A student, Jack, in the Analytical Chemistry class, conducted a Mohr Titration t
ID: 486653 • Letter: A
Question
A student, Jack, in the Analytical Chemistry class, conducted a Mohr Titration to determine the content of chloride ions in an unknown solution. First, he standardized the AgNO3 titrant with 0.1424 g dry NaCl dissolved in 25.0 mL DI water, and 26.25 mL of titrant was consumed. Then he used the standardized titrant to determine the concentration of chloride in the solution. 12.63 mL of AgNO3 solution was used to titrate 25.00 mL of solution. Answer the following questions about this titration. Note: use appropriate significant figures in your answer!
A) Calculate the concentration (M) of AgNO3 titrant.
B)Determine the content of chloride in the unknown solution (M).
Explanation / Answer
AgNO3 + NaCl ----------> AgCl + NaNO3
moles of NaCl = mass/Molar mass = 0.1424/58.5= 0.002434
from the reaction , 1 mole of AgNO3 requires 1 mole of NaCl.
moles of AgCl = 0.002434 , Molarity of standardized AgNO3= 0.002434*1000/26.25 M=0.093M
for the second case, M1V1= M2V2
M2= molarity of NaCl = 0.093*12.63/25 =0.047
Molarity of Cl = 0.047 ( since NaCl-----> Na+ + Cl-)
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