1. Calculate the volume in milliliters (mL) of a 6.00 MNaOH solution needed to make 5.00 x 102 mL of a 0.100 M NaOHsolution. (Recall that M = molar = mol/L, and show allyour work).
2. An approximately 0.1 M NaOH solution was standardizedwith KHP by titration to a phenolphthalein endpoint. From thefollowing data, calculate the average molarity of the NaOH. Themolar mass of KHP is 204.22 g/mol.
Trial 1 Trial 2 Mass of weighing paper + KHP 2.1467 g 2.1719 gMass of weighing paper 1.4125 g 1.4136 g Mass of KHP ____________________ Moles of KHP __________ __________ Final buret reading31.80 mL 32.67 mL Initial buret reading` 0.15 mL 0.04 mL Volume ofNaOH (mL) __________ __________ Molarity of NaOH (moles per liter)__________ __________ Average molarity __________
3. Calculate the average molarity, standard deviation(SD), and percent (%) variation of the three titration molaritiesgiven below. Recall: % variation = (SD/mean)*(100%).
Molarity of HCl: 0.3087 M 0.3083 M 0.3092 M
Average Molarity: ___________________ ± _____________ (SD)[UNITS!]
Percent (%) variation: ____________________ %
Is the percent variation less than 1%? _________
