A solution prepared by mixing 60.0 mL of 0.220 M AgNO3 and 60.0 mL of 0.220...

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Chemistry

A solution prepared by mixing 60.0 mL of 0.220 M AgNO3 and 60.0mL of 0.220 M TlNO3 was titrated with 0.440 M NaBr in a cellcontaining a silver indicator electrode and a reference electrodeof constant potential 0.175 V. The reference electrode is attachedto the positive terminal of the potentiometer, and the silverelectrode is attached to the negative terminal. The solubilityconstant of TlBr is Ksp = 3.6 Ã— 10â€“6 and the solubility constant ofAgBr is Ksp = 5.0 Ã— 10â€“13.
(c) Calculate the first and second equivalence points of thetitration.
(d) What is the cell potential when the following volumes of0.440 M NaBr have been added? a. 1.0 ml b. 16.0 ml c. 29.0 ml d.29.9 ml e. 30.3 ml f. 46.0 ml g. 60.0 ml h. 62.0 ml

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3.6 Ratings (298 Votes)

Titration a Equivalence points First equivalence point all of AgBr gets precipitated E 1066 0802 0175 0758 V Second equivalence point all of TlBr gets precipitated E 1066 0342 0175 0528 V d Cell potential when a 1 ml NaBr added moles of AgNO3 022 M x 60 ml 132 mmol moles of NaBr 044 M x 1 ml 044 mmol Excess Ag remain 1276 mmol61 ml 021 M E Eo 00592 logAg 0175 08 00592 log021 See Answer

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