Using Volumetric Glassware to Measure, Dilute,and Titrate Acid Solution
1)For each of the following procedural errors, indicate whether the calculated molarity of the HCl solution would be higher or lower than the actual molarity. Briefly explain.
a)The NaOH titrant is obtained in a wet beaker
b)The volumetric flask is filled to above the calibration mark with water when the original HCl solution is diluted.
c)The buret tip is not filled with titrant when the first titration is begun.
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a) If the NaOH titrant is obtained in a wet beaker, the calculated molarity of the HCl solution would be higher than the actual molarity. This is because some water from the wet beaker could dissolve into the NaOH solution, increasing the volume of the solution. As a result, the moles of NaOH present in the solution would be calculated based on a higher volume, leading to an overestimate of the molarity of the HCl solution.
b) If the volumetric flask is filled to above the calibration mark with water when the original HCl solution is diluted, the calculated molarity of the HCl solution would be lower than the actual molarity. This is because diluting the HCl solution with excess water would increase the total volume in the flask. As a result, the initial concentration of HCl would be diluted, leading to a lower molarity than expected.
c) If the buret tip is not filled with titrant when the first titration is begun, the calculated molarity of the HCl solution would be higher than the actual molarity. This is because the initial volume of the titrant would be underestimated due to the empty space in the buret tip. As a result, the moles of titrant reacted with the HCl solution would be calculated based on a smaller volume, leading to an overestimate of the molarity of the HCl solution.