A 40.0-mL solution of 0.040 0 M Hg 2 (NO 3 ) 2 was titrated with 60.0

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A 40.0-mL solution of 0.040 0 M Hg₂(NO₃)₂ was titrated with 60.0 mL of 0.100 M KI to precipitate Hg₂I₂ (K_sp = 4.6 × 10^-29).

(a) Show that 32.0 mL of KI are needed to reach the equivalence point.

(b) When 60.0 mL of KI have been added, virtually all Hg₂²⁺ has precipitated, along with 3.20 mmol of I^-. Considering all ions remaining in the solution, calculate the ionic strength when 60.0 mL of KI have been added.

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Quantitative Chemical Analysis

ISBN: 9781464135385

9th Edition

Authors: Daniel C. Harris

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Question Posted: Jun 24, 2021 08:50 AM

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A 40.0-mL solution of 0.040 0 M Hg 2 (NO 3 ) 2 was titrated with 60.0

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a 40 mL 004 M Hg 2 NO 3 2 16 mmol of Hg 2 2 ions or 32 mmol of Hg 2 ion Hence 32mL 01M KI s...View the full answer

Quantitative Chemical Analysis

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