Reply 3 on: Yesterday
Great answer, keep it coming :)

 

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