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A limestone sample weighing 400 mg was dissolved in acid treated with excess
sodium oxalate. The solution was made basic and the resulting calcium oxalate
was filtered, washed and redissolved in dilute acid. This solution required 14.0
mL of 0.00865 M KMnO4. What is the % Ca of the limestone.
CaC2O4(s) + 2H+ ⇌ Ca2+ + H2C2O4
5H2C2O4 + 2MnO4- + 6H+ ⇌ 10CO2 + 8H2O + Mn2+
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- A saturated solution of magenusium hydroxide is prepared and the excess solid magneusium hydroxide is settled. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, 2 dropfs of indicator are added. A 0.00053 M HCL solution is dispensed from a buret into the solution. The soution changes color after the addition of 13.2 mL. How many moles of hydroxide ion are neutralized in the analysis?A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the molar solubility of magnesium hydroxide?A 10.0 mL aliquot of H2 SO4 solution was diluted to 100.0 mL. Then 25.0 mL aliquot of the diluted H2 SO4 solution was titrated with 30.0 mL of 0.200 M NaOH solution using phenolphthalein as indicator. What is the molar concentration of the original H2 SO4 solution?
- A metal M forms a water-soluble hydroxide with a chemical formula of MOH. To determine whatM is, a student prepared 250.0 cm3 of MOH standard solution by dissolving 1.17 g of MOH in distilled water. Then the student titrated 25.0 cm3of the solution with 0.055 M H2SO4(aq) usingphenolphthalein as indicator. The titration was repeated several times and the mean titre was 18.85cm3.(a) Describe how the 250.0 cm3 of MOH standard solution was prepared. (b) (i) Calculate the molar mass of MOH. (ii) Determine what M is. (Relative atomic masses: H = 1.0, O = 16.0) THANKYOU!!!A reprecipitation was employed to remove occluded nitrate from BaSO4 precipitate prior to isotopic analysis of oxygen for geologic studies.9 Approximately 30 mg of BaSO4 crystals were mixed with 15 mL of 0.05 M DTPA in 1 M NaOH. After dissolving the solid with vigorous shaking at 708C, it was reprecipitated by adding 10 M HCl dropwise to obtain pH 3–4 and allowing the mixture to stand for 1 h. The solid was isolated by centrifugation, removal of the mother liquor, and resuspension in deionized water. Centrifugation and washing was repeated a secondtime to reduce the molar ratio NO-3 /SO-4 2 from 0.25 in the original precipitate to 0.001 in the purified material. What will be the predominant species of sulfate and DTPA at pH 14 and pH 3? Explain why BaSO4 dissolves in DTPA in 1 M NaOH and then reprecipitates when the pH is lowered to 3–4.A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the Ksp of magnesium hydroxide?
- A 14.92 g sample of bacon is pureed in a blender with 100.0 mL of water. The suspension is filtered and the clear solution containing dissolved sodium nitrite is adjusted to pH 2. The solution is treated with 25.0 mL of 0.0150 M KMnO4 to oxidize the nitrite to nitrate and after standing for 10 minutes, the excess KMnO4 is back titrated with 15.0 mL of 0.0818 M FeSO4. What is the concentration of nitrite in the bacon as parts per million?In developing a method for the determination of formic acid by neutralization volumetry, an analyst calculated the pH as a function of the addition of NaOH for the titration of 30.00 mL of 0.1280 mol/L formic acid with standardized NaOH with concentration of 0.1570 mol/L. With respect to this titration curve, determine the pH of the solution after adding the following volumes of NaOH: 0.00 mL; 10.00 ml; 25 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two decimal places and show your calculations.The composition of PBS is 0.137M NaCl, 0.012M Phosphate, 0.0027M KCl, pH 7.4. Below is the protocol to make 1 litre of 10x concentrate PBS. Combine the following: • 80g NaCl • 2g KCl • 14.4g Na2HPO4 (dibasic anhydrous) • 2.4g KH2PO4 (monobasic anhydrous) • 800mL distilled H2O 1. Adjust pH to 7.4 with HCl 2. Add H2O to 1L 3. Autoclave for 20 minutes on liquid cycle. Store at room temperature. Which ions are being produced by this process, assuming that each of the chemical compounds dissociate into their constituent parts once they are dissolved in water?
- 1ml of 1mg/ml of diluted aspirin powder solution is titrated by 0.005M NaOH. Before titration, 5 ml ethanol, 14 ml CO2 free water, and 4 drops bromothymol blue indicator is added into diluted aspirin powder solution. Mass of 0.005M NaOH used is obtained by weight titration = 1.1384g . [Molar mass of aspirin =180.15]; for solution, 1g=1mL at 25 degree Celcius. Calculate the purity of the powder.A 50-mL solution of 0.5005 N standard NaOH was added to a 0.9250-g sample of Aspirin and was boiled for 10 minutes. After cooling a full pipet of phenolphthalein was added to the solution before it was titrated with 24.7 mL of 0.5015 N standard HCl solution until the disappearance of the pink color. The same procedure was carried using a blank which consumed 4.6 mL of the same standard acid. Calculate for the %Aspirin in the sample. Atom weights: C =12, H =1, O =16.A weighed sample of sodium nitrite was treated with 0.05 mol of ceric sulfate in solution, in air-free conditions. The resulting solution was titrated with standard Fe(II) solution and 0.01 mol of Fe(II) were required. Determine the moles of sodium nitrite present in the weighed sample. NO2– + 2 Ce4+ + H2O → NO3– + 2 Ce3+ + 2 H+ Fe2+ + Ce4+→ Fe3+ + Ce3+
