100 mL of mineral water containing Mg2+ and Ca2+ is taken and titrated with 86.65 mL of 0.06120 M EDTA. NH4F was added to the second 100 mL portion taken from the mineral water to mask the magnesium in the sample as MgF2, and when this sample was titrated with the same EDTA solution, 38.56 mL was spent. Find the concentration of CaCO3 and MgCO3 in the sample in ppm
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- A 30-mL portion of a solution containing Ca2+ and Mg2+ was titrated with 28.19 mL of 0.213 M EDTA at pH 10. Another 30-mL aliquot of the same Ca-Mg mixture was treated with NaOH to make the solution strongly alkaline and precipitate Mg(OH)2. This solution was then titrated with the same EDTA solution. What would be the required EDTA volume (in mL) to reach the endpoint of the second aliquot if it was found that there was 0.061 M of Mg2+ in the sample?a. A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 10 ( with Mg-EDTA pH 10 buffer reagent) and consumed 31 mL. Calculate the Total Hardness of the water sample as mg CaCO3. b. A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 12 and consumed 31 mL. Calculate the Calcium content of the water sample in mg/L.Calculate the PCa vs. EDTA titration curve for 50.0 mL of 0.0060 M Ca2+ being titrated with 0.0150 M EDTA in a solution buffered to a constant pH of 10.00. After the addition of 0.00 mL After the addition of 5.00 mL After the addition of 26.00 mL
- 1 gm of calcium carbonate is dissolved in dilute HCl and diluted to 1 liter with distilled water. 100 ml of this standard hard water requires 90 ml of EDTA solution. 100 ml of unknown hard water requires 36 ml of EDTA solution. 100 ml of same water sample after boiling requires 18 ml of EDTA solution. Calculate Carbonate and Non-carbonate hardness of water sample.0.75 gm of calcium carbonate is dissolved in 1 liter of distilled water. 100 ml of this standard hard water requires 25 ml of EDTA solution. 100 ml of unknown hard water requires 15 ml of EDTA solution. 100 ml of same water sample after boiling requires 10 ml of EDTA solution. Calculate Total, Permanent and Temporary hardness of water sample.Calculate the PCa vs. EDTA titration curve for 50.0 mL of 0.0060 M Ca2+ being titrated with 0.0150 M EDTA in a solution buffered to a constant pH of 10.00. After the addition of 0.00 mL After the addition of 26.0 mL
- You took 25.00 mL of unknown water solution and titrated it with EDTA. The EDTA solution molarity was 0.01 M, and it took 16.50 mL to reach the end point. With the blank it took only 0.98 mL to reach end point. 15.52 mL of EDTA solution were used to titrate hardness that actually came from the unknown 1.552×10−4 moles of EDTA reacted with hardness-causing ions from the unknown sample 1.552×10−4 moles of hardness-causing ions were present in the unknown sample A) Assuming that the total hardness of water is due to CaCO3, how many grams CaCO3 does it correspond to? B) What is the total hardness of the unknown water in ppm CaCO3?A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint.In the titration of 25.00 mL of a water sample, it took 20.690 mL of 4.050x 10−3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures) The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. Calculate the number of grams of CaCO3 present and convert to mg. Calculate the ppm of CaCO3 = mg CaCO3 / Liters H2O used. (enter…
- In order to titrate EDTA into a water sample of unknown water hardness, the EDTA of known concentration is first diluted. If 25.0 mL of a 0.0632 M EDTA solution is transferred into a 250.0 mL volumetric flask, what is the concentration of the diluted EDTA solution? 0.00632 M 0.006320 M 3.950e-4 M 0.01580 M 0.00158 M 3.95e-4 M 0.6320 MPlease answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. A 50.00-mL sample of water containing Ca2+ and Mg2+ is titrated with 10.28 mL of 0.01001 M EDTA in an ammonia buffer at pH 10.00. Another 50.00-mL sample is titrated with NaOH to precipitate Mg(OH)2 and then titrated at pH 13.00 with 6.75 mL of the same EDTA solution. Calculate the concentration of CaCO3 and MgCO3 in the sample in ppm.A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 12 and consumed 31 mL. Calculate the Calcium content of the water sample in mg/L. Ans in 3 sig figures. no need to write the unit.