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Please check if my second data table is correct. I don't think the molar mass is correct
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- 20.0 mL of 1:1 buffer 5.00 mL of standard NaOH pKa=4.66 [NaOH]=0.1108M pH=5.19please stop rejecting. we pay for this service, so we deserve getting our answer! I do not want to have to put a claim in and report Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10Calculate the silver ion concentration after the addition of 5.00, 15.00,25.00,30.00, 35.00, 39.00,40.00,41.00,45.00, and 50.00mL of 0.05000M AgN03to50.0mL of 0.0400M KBr. Construct a titration curve from these data plotting pAg as a function of titrant volume.
- concentration of I3- : 0.002M d. Titration data: Final volume: 29.05 mL Starting volume: 38.10 mL Delivered volume: 25.15 mL How do you calculate g?Data Table 3: Complexometric Titration of Soft Water 5 ml of water 1ml of buffer Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 77ml 79ml 75ml Volume of EDTA Consumed (mL) .23ml .21ml .25ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L):Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________
- Molarity of titrant (NaOH): 0.4550 M HC2H3O2 (aq) + NaOH (aq) → NaC2H3O2 (aq) + H2O (l) Trial # First Second Third Fourth Initial buret reading 0.15 mL 2.43 mL 1.32 mL 0.58 mL Final buret reading 18.62 mL 20.87 mL 20.03 mL 19.14 mL Volume of titrant used 18.47 mL 18.44 mL 18.71 mL 18.56 mL 4) Calculate the molarity of the acetic acid in the vinegar solution (Show your work). use FW for moles-->grams acetic acid. Molarity acetic acid = _____________ M 5) Calculate the weight % of acetic acid in the vinegar. How does this compare with the % listed on the label (5.00%)? (For this calculation assume that density of vinegar is 1.03 g/mL and of course, show your work). Weight % = ___________ 6) If you didn’t get the same weight % of acetic acid as listed on the vinegar label (5.00 %), what are two things (be specific) that could’ve happened during the experiment that could explain the variation from the expected weight %? To do…Data Table for Weak Acid Vol. of Titrant pH Avg. Vol. ∆pH/∆vol 0 2.881 0.25 0.622575 0.5 3.193 0.75 0.453769 1 3.420 1.25 0.32668 1.5 3.583 1.75 0.251434 2 3.709 2.25 0.20456 2.5 3.811 2.75 0.173202 3 3.897 3.25 0.150977 3.5 3.973 3.75 0.134517 4 4.040 4.25 0.12191 4.5 4.101 4.75 0.112002 5 4.157 5.25 0.104057 5.5 4.209 5.75 0.097586 6 4.258 6.25 0.092253 6.5 4.304 6.75 0.087819 7 4.348 7.25 0.084111 7.5 4.390 7.75 0.081001 8 4.431 8.25 0.078391 8.5 4.470 8.75 0.076209 9 4.508 9.25 0.074397 9.5 4.545 9.75 0.072912 10 4.582 10.25 0.071719 10.5 4.617 10.75 0.070794 11 4.653 11.25 0.070117 11.5 4.688 11.75 0.069675 12 4.723 12.25 0.06946 12.5 4.757 12.75 0.069467 13 4.792 13.25 0.069696 13.5 4.827 13.75 0.070152 14 4.862 14.25 0.070845 14.5 4.897 14.75 0.071787 15 4.933 15.25 0.072999 15.5 4.970 15.75 0.074507 16 5.007 16.25 0.076346 16.5 5.045 16.75 0.078561 17 5.085 17.25 0.081211 17.5 5.125 17.75 0.084372 18…15. A 300.00 mL solution of 0.00165 M A2B5 is added to a 230.00 mL solution of 0.00380 M C2D3. What is pQsp for A2D5?
- Data Table 3: Complexometric Titration of Soft Water 6ml of water used (1ml of buffer and 5ml of soft water) Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 77ml 79ml 75ml Volume of EDTA Consumed (mL) .23ml .21ml .25ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L):What conditions must be followed to perform complexometric titration?In the determination of the water hardness of a river water sample, the pH of the sample was adjusted to 12 instead of 10. Is there a positive error, negative error, no effect, or error could not be determined In terms of the ppm CaCO3 of sample?