A student titrated a 25.00 mL sample of water with 0.0200 M EDTA. The titration required 20.40 mL of EDTA. Calculate the ppm hardness in the water sample
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- 50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, what is the amount of magnesium in the sample in ppm?50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, which of the following is the amount of magnesium in the sample in ppm? (Mg:24 g/mol) A. 378 B. 302 C. 214 D. 251In the titration of 25.00 mL of a water sample, it took 20.840 mL of 4.350x 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)
- 50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, what is the value of magnesium in ppm in the sample?(Mg:24 g/mol)A 15.00 mL sample of hard water was titrated with a 0.0150 M EDTA solution. The titration required 26.72 mL of EDTA to reach the end point. What is the total hardness concentration of the water sample in ppm?A 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution. It is determined that 8.54 mL of EDTA is required to reach the end point. The blank titre was determined to be 1.50 mL. Determine the concentration of Calcium in the water sample in ppm. (mwt. of CaCO3 = 100.0892 g/mol).
- 50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, which of the following is the magnesium amount in the sample in ppm? (Mg:24 g/mol)When doing a titration, it is helpful to know approximately the volume of titrant that will be needed. You will be titrating 25.00 mL of a 5.000 x 10-3 M CaCl2 solution with EDTA that is approximately 0.010 M. Calculate the volume of EDTA (in mL) that will be needed to titrate the 25.00 mL of the CaCl2 solution given the approximate molarity of the EDTA.You titrate 50.00 mL of hard water with 14.86 mL of 0.0100 M EDTA solution. How many moles of Ca²+ are present in the sample? What is the hardness in units of mg CaCO, per Liter of solution?
- C1. A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible. What is the MW of calcium carbonate? (use C1 as reference)* 102 g/mol 98 g/mL 100 g/mL 100 g/mol What is the molar concentration of the standardized EDTA solution? (use C1 as reference)* 0.08m 0.8M 0.08N 0.08M How many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?* 0.1825 0.1852 1.825 1.1852The amount of calcium in physiologic fluids can be determined by a complexometric titration with EDTA. In one such analysis, a 0.100-mL sample of blood serum was made basic by adding 2 drops of NaOH and titrated with 0.00528 M EDTA, requiring 0.233 mL to reach the end point. Report the concentration of calcium in the sample as miligrams of Ca per 100 mL. (Ca = 40.078 amu).If 10.00 mL sample of 0.01 M standard Ca2+ solution is titrated with 9.8 mL of EDTA solution, what is the molarity of EDTA? (Ca: 40 g/mol)