12-10. Calculate [HY3-][HY3-] in a solution prepared by mixing 10.00 mL10.00 mL of 0.0100 M0.0100 M VOSO4, I VOSO4,9 90 mL9.90 mL of 0.010.0 M0.010 0 M EDTA, and 100 ml.10.0 mL of buffer with a pHpE of 4.00.4.00.
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![12-10. Calculate [HY3-[HY3] in a solution prepared by mixing 10.00 mL10.00 mL of 0.010 0 M0.0100 M VOSO4,
I
VOSO4, 9.90 mL9.90 mL of 0.0100 M0.010 0 M EDTA, and 10.0 mL10.0 mL of buffer with a pHpH of 4.00.4.00.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb5bf4ba0-b032-4556-ac45-0f5d16670fd8%2F6c814bb2-7ca3-4075-8f6a-01f252f0f2ba%2Fz4tciql_processed.jpeg&w=3840&q=75)
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- What is the mass of pure dry CaCO3 (MW: 100.0869 g/mol) standard used in the standardization of EDTA solution? Assume that 1.758 M EDTA solution was computed based on the titration of CaCO3 standard. The volume of titrant needed to reach the endpoint was 35.00 mL. Ca2+ + Y4- → CaY2- 0.1500 g 5.630 g 6.158 g 0.6158 gTitration of 25.00ml of 0.100M I- with 0.0500M Ag+. Calculate pAg+ (=-log[Ag+]) at VAg+= 10.00ml; 49.50ml; 50.00ml; 50.50ml; 52.00ml. (Ksp,Ag+)= 8.3*10^-17Construct a titration curve (pCl^- vs. Vtitrant) for the titration of 25.0 mL of 0.100 M Cl^– solution with 0.100 M AgNO3. MS Excel® can be used. Titrant volumes: 0.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL.AgCl: Ksp = 1.82 x 10^-10
- A 50.0 mL of 3.1% (w/v, g/mL) NaOH solution is mixed with 40.00 mL of 1.2% (w/v, g/mL) Na2CO3 solution. What volume of 0.087 M HCl will be required to titrate the resultant solution to bromocresol green indicator end point (Bcg pH transition range 3.8-5.4, Fwt of NaOH=40 g/mol, Na2CO3= 105.99 g/mol).An EDTA solution prepared from its disodium salt was standardized using 0.250-g primary standard CaCO3 (MW=100.087) and consumed 28.50 mL of the solution. The standard solution was used to determine the hardness of a 2.0 L sample of mineral water, which required 35.57 mL EDTA solution. Express the analysis in terms of ppm CaCO3A 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. Ans in 3 sig figures. no need to write the unit.
- The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 1: Final Buret reading (ml)-19.80; Initial Buret reading (ml)- 13.00; Temperature (Celcius)- 25 Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 1- 6.80ml; Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5.…The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)26. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature…1. How much volume (mL) is needed to standardize 0.05M of EDTA using 180mg of magnesium ribbon? MW: 24g/mol2. How many grams of EDTA is required to prepare 250mL of a 0.05M solution? MW: 292g/mol3. What is the Molarity of the EDTA solution if 35mL of the titrant was added to 0.2g of calcium carbonate? Round off to four decimal places
- 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 MThe potentiometric titration data of 2,422 mmol chloride ion with 0.1000 M AgNO3 are as follows. What should the x and y axis values be to find the turning point using the first derivative curve? AgNO3 volume (mL) Potential (Volts) 5.0 0.062 15.0 0.085 20.0 0.107 22.0 0.123 23.0 0.138 23.50 0.146 23.80 0.161 24.00 0.174 24.10 0.183 24.20 0.194 24.30 0.233Construct a titration curve that is expected to be obtained by titration 50.00mL of 0.1000M Sr2+ with 0.1000M EDTA at pH 11. Kf = 4.3 x 10^8. Use the following volumes to construct the curve: 0.00, 10.00, 30.00, 40.00, 45.00, 50.0, 55.00, 60.00 and 70.00mL.