By titration, it is found that 29.9 mL of 0.108 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution. [HCI] = M
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![By titration, it is found that 29.9 mL of 0.108 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
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- Sulfide ion (S2- ) is formed in wastewater by the action of an aerobic bacteria on organic matter. Sulfide can be readily protonated to form volatile, toxic H2S. In addition to the toxicity and noxious odor, sulfide and H2S cause corrosion problems because they can be easily converted to sulfuric acid when conditions change to aerobic. One common method to determine sulfide is by coulometric titration with generated silver ion.At the generator electrode, the reaction is Ag Ag+ + e-. The titration reaction is S2- + 2Ag+ Ag2S(s). (a) A digital chloridometer was used to determine the mass of sulfide in a wastewater sample. The chloridometer reads out directly in ng Cl-.In chloride determinations, the same generator reaction is used,but the titration reaction is Cl- + Ag+ AgCI(s). Derive an equation that relates the desired quantity, mass S2- (ng), to the chloridometer readout in mass Cl- (ng). (b) A particular wastewater standard gave a reading of 1689.6 ng Cl-. What total charge in coulombs was required to generate the Ag+ needed to precipitate the sulfide in this standard? (c) The following results were obtained on 20.00-mL samples containing known amounts of sulfide.17 Each standard was analyzed in triplicate and the mass of chloride recorded. Convert each of the chloride results to mass S2- (ng). (d) Determine the average mass of S2- (ng), the standard deviation, and the %RSD) of each standard. (e) Prepare a plot ofthe average mass of S2- determined (ng) versus the actual mass (ng). Determine theslope, the intercept, the standard error, and the R2 value. Comment on the fit of the data to a linear model. (f) Determine the detection limit (ng) and in parts per million using a k factor of 2 (see Equation 1-12). (g) An unknown wastewater sample gave an average reading of 893.2 ng Cl. What is the mass of sulfide (ng)? If 20.00 mL of the wastewater sample was introduced into the titration vessel, what is the concentration of S2- n parts per million?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 ) = 204.22A Medical Technology student was given a capsule of a multivitamins and she was asked to determine the % by mass (w/w) of ascorbic acid present in the capsule. The student analyzed the 2.001 g sample using volumetric titration. The following data was generated in the analysis: KIO3 + 5KI + 6H+ → 3I2 + 6K+ + 3H2O C6H8O6 + I2 → C6H6O6 + 2I- + 2H+ Table 1. Standardization of KIO3 Molarity of Ascorbic Acid Standard Solution 0.03542 M Volume of Ascorbic Acid 25.00 mL Volume of KIO3 8.70 mL Molarity of KIO3 ______________M Table 2. Determination of Ascorbic Acid Concnetration Initial burette reading, KIO3 0.00 mL Final burette reading, KIO3 33.60 mL Volume consumed, KIO3 33.60 mL MM of Ascorbic Acid 176.12 g/mole choices 7.30% 30.1% 33.6% 32.5%
- The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.Suppose you are given 0.0856ppm to be the concentration of dissolved lead found in pond water after dilution factor of 1:100 in 100ml volumetric flask and the other sample is diluted at the dilution factor of 1:2 and the concentration is 2.14ppm. How would you comment on the amount of lead in pond waterCalculate the solubility at 25°C of CaF2 in pure water and in a 0.0060M NaF solution. You'll find Ksp data in the ALEKS Data tab. (CaF2 Ksp is 3.45×10−11 Round both of your answers to 2 significant digits. solubility in pure water: ? gL? solubility in 0.0060 M NaF solution:? gL?
- a 10g soil sample was gently stirred with 250 ml of 1.0 M CH3COO(NH4) solution for 24 h and centrifuged to separate the solution. The solution recovered after centrifugation was titrated with distilled water to a volume of 1 liter and analyzed for cations. Analytical results showed that the solution contained 20 mg/L Ca, 2 mg/L Mg, 1 mg/L K, and 0.5 mg/L Na. Calculate the number of cation exchange equivalents and express it in meq/100 g of soilIn one trial determination of the concentration of NaOCl in the diluted bleach sample, 10.00 mL of the diluted bleach solution required 23.32 mL of 0.0195 M Na2S2O3 titrant to reach the endpoint. What is the molar concentration of NaOCl in the diluted bleach solution?To determine the concentration of glucose in the packaged juice industry, 50 mL of sample is analyzed. Analysis of it (and other reducing sugars) was carried out there using triiodide back titration. An excess volume of 75.00 mL of 0.338 M triiodide standard solution in alkaline medium was added to the glucose solution. The resulting solution was acidified and the excess triiodide was titrated with 18.37 mL of standard 0.526 M thiosulfate solution. Calculate is the concentration in ppm in the sample. In alkaline medium: Glucose (C6H12O6) / Gluconate (C6H11O7-), Triiodide (I3- ) / Iodide (I-) In acid medium: Thiosulfate (S2O32-) / Tetrathionate (S4O62-), Triiodide (I3- ) / Iodide (I-)
- Calcium fluoride is considered as a relatively insoluble compound and therefore lime or slakedlime has been considered as a possible material to remove excess fluoride in water of boreholesin certain parts of the country. The solubility product of CaF2 is Ksp = 3 x 10 – 11 and that ofCa(OH)2 isKsp =8x10-61. How much lime can be added to the water to remove 10 mg of F- ion per litre ofborehole water?(The atomic masses are Ca: 40.08; F: 19.00; O: 16; H: 1)You have performed an iodimetric titration using a commercial vitamin C tablet. Based on the following information below, calculate the %(w/w) of vitamin C(MM=176.16 g/mol) in the tablet: Mass of tablet dissolved in 250.0 mL: 5.422 g Aliquot volume of sample titrated: 25.00 mL Concentration of KIO3: 0.023 M Final burrette volume: 41.31 mL Initial burrette volume: 8.89 mL Blank volume: 0.14 mLCalculate the solubility and molar solubility of Cu3(PO4)2 (MW=380.58 ; Ksp=1.4x10-37).
