Can you check my work please and make sure everything is in the correct significant figures

204 Experiment 24 Standardizing a Basic Solution and Determining this Molar Mass of an Actis see them 3. A 0.5891-g sample of an unknown monoprotic acid required a total of 38.50 ml of 0. 101 1 M NaOf in each titrant for neutralization to a pink phenolphthalein endpoint. The endpoint was initially overshot. so topesek 0.39 ml of 0.0997 M standardized HCI was used for back-titration. and bring lution. a. How many moles of OH were added? How many moles of H* from HCI? ase bure 38, 50 ML / IL lee bure 1 10 00 md = 0.03850 L Add at 0 . 39 mc / 12 I IODOML ) = 0 . 00639 L solution se the ce or cup, are m moles of OH- = M Naolt X UNaOH trant 0: 1011 mol Naolt X 0. 038 50( NaOH = 3. 80335 x 10-3 nal sta for ab moles ps of the s molds of it - - 3.893 x 16-3 = MHCI X VHCI moles 250- moles of it = 0. 099 7 mollHel X 0- 0 0039 4= 3:888 3 X 10-5 moles Itit on - 3. 888 x 16-5 moles 3 . 893 X 16 moles of OH- 3. 888 X / moles of H* b. How many moles of H were in the solid acid? (Use Equation 6.) moles of it in solid acid = moles of OH- in Naolt titrant - moles of it in standarized Hel 3- 893 X 16- moles OH 3. 888 X 10 -5 moles #t = 0- 063 85412 moles ~ 0. 00 3854 2 3. 85 X 10-3 3. 85 4x / ( 10 - 3 moles of H* in solid What is the molar mass of the unknown acid? (Use Equation 5.) MM - Grams of ACIC moles of HF Ion furnished 152.8 -g/mol AM = 0 . 589 1 9 = 152. 8 54 / 775 g1mol 3 . 85 4 X 10-3 mol 2 152, 89 1 mo)