EDTA: 0.2 M solution KH2PO4: 0.4 solution Sodium Nitrate MW: 84.9947 g/mol A 150 mL buffer solution of 50 mM of sodium nitrate, 25 mM KH2PO4, 0.05 mM EDTA (acid) is needed. How much of each is needed, also include how much water?
Q: lution. What is the to
A: Concentration of CaCO3 Solution = 0.3834/100 = 3.834 x 10-3 M
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- A 47.6 mL aliquot from a 0.5 L solution that contains 0.45g of MnSO4 (MW is 151 g/mol) required 41.9 mL of an EDTA solution to reach the titration endpoint. What mass of CaCO3 (MW is 100.09 g/mol) will react with 1.58 mL of the EDTA solution?The sulfate in 266.5 mg sample was precipitated as BaSO4 by addition of 27.00 mL of 0.0340 M BaCl2. The precipitate was removed by filtration and the remaining BaCl2 consumed 34.2 mL of 0.0200 M EDTA for titration to the end point. (All 1:1 ratio) Calculate the % SO3 in the sample. (MW of SO3 is 80.06 g/mol)6mL of 125mM EDTA was added to 244mL of water. The resulting solution was added to 219mL of water and the pH was adjusted to 8.0 using 6mL of NaOH. A further 25mL of water was added. What is the concentration of the final solution (in micromolar)? MW of EDTA is 292.24, MW of NaOH is 39.99
- Determine the solubility of KIO4 in water. Volume of saturated KIO4 in conical flask is 25.0 ml,KI is 2g,H2SO4 (3.0M) is 20.0 ml added to KI solution , volume of 0.200 M sodium thiosulphate used for titration is 8.00 ml.and if mean ionic activity co efficient,y+- of KIO4 in the saturated solution is 0.85 ,what is Ksp. .To determine the concentration of an EDTA solution, the following magnesium(II) solution is prepared: metallic magnesium (m(Mg) = 0.5915 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.250 L and is filled to the graduation mark with water. The titration of an aliquot of magnesium(II) solution with a volume of 25.00 ml consumes (11.11 ml; 11.32 ml; 11.24 ml; 11.29 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.A 46.4046.40 mL aliquot from a 0.4850.485 L solution that contains 0.3500.350 g of MnSO4MnSO4 (MW=151.00MW=151.00 g/mol) required 35.235.2 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3CaCO3 ( MW=100.09 MW=100.09 g/mol) will react with 1.691.69 mL of the EDTA solution?
- The concentration of a solution of EDTA was determined by standardizing against a solution of Ca2+ prepared from the primary standard CaCO3. A 0.4302g sample of CaCO3 was transferred to a 60mL volumetric flask, dissolved using a minimum of 6 M HCl solution, and diluted to volume. A 44mL portion of this solution was transferred into a 250-mL Erlenmeyer flask and the pH adjusted by adding 5 mL of a pH 10 NH3-NH4 L buffer containing a small amount of Mg2+ EDTA. After adding calmagite as a visual indicator, the solution was titrated with the EDTA, requiring 632mL to reach the end point. Calculate the molar concentration of the titrantIs this for Average Molarity of EDTA Standard Solution? Then, would it be always the same with average Molarity of EDTA? How about the Ca Titer (mg Ca/mL of EDTA Solution? Show step by step solution.A 10.0-mL aliquot of a standard manganese solution containing 62.5 mg/L of Mn is oxidized to MnO4- and diluted to 50.0 mL in a volumetric flask. The absorbance is measured in a 1.00-cm cell at 525 nm is 0.343. Next, a 850-mg steel sample containing manganese in dissolved in acid and diluted to 250 mL. A 50.0-mL aliquot is treated with KIO4 to oxidize Mn to MnO4- and diluted to 100.0 mL. If the absorbance at 525 nm is 0.468 in a 1.00-cm cell, calculate the weight percent of Mn in the steel.
- For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 4. Why is it necessary to carry out the reduction of iron and then the titration, before going on to the next sample 5. If you look carefully, there are pieces of tin metal on the bottom of the SnCl2 reagent solution. Why is it there?For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 1. What is the purpose of the phosphoric acid in this experiment? Please be specific. 2. How does the Diphenylamine sulfonate indicator work? What chemical reaction causes the color change? How is an indicator chosen in a redox reaction?For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 3. How would you prepare a complete anlaysis procedure using KMnO4 as the oxidant instead of K2CrO7? Include sample and solution preparation, approximate weights of samples and reagents, procedure and chemical reactions. In particular what is the purpose of the Zimmerman Reinhardt Reagent?