A solution was prepared by dissolving 514 mg of K3Fe(CN)6 (329g/mol) in sufficient water to give 850 ml of solution. Calculate the pK for the solution.
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A solution was prepared by dissolving 514 mg of K3Fe(CN)6 (329g/mol) in sufficient water to give 850 ml of solution. Calculate the pK for the solution.
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- A 0.5843-g sample of a plant food preparation was analyzed for its N content by the Kjeldahl method, the liberated NH3 being collected in 50.00 mL of 0.1062 M HCl. The excess acid required an 11.89 mL back-titration with 0.0925 M NaOH. Express the results of this analysis in terms of (a) %N (b) %urea, H2NCONH2 (c) %(NH4)2SO4 (d) %(NH4)3PO4A 0.5123g sample (molar mass 204.23g/mol) of KHP was dissolved in about 25 mL of distilled water and titrated to the phenolphthalein end point with 28.75 mL of a sodium hydroxide solution. Calculate the molar concentration of the hydroxide solution.A 1.43 x 10-4 L solution of 45.7 mg/mL protein was analyzed using the Kjeldahl procedure. After digestion of the protein, the liberated NH3 was collected in 9.80 mL of 0235 M HCl. The unreacted acid required 10.75 mL of a standard solution of 0.0149 M NaOH for complete titration. Calculate the weight percent of nitrogen in the protein. (Molar mass N = 14.00674 g/mol)
- Directions: Solve the problem with a complete step-by-step solution. Titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar concentration of the KMnO4 solution? The chemical reaction is 2MnO4- + 5C2O42- + 16H+ + ----> 2Mn2+ + 10CO2 + 8H2O1. A mixture containing only KCl and NaBr is analyzed by the Mohr Method. A 0.3172-g sample is dissolved in 50 mL water and titrated to the Ag2CrO4 endpoint, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same endpoint. Report the % (w/w) KCl and NaBr in the sample. [Ans. 84.41 % (w/w); 17.59 % (w/w)]A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.5072-g sample is dissolved in 50 mL of water and titrated to the Ag2CrO4 end point, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.KCl = 74.551 NaBr = 102.89
- G.109. Calculate Qsp for calcium fluoride (Ksp = 3.9 × 10-11 ) when 180.0 mL of a 6.50×10-3 M solution of Ca(NO3)2 is added to 295.0 mL of a 5.40×10-3 M solution of KF.A 25.0-mL aliquot of vinegar was diluted to 250 mL in a volumetric flask. Titration of 50.0-mL aliquotsof the diluted solution required an average of 35.23 mL of 0.08960 M NaOH. Express the acidity of the vinegar in terms of the percentage (w/v) of acetic acid.Titration of a 0.824 g of 99.99% KHP (204.23 g/mol) with phenolphthalein required 18.3 mL of NaOH (40.00 g/mol) solution to reach the end point. The same titrant was used to analyze an impure acetic acid (CH3COOH, 60.06 g/mol) solution. A 10.0 mL aliquot of the sample required 12.9 mL of the titrant. What substance served as the primary standard?Which served as the indicator in the titration?What is the color at the end point?What is the concentration of the titrant?What is the molar concentration of the acetic acid solution?
- What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9? The pK a of the acid is 5.7.A 10.00 ml sample containing 6.0000 g/L of a mixture of KCI (74.5 g/mol) and NaCl (58.5 g/mol) was titrated with 0.10 M standard solution of AgNO; where 5.6 mL was needed to reach the end-point. Calculate the mass of sample (in grams). O 0.0063 b) 0.0337 c) 0.0033 d) 0.0221 e) 0.0600A certain local brand of “healthy” chicharon was found to contain 0.4132 g of NaCl after Fajan titration. How much sodium is present in the sample? MM NaCl=58.44 g/mol; MW Na+= 22.99 g/mol; MW Cl =35.45 g/mol 0.1626 mg 105.4 mg 0.1054 mg 162.6 mg