How would the calculated molarity of KMNo4 be affected when KMno4 is added to rapidly and too much KMnO4 is added, overshooting the endpoint.

I suppose the question is talking about using a primary standard for standardization of KMnO4.

M = mols/L. If you overshoot the end point that means L is too high so M is too low.

Its just a scenario question.

Thanks

When an excess amount of KMnO4 is added beyond the endpoint, it is referred to as overshooting the endpoint. This can affect the calculated molarity of KMnO4 due to several factors:

1. Dilution: Overshooting the endpoint means adding more KMnO4 than required for the reaction. Consequently, this excess KMnO4 will become part of the solution, causing the volume to increase. The increase in volume results in dilution of the solution, which affects the molarity calculation.

2. Incomplete reaction: Overshooting the endpoint can lead to the formation of excess products in the reaction. The excess MnO4- ions may react with other species in the solution, resulting in side reactions or incomplete reactions. This can affect the accuracy of the titration and the calculated molarity.

3. Titration curve: When plotting the titration curve, overshooting the endpoint will result in a higher volume of KMnO4 needed to reach the endpoint. This will affect the point at which the equivalence point is detected, leading to a shift in the curve. As a result, the calculated molarity will be higher than the actual molarity.

Overall, when overshooting the endpoint occurs, the calculated molarity of KMnO4 is likely to be higher than the actual molarity due to dilution, incomplete reactions, and the impact on the titration curve.

When adding KMnO4 to a solution for titration, the concentration of the KMnO4 solution is typically known, and by calculating the molarity, you can determine the concentration of the analyte (the substance being titrated). However, if KMnO4 is added too rapidly or in excess, overshooting the endpoint, it can affect the accuracy of the molarity calculation. Here's how:

1. Understanding the endpoint: In a titration, the endpoint is the point at which the reaction between the analyte and the titrant is complete. It is usually indicated by a color change or other noticeable change in the solution. For KMnO4 titrations, the endpoint is often signaled by a change from a pink or purple color to colorless.

2. Balancing the equation: To determine the number of moles of KMnO4 required for the titration, you need to balance the chemical equation for the reaction between KMnO4 and the analyte. This equation is important for the stoichiometric calculation.

3. Overshooting the endpoint: If too much KMnO4 is added, it can result in overshooting the endpoint. This means that the reaction has gone beyond completion and consumed more KMnO4 than required to fully react with the analyte. As a result, the volume of KMnO4 used in the calculation will be greater, leading to an overestimated molarity.

4. Affected molarity calculation: The molarity (M) is calculated using the formula M = n/V, where n is the number of moles of solute and V is the volume of the solution in liters. If the volume of KMnO4 used is higher than necessary due to overshooting the endpoint, it will lead to a larger V value in the equation. Thus, the calculated molarity will be higher than the actual value.

To minimize the impact of overshooting the endpoint, it is crucial to add KMnO4 slowly and cautiously, beyond the color change, drop by drop, until a permanent color change is observed. This allows for a more precise measurement of the volume used, leading to more accurate molarity calculations.