Fe+3 (aq) + SCN – (aq) FeSCN +2 (aq) She mixes 4.00 mL of 2.00 mM SCN– and 5.00 mL of 2.00 mM Fe+3 ions, then diluting with 1.00 mL of water to give a total volume of 10.00mL. She measures the absorbance of the solution as being 0.210. If she has previously calculated the molar absorbtivity constant (ε) of the product to be 2583 cm–1 M–1, what is her best estimate for the K value for this reaction?
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mL of water to give a total volume of 10.00mL. She measures the absorbance of the solution as
being 0.210. If she has previously calculated the molar absorbtivity constant (ε) of the product to
be 2583 cm–1 M–1, what is her best estimate for the K value for this reaction?
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Solved in 4 steps
- Standardisation of the Permanganate Solution 5 C2O42-(aq) + 2 MnO4-(aq) + 16 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O Calculate the number of moles Na2C2O4 used in each of the three samples. Calculate the concentration of potassium permanganate in the standard solution for each of the three titrations you performed. Average the titration results and determine the concentration of Permanganate in the Standard Solution Recorded mass of sodium oxalate (Na2C2O4) in grams (g): Sample Mass M1 0.1134 M2 0.1136 M3 0.1124 M4 0.1100 Recorded initial- and final volume of Potassium Permanganate after titration: Sample Initial Volume in mL (Vi) Final Volume in mL (Vf) Total volume of KMnO4 used in mL. (Vf – Vi) 1 6.5mL 23.7mL 17.2mL 2 23.7mL 40.5mL 16.8mL 3 17.7mL 34.8mL 17.1mL 4 3.0mL 19.4mL 16.4mLCa(OH)2(aq)+2HCl(aq)CaCl2(aq)+H2O(l)An aqueous solution of Ca(OH)2with a concentration of 0.209 M was used to titrate 25.00 mL of aqueous HCl. 15.93 mL of the Ca(OH)2was required to reach the endpoint of the titration. A. How many moles of base were required to react completely with the acid in this reaction? _____mol Ca(OH)2 B. How many moles of HCl were present in the original 25.00 mL of acid?______mol HClA 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was added
- Direct titration: 10.90 ± 0.02 mL of an unknown KHP solution required 11.72 ± 0.02 mL of 0.1090 ± 0.0006 M NaOH to reach the end point. What is the concentration of KHP in the unknown solution reported with absolute uncertainty? If the unknown solution was prepared by dissolving 5.128 g of the unknown KHP (204.22 g/mol) in 100.00 mL of water, what is the weight percent of KHP in the sample?A 20.00 mL aliquot of sorbic acid solution (HC6H7O2) was titrated with 0.0985 M NaOH * (aq) using both an indicator and a pH meter. Ka (HC6H7O2) , is 1.7*10^ -5 . A total of 25.34 mL of 0.0985 M NaOH * (aq) was required to reach the equivalence point a) Calculate the molarity of the sorbic acid solution. b) Calculate the pH of the sorbic acid solution (use the RICE table) . c) .Calculate the pH and [C6H 7 O 2-] at the half-equivalence point . d) Calculate the pH at the equivalence point of the titration . (use Kb for hydrolysis of sorbate anion and RICE table ). e)Suggest an appropriate indicator for titration . Explain your choice . f) Calculate the pH of the solution after 10.00 mL of 0.0985 M NaOH * (aq) was added . (find moles of sorbic acid and sorbate and use Henderson Haselbalch equation ) Indicator pKa Phenolphthalein 9.3 Bromothymol blue 7.0 Methyl red. 5.0 Thymol blue. 2.0 Methyl violet…A sample of 0.10 M CH3COOH(aq) of volume 25.0 cm3 is titrated with 0.10 M NaOH(aq). The Ka for CH3COOH is 1.8 x 10-5. (a) What is the pH of 0.10 M CH3COOH(aq)? (b) What is the pH after the addition of 10.0 cm3 of 0.10 MNaOH(aq)? (c) What volume of 0.10 M NaOH(aq) is required to reach halfway to the stoichiometric point? (d) Calculate the pH at that halfway point. (e) What volume of 0.10 M NaOH(aq) is required to reach the stoichiometric point? (f) Calculate the pH at the stoichiometric point.
- Consider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq., 25 oC). The Ka HN3 = 4.50 x 10–4. What is the pH of the solution after 15.00 mL of NaOH has been added?The absorbance of a solution containing 5.0 x 10^-3 g/L of a solute in a 1.00 m cell is 1.00. Calculate the absorptivity and the molar absorptivity if the molecular mass of the solute is 1.25.To determine the concentration of an EDTA solution, the following magnesium(II) solution is prepared: metallic magnesium (m(Mg) = 0.5915 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.250 L and is filled to the graduation mark with water. The titration of an aliquot of magnesium(II) solution with a volume of 25.00 ml consumes (11.11 ml; 11.32 ml; 11.24 ml; 11.29 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.
- A student performed a titration to determine the exact concentration of NaOH(aq). The titration was performed against a standard 0.1000 M HCl(aq) solution. Phenolphthalein indicator was used. The following end-point volumes were recorded by the student in units mL: Trial Number Volume 1 25.06 2 25.15 3 25.02 4 25.17 5 25.07 Calculate the 95% confidence limit. Assume that there is no outlier. Provide your answer to the correct number of decimal places, without units, and without the ± sign. Use the T-table shown below.Q2) a) Explain the titration curve (variation of pH with respect to addition of titrant) with suitable diagram and reactions involved when a strong base is added as titrant to a weak acid as analyte. (b) The saline water discharged from a thermal desalination plant was analyzed and it has following composition.(i) If the discharged water sample contains 4.2 g of potassiumchloride (KCl) per 500 mL of solution, determine its molarity.(ii) The sample contains CaCl2 and its concentration was found to be 0.04M. Calculate grams of CaCl2 present in 100 mL of the sample. (c) In complexometric titration, explain why a constant pH need to be maintained during estimation of metal ions using EDTA.An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled to 15°C, treated with 2 drops of Pp indicator and titrated with 1.058 N H2SO4 requiring 6.8 ml to render the solution colorless. Upon adding 2 drops of MO and continuing the titration, 16.5 ml more of the acid were needed to complete the analysis. What is the quantitative composition of the sample? MW: NaOH = 40.0, Na2CO3 = 106.0, NaHCO3 = 84.01