Please I need help I’m stock in this part please 4.4.14.24.34.44.54.6Quantitative determination of calcium ion concentration in water samples.Set up a titration apparatus using a 250 mL Erlenmeyer flask with a stir bar, a 50 mL buret containing yourEDTA solution (remember to rinse your buret with a small amount of EDTA solution several times prior tofilling).To the Erlenmeyer flask combine the following: 50 mL of distilled water, 5.0 mL of ammonia buffer, 1.0mL of Mg-EDTA solution and 1-2 drops of Eriochrome Black T (EBT) indicator. Pipette 25.00 mL ofdistilled water as a blank sample to the flask and turn on the stirrer. The solution should be a light pinkcolor.Record the initial volume in the buret and titrate this solution with the EDTA solution you prepared untilthe color changes from light pink to blue (Be aware that the endpoint change from one color to another willbe more subjective than a phenolphthalein acid-base endpoint). Record the final volume in the buret.Remember that the distilled water should not contain an appreciable concentration of calcium ions so thecolor should change after a very small volume of titrant has been added.Repeat 4.2-4.3 for one of the water samples for which you determined the total dissolved solids. (Againtitrating 25.00 mL of the water sample (or other volume if desired) transferred by pipette.) Perform thisdetermination in duplicate trials. If the water sample has a very high calcium ion concentration you mayneed to reduce the volume added in the second trial.Repeat 4.4 for a second water sample (be sure that one of your titrations of the commercial samples iscontained on the list provided by the instructor). You should have data for 5 titrations in all: one fordistilled water and two each for two water samples (one hard and one soft).Calculate the concentration of calcium ion in molarity for each of the titrations performed (note that 1 moleof EDTA complexes one mole of calcium ion). Using the values below rate the water samples tested asbeing soft (S), moderately hard (MH), hard (H), or very hard (VH). Note that distilled water has very littlecalcium ion and the volume of the water sample added via pipette (25.00 mL or less if very hard water) iswhat should be used to calculate the calcium ion molarity.Soft (S): 0.0-6.0 x 104 M, Moderately hard (MH): 0.6-1.2 x 10-³ M,Hard (H): 01.2-1.8 x 10-³ M, or Very hard (VH): exceeds 1.8 x 10-³ M. Change3. Quantitative Determination of Calcium Ion in Water Samples by EDTA Titration(Duplicates of two water samples, one hard and one soft as defined by the instructor.)SampleTrial No.SampleVolumeInitialVolume[4.3]FinalVolume[4.3]NetVolumemoles ofEDTACalcium IonMolarity (M)[4.6]WaterHardness[4.6]Distilled WaterPellegrino225 m415 mu248.blue.Crystal CrystalGersterZS.Pellegrino Geyser3415 mL 25 mL 25 ML48,80 49.50 31,848 m² √2 12.75 14.4 31.8. 14.25

Question

Please I  need help I’m stock in this part please 4.4.14.24.34.44.54.6Quantitative determination of calcium ion concentration in water samples.Set up a titration apparatus using a 250 mL Erlenmeyer flask with a stir bar, a 50 mL buret containing yourEDTA solution (remember to rinse your buret with a small amount of EDTA solution several times prior tofilling).To the Erlenmeyer flask combine the following: 50 mL of distilled water, 5.0 mL of ammonia buffer, 1.0mL of Mg-EDTA solution and 1-2 drops of Eriochrome Black T (EBT) indicator. Pipette 25.00 mL ofdistilled water as a blank sample to the flask and turn on the stirrer. The solution should be a light pinkcolor.Record the initial volume in the buret and titrate this solution with the EDTA solution you prepared untilthe color changes from light pink to blue (Be aware that the endpoint change from one color to another willbe more subjective than a phenolphthalein acid-base endpoint). Record the final volume in the buret.Remember that the distilled water should not contain an appreciable concentration of calcium ions so thecolor should change after a very small volume of titrant has been added.Repeat 4.2-4.3 for one of the water samples for which you determined the total dissolved solids. (Againtitrating 25.00 mL of the water sample (or other volume if desired) transferred by pipette.) Perform thisdetermination in duplicate trials. If the water sample has a very high calcium ion concentration you mayneed to reduce the volume added in the second trial.Repeat 4.4 for a second water sample (be sure that one of your titrations of the commercial samples iscontained on the list provided by the instructor). You should have data for 5 titrations in all: one fordistilled water and two each for two water samples (one hard and one soft).Calculate the concentration of calcium ion in molarity for each of the titrations performed (note that 1 moleof EDTA complexes one mole of calcium ion). Using the values below rate the water samples tested asbeing soft (S), moderately hard (MH), hard (H), or very hard (VH). Note that distilled water has very littlecalcium ion and the volume of the water sample added via pipette (25.00 mL or less if very hard water) iswhat should be used to calculate the calcium ion molarity.Soft (S): 0.0-6.0 x 104 M, Moderately hard (MH): 0.6-1.2 x 10-³ M,Hard (H): 01.2-1.8 x 10-³ M, or Very hard (VH): exceeds 1.8 x 10-³ M. Change3. Quantitative Determination of Calcium Ion in Water Samples by EDTA Titration(Duplicates of two water samples, one hard and one soft as defined by the instructor.)SampleTrial No.SampleVolumeInitialVolume[4.3]FinalVolume[4.3]NetVolumemoles ofEDTACalcium IonMolarity (M)[4.6]WaterHardness[4.6]Distilled WaterPellegrino225 m415 mu248.blue.Crystal CrystalGersterZS.Pellegrino Geyser3415 mL 25 mL 25 ML48,80 49.50 31,848 m² √2 12.75 14.4 31.8. 14.25

Accepted Answer

Net volume = Final volume - Initial volume 
For example, trial 1: 
Net volume = 50 ml - 48 ml = 2…

Net Volume moles of EDTA Calcium Ion Molarity (M) [4.61 Water Hardness [4.6]