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- In the conductivity test, _____________________ is going to result to a brightly lit light bulb. a. 70% v/v ethanol b. 1.0 M citric acid c. Mixture of 10.0 mL 1.0 M Mg(OH)2 and 10.0 mL 1.0 M HNO3 d. Glacial acetic acidA solution of Ca(OH)2 (FM = 74.09) was used in determining the equivalent weight of an unknown acid. To do so, the said solution was standardized against 0.1235 g KHP (FM = 204.22), requiring 7.45 mL to reach the phenolphthalein endpoint. On the other hand, a 0.0543 g unknown acid requires 12.85 mL standard Ca(OH)2 to reach the desired endpoint.a. Calculate the standard normality of Ca(OH)2.b. Calculate the equivalent weight of the unknown acid.c. From the information in the table, what is the most probable identity of the unknown acid?Compute the molarity of KMnO4 solution if 1.0092 g of pure FAS required 25.11 mL of KMnO4 solution to reach end point in an acidic medium. An impure sample of FAS weighed 1.2352 g and it required 26.01 mL of KMnO4 solution (use molarity from Q#2) to reach end point in an acidic medium. Compute %Fe in this sample.
- A local company sent you their green alternative for window cleaner to be tested for percent (w/v) acetic acid content. For your experiment, you first standardized your NaOH titrant with 0.8053 g of (99.80 % purity) KHP. You used 40.60 mL of NaOH for your standardization. After that you then analyzed a 10.00 mL sample and found that you needed 43.20 mL NaOH to reach the end point. Summary of results: Standardization Sample analysis KHP Weight (g) 0.8053 g Volume of sample 50.00 mL Purity 99.80% NaOH (mL) used 33.20 mL NaOH (mL) used 40.60 mL Determine the following: Molarity of NaOH % (w/v) acetic acidThe solution is 0.20 M MgSO4 and 0.70 M NaCl. Solid Na2SO4 is added to the solution so that the total ionic strength of the solution is 3.3. What is the Na2SO4 concentration of the solution then. The change in solution volume is not taken into account when adding reagents.A 10 mL sample of sulfuric acid solution required 16.85 mL of NaOH solution in a titration. Each mL of the NaOH solution was equivalent to 0.2477 g of potassium hydrogen phthalate. Calculate the sulfuric acid content in %w/v. MW of sulfuric acid, 98; MW of potassium hydrogen phtalate(KHC8H4O4 ) = 204.22
- Sixty mL of an impure acid solution was diluted to 500mL. A 30.00mL portion of this solution was titrated with 25.00mL of 0.1230M NaOH solution. Calculate the % (w/v) HAc in the sample. (FWt HAc = 60) Show all the solutions involved and round-off final answers to two decimal places except for Molarity. (Molar concentrations should be in four decimal places)5. How to prepare 50mL of 375 mM citrate buffer pH 1.8 (8% (v/v) ethanol)Use the follow data below and answer the following questions: Component Concentration (mg/L) CO2 8 Ca2+ 45 Mg2+ 13 Sr2+ 12 Alkalinity 270 Determine the quantity (mass flow) of CaO and Soda Ash using practical solubility limit required to treat hard water taking volumetric flow as 145000 L/d and pH of 7.5 and purity of both reagents as 97%.
- Please answer as soon as possible. Thank you! A 10.000-g cocoa powder sample was dissolved in concentrated acid and then diluted to 100.00 mL using distilled water. The solution was found to contain 5.45 uM Fe. Calculate concentration of Fe (MM: 55.845) in the cocoa powder sample in parts-per-million (ppm) (weight by volume).A STOCK SOLUTION containing 0.1581 g/L K2CrO4 was prepared.In order to make the CALIBRATION STANDARD, 5 ml of the STOCK was transferredinto a 50ml volumetric flask and then diluted with an appropriate solvent.Calculate:(a) The ppm of K2CrO4 in the CALIBRATION STANDARD.(b) The molarity of K2CrO4 in the CALIBRATION STANDARD. (c) Calculate the molar absorptivity of K2CrO4 (at 371.0 nm). Assume that Beer's Law isobeyed over this concentration range.At 371.0 nm, this CALIBRATION STANDARD in a cell of path length 1.00 cm gave a %T of 59.752.The total cation content of natural water is often determined by exchanging the cations for hydrogen ions on a strong acid ion-exchange resin. A 25.00 mL sample of a natural water was diluted to 100.00 ML with distilled water, and 2.06 g of a cation - exchange resin was added. After stirring, the mixture was filtered and the solid remaining on the filter paper was washed with three 15.00 mL portions of water. The filtrate and washings required 16.30 mL of 0.0282 M NaOH to give a bromocresol green end point. a) Calculate the number of millimoles of cation present in exactly 1.00 L of sample. b ) Report the results in terms of milligrams of CaCO3 per liter. Only typed solution.