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13 Dec 2019

45mL of 3.67M of Ag(NO3) is titrated with 8.83M NaCl to form AgCl(s). What are pAg+ and pCl- when 23mL of 8.83M NaCl is added, and at the equivalence point?

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17 Dec 2019
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Related questions

What are the [I- ], [Ag+ ] and pAg+ values after the equivalence point, when the total added titrant volume is 65 mL?

Part A: First determinethe volume ofAgNO3 at your equivalence point by usingyour Kspexpression. Then calculate a precipitation titration curveplottingpAg+(aq) against volume of AgNO3added for atitration involving adding 0.1015 M AgNO3 toa 50.00 mLsolution of 0.0511 M NaCl. Use a volume range of1.00 to 40.00 mLfor AgNO3. Start at 1.00 mL, with2.00 mL volumes ofAgNO3. As you near theequivalence point, (1.00 mL) oneach side of the equivalence point,narrow the volumes ofAgNO3 to 0.25 mL and then 0.10mL. After the equivalencepoint + 1.00 mL, return to 2.00 mLvolumes of AgNO3 tocomplete yourtitration.

AgNO3(aq)+ NaCl(aq) ------- AgCl(s) +Na+(aq) +NO3-(aq)

AgCl(s)? Ag+(aq)+Cl-(aq) Ksp= [Ag+(aq)][Cl-(aq)] = 1.82x10-10

PointA – Calculateprecipitation of Ag+ used beforethe equivalence point, using ¼ ofthe total volumeof

AgNO3added.

PointB – CalculatepAg+ at the equivalence point, usingyour Ksp.

PointC – CalculatepAg+ after the equivalence point,using ¾ of the total volume ofAgNO3

added.

Consider the titration of 25.00 mL of 0.08230 M KI with 0.05110 MAgNO3. 39.00mL of AgNO3is added. Ksp, AgI(s) = 8.3*10-17


What is the pAG at equivalence point ?


calculate the concentration of Ag+ion after 45.00 mL of Ag+solution was added.

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