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1) How many millileters of 0.100M KI are needed to react with 40.00 ml of 0.0400 M Hg^2(NO3) if the reaction is:
Hg2^2+ + 2I -> Hg2I2(s) ?
2) A solution of NaOH was standardized by titration of a known quantity of the primary standard potassium hydrogen phthalate (KHP, FM 204.221 g/mol). Titration of 0.824 g of potassium hydrogen phthalate required 38.314 mL of NaOH to reach the endpoint detected by phenolphthalein. Find the concentration of NaOH in molarity (M).
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- 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)1. What is the molar solubility of PbCl2 in a solution of 0.23 M CaCl2? Ksp = 1.6 ✕ 10-5 for PbCl2. 2. What is the Qsp when 32.0 mL of 6.50 ✕ 10-7 M Na3PO4 are mixed with 41.4 mL of 5.50 ✕ 10-5 M CaCl2? Assume the volumes are additive. Ksp = 2.0 ✕ 10-29. 3. What is the Qsp when 61.0 mL of 1.50 ✕ 10-4 M AgNO3 are mixed with 80.0 mL of 5.20 ✕ 10-3 M CaCl2? Assume the volumes are additive. Ksp = 1.6 ✕ 10-10. 4. What [I-1] is needed to start the precipitation of AgI from a saturated solution of AgCl? Ksp = 2.9 ✕ 10-16 for AgI and Ksp = 1.2 ✕ 10-10 for AgCl.A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. Report the purity of the Na2CO3 sample. [Ans. 90.9 % (w /w )]
- 1. 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. The percentage Na2CO3 (MW = 106.0 g/mole) in the tested sample is ________ % ? Note: Express final answer using least number of significant figures. 2. The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01 g/mole), and HCO3- (MW = 61.01 g/mole), which may be present singularly or in combination. Titrating a 10.0-mL sample to a phenolphthalein endpoint requires 38.12 mL of a 0.5812 M solution of HCl, and an additional 18.67 mL of the same titrant to reach the methyl orange endpoint. The composition of the sample is _________% CO3-2 and ___________ % OH- Note: Express final answers using least number of significant figures.A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample. Please use the factor label method in answering.A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample.
- 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 mL0.7050-g of pure KHP (FW = 204.2) was dissolved and titrated with 35.00mL of NaOH solution. The excess NaOH was backtitrated with 5.00mL of HCl solution. In a separate titration it was found that 30.00mL of NaOH will react with 28.00mL of HCl. Find the molarity of NaOH and HCl.Following the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol) used to standardize a 0.987 N sulfuric acid solution. 1. What specific type of titration is involved? A. Direct Acidemetry B. Direct Alkalimetry C. Residual Acidemetry D. Residual Alkalimetry 2. What is the analyte- titrant chemical reaction involved? A. Strong Base+Weak Acid B. Weak Acid+Strong Base C. Strong Acid+Weak Base D. Weak Base+Strong Acid 3. What is the preferred indicator for the chosen type of reaction above? A. Methyl Orange B. Penolphtalein C. Methyl Red 4. Consider that the burette was completely filled to the 0mp mark before titrating. What is the volume of titrant consumed based from the image below? A. 22.9 mL B. 22.2 mL C. 21.3 mL D. 22.7 mL 5. What is the unknown weight (grams) the problem? Your Answer:
- How much amount (in grams) do you need to prepare the following solutions 500.0 mL 0.1000 M stock EDTA solution from Na2H2EDTA•2H2O (FW=372.24) and MgCl2•6H2O crystals 100.0 mL 0.0500 M stock Ca2+ solution from pure CaCO3 (FW=100.09) and concentrated HCl 250 mL 1.0 M NH3-NH4+ pH 10 buffer solution from NH4Cl and NH3A 0.1214-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.07011 M AgNO3, the sample was back titrated with 0.06021 M KSCN, requiring 27.15 mL to reach the end point. State the net ionic equation.After titration, weight percent of oxalate in K3[Fe(C2O4)3] (MW: 437.2 g/mol) sample was determined to be 55.8%. What is the percent error of oxalate content determination?