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A 1x working solution contains 50mM of EDTA. What is the EDTA concentration in your 91x concentrated stock solution? Round your result to 2 decimal points.
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- A water sample was analyzed for Fe content using the iron- phenanthroline method. The following data were obtained from the analysis: Reagent Blank Absorbance Absorbance (au) Reagent Blank Absorbance 0.003 Concentration of Stock Solution: 10 ppm Volume of Stock Solution (mL) Total Volume of Standard Solution Concentration of Standard Solution (ppm) Absorbance (au) (mL) 0.50 10.00 0.012 1.00 10.00 0.132 2.00 10.00 0.267 3.00 10.00 0.349 4.00 10.00 0.428 5.00 10.00 0.560 Volume of Unknown Solution Total Volume of Unknown Solution Trial Absorbance (au) (mL) (mL) 1 5.00 10.00 0.289 2 5.00 10.00 0.296 3 5.00 10.00 0.281 Determine the value of the slope (m), y-intercept (b), and the coefficient of determination (r²) A m = 0.1128; b = -4.0 x 10-5; r2 = 0.9880 B m = 0.1128; b = -4.0 x 10-5; r² = 0.9762 C) m = 0.1128; b = -3.0 x 10-³; r² = 0.9880 D m = 0.1128; b = -3.0 x 10-³; r² = 0.9762Table 2: Absorbance Values of Standards and Unknowns. Sample Blank Standard Solution 1 Standard Solution 2 Standard Solution 3 Standard Solution 4 Standard Solution 5 Water Sample 1 Water Sample 2 Phosphate Concentration (in ppm) Y17 0 ppm 0.02 ppm 0.04 ppm 0.08 ppm 0.16 ppm 0.32 ppm Freeman Lake 0.001 0.325 0.292 0.413 0.315 0.039 0.054 0.049 Absorbance at 2= 690 nm Calculations: 1. Construct a phosphate standard curve in Excel by plotting concentration (in ppm) on your x-axis and Absorbance (unitless) on your y-axis for your known solutions. Label the axes on the graph and provide the curve with a title. Use a linear trendline to generate a best fit line to your data. Label the graph with the equation and the R" value. Insert your labeled graph in the space below. XC1. 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 1.1852
- A solution of FESCN2+ has a concentration of 1.00 x 10-2M and an absorbance of 0.755. What is the concentration of an FESCN2+ solution with an absorbance of 0.373? Enter your answer in scientific notation, with one decimal place, as follows: 2.3e-4 or 2.3E-4 Do not include units and note that 10 and x are NOT USED in this type of scientific notation.A water sample was analyzed for iron content using the iron-phenanthroline method. Using the set of data from Question 15 (as presented below), Reagent Blank Absorbance Absorbance (au) Reagent Blank Absorbance 0.003 Concentration of Stock Solution: 10 ppm Volume of Stock Solution (mL) Total Volume of Standard Solution (mL) 0.50 10.00 1.00 10.00 2.00 10.00 3.00 10.00 4.00 10.00 5.00 10.00 Volume of Trial Unknown Solution (mL) 1 5.00 2 5.00 3 5.00 find the true concentration of Fe2+ of the original sample. A) 5.12 ppm B) 2.56 ppm 2.52 ppm D) 5.05 ppm Concentration of Standard Solution (ppm) Total Volume of Unknown Solution (mL) 10.00 10.00 10.00 Absorbance (au) 0.012 0.132 0.267 0.349 0.428 0.560 Absorbance (au) 0.289 0.296 0.281Standardization of EDTA was done using MgSO4 standard wherein a 50-mL aliquot of solution obtained from 0.480 g MgSO4 in 500 mL needed 39.4 mL of the EDTA solution to reach the endpoint. Determine how many milligrams of CaCO3 will react per mL of this EDTA solution.
- ANSWER ASAP PLEASE The Ca2+ in a 25.00mL of underground powder was titrated with 28.60 mL of 0.01350 M EDTA. Calculate the concentration of Ca2+ in ppm. Round off your final answer to four significant figures.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. A) How many milliliters of EDTA solution were used to titrate hardness that actually came from the unknown? B) How many moles of EDTA reacted with hardness-causing ions from the unknown sample? C) How many moles of hardness-causing ions were present in the unknown sample? D) Assuming that the total hardness of water is due to CaCO3, how many grams CaCO3 does it correspond to? E) What is the total hardness of the unknown water in ppm CaCO3?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?
- 20.0 mL water sample was titrated with 0.0100 M EDTA solution that required 14.50 mL for CaCO3 hardness. The total hardness of the water sample in terms of CaCO3 (MW = 100.1 g/mole) in parts per million is _________? Note: Express final answer using least number of significant figures. 2. If 35.2 mL of EDTA solution is required to reach the endpoint with 0.3120-g of primary standard grade CaCO3 (MW = 100.1 g/mole), the normal concentration of the EDTA (MW = 292.24) solution is _________ N?I PUIRE UVVIS spectrophotometry of water sample containing cobalt (Co) and nickel (Ni) is performed in a lab. In the beginning, blank reading is taken by taking in the cuvette. A Water only Both A and C Water sample having Ni and Co Co and Ni solution0.00599 M EDTA solution is used to titrate 250 mL of solution formed by adding MgSO 4 to water. The volume of EDTA solution required to reach the turning point is 10.10 mL. Find the MgSO4 concentration (M) in the solution? A. 2 x 10-4 M b.6.05 x10-2 M C. 4.84x10-4 M D. 2.42x 10-4 M