A 10.00-ml. solution containing cr was treated with excess AgNO to precipitate 0.4368 g AgCl. What was the molarity of CI in the unknown?

0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the evolved gases in a solution of NaOH.  After neutralizing, the sample was treated with 25.74 mL of a 0.264 M AgNO3 solution.  This precipitated the chloride (Cl-) out as AgCl and left an excess of AgNO3.  The excess AgNO3 was titrated with 0.1 M KSCN and required 16.47 mL to reach the endpoint in a Volhard titration. Calculate the % w/w Cl– (35.45 g/mol) in the sample.  Provide your answer to 2 places after the decimal point and without units. Reactions: Cl– + Ag+  →  AgCl(s)                             Reaction 1                   Ag+ + SCN–  →   AgSCN(s)                    Reaction 2 HINT: This is an example of a back-titration.  Steps to success: First, calculate the TOTAL amount (in moles) of Ag+ added from the volume and molarity of the silver nitrate solution. Second, determine the EXCESS amount of Ag+ from the reaction with thiocyanate (Reaction 2 above).  Third, calculate the…

Write the balanced equation for the reaction of aqueous Pb(ClO3)2Pb(ClO3)2 with aqueous NaI.NaI. Include phases. chemical equation:   What mass of precipitate will form if 1.50 L1.50 L of highly concentrated Pb(ClO3)2Pb(ClO3)2 is mixed with 0.500 L 0.300 M NaI0.500 L 0.300 M NaI? Assume the reaction goes to completion.

25.0 mL of a 0.2450 M NH,CI solution is added to 55.5 mL of 0.1655 M FeCl,. What is the concentration of chloride ion in the final solution? Select one: a. 0.607 M b. 0.276 M с. 1.35 М d. 0.418 M e. 0.190 М