In Standardization of NaOH, why can the flasks you put your samples of acid into be wet?
Wet with water? Because the acid creates heat and spits acid back in the chemist's face.
Is this CAN or CAN'T be wet?
If CAN, you must be thinking that it dilutes the acid if the flask is wet. Of course, that's true; however, it dilutes the base by the same amount when you add NaOH to titrate it. A much more sophisticated answer is that adding acid to a flask contains x mols of the acid (molarity x liters = moles). The indicator changes when the MOLES of acid and MOLES of base are equal. Adding water before or during the titration doesn't change the number of moles of either acid or base.
The reason the flasks used to hold the acid samples can be wet in the process of standardizing NaOH is because water does not react with NaOH. By ensuring that the flasks are wet, any residue or solution left in the flask will be diluted when the acid is added, without affecting the accuracy of the titration.
However, it is important to note that the presence of water in the flask should be considered in the calculation of the molarity of NaOH solution. This can be achieved by conducting a blank titration, which involves running a control titration without the presence of acid, and subtracting any water's contribution to the volume of NaOH used.
To summarize, using wet flasks in the standardization of NaOH is permissible because water does not react with NaOH, but it is crucial to account for the volume of water in the flask during the calculations.