Final answer:
Calculating the molarity of an MnSO4 stock solution from the volume and molarity of standard EDTA used in a titration involves determining the moles of EDTA, using stoichiometry to find the moles of MnSO4, and then calculating the stock solution's molarity. The standard deviation requires more data points and statistical analysis.
Step-by-step explanation:
To calculate the molarity and standard deviation of an original MnSO4 stock solution from the molarity and volume of standard EDTA used in a titration, a step-by-step approach is taken. First, determine the moles of EDTA used by multiplying its molarity by the volume in liters. Then, find the moles of MnSO4 that reacted with EDTA using the stoichiometry of the titration reaction. Finally, calculate the molarity of the MnSO4 solution by dividing the moles of MnSO4 by its original volume in liters. As for standard deviation, usually additional data points would be necessary, and statistical formulas would be applied.
The detailed calculations would depend on the balanced chemical equation for the reaction and the concentration of the stock MnSO4 solution. If the concentration of the EDTA is known and the volume used in the titration is measured, one can apply the concepts of molarity directly to these titration calculations. The molarity of the stock solution is determined by the stoichiometry of the reaction, given that EDTA typically reacts in a 1:1 mole ratio with the metal ions in the MnSO4.