All of the following regarding Argentometric titration are correct except a. Chromate indicator is used in Mohr method b. Greater values of Ksp give sharper break and inflection at end point c. Increasing reagent concentration makes the change in pAg larger. d. Volhard's method involves adding excess AgNO; to the analyte, then back titration with standard SCN solution. e. Fajan's method depends on adsorption of fluorescence indicator on the colloidal precipitate formed
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- 10mL of a 10% by weight MgCl2 solution (density = 1.1 g / mL) is precipitated as magnesium ammonium phosphate after necessary processes, filtered and washed. The precipitate is dissolved in 50mL 1M HCl and excess acid is titrated with 2.0M NaOH solution in the presence of methyl orange. Find the NaOH consumption (Mg = 24,3g / mol, Cl = 35,5g / mol)If a 25.00 ml aliquot of a solution containing sulfide ions was added to 25.00 ml of 0.0103 M Cu2+ solution. The CuS precipitate was washed and collected. The pH of the combined filtrate and washings was then adjusted by the addition of ammonia and the solution was titrated with 0.01453 M EDTA, using a suitable indicator. The endpoint volume was found to be 12.20ml. Find the molarity of the sulfide in the sample solution.In complexometric titration ‘the reaction with analyte should be rapid andcomplete’ give reason with suitable justification for the above statement.
- Which of the following is a good description of a standard solution as a titrant? a) selectively reactive with the analyte b) only reacts with the matrix c) oxidize when exposed to air d) reacts very slowly but completelyChemistry A 20 mL solution containing both Ca2+ and Mg2+ cations is diluted in to 100 mL. When 10 mL of this solution is taken and titrated with 0.05 M EDTA at pH = 10 in the presence of Erio – T indicator, the consumption is found as 12 mL. A new 10 mL was taken from the same solution and (NH4)2C2O4 is added on it and then formed the precipitate is filtered. The filtered solution is titrated with the same EDTA solution and the consumption is found as 3 mL. So find the Ca2+ and Mg2+ amounts in the main sample solution in terms of mg/L.A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)
- A solid containing tris was dissolved in water and brought to a total volume of 50.00 ml. A 10.00 ml aliquot of the solution was titrated with 0.09978 M HCl to a bromcresol green endpoint. The aliquot consumed 38.93 ml of titrant. Calculate the weight of tris in the original sample.A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A small amount of MgCl2 solution is added to a 25 mL aliquot of the solution., and the mixture is titrated with (ethylenediaminetetraacetic acid) EDTA to the Eriachrome Black T (with MgCl2 is used as indicator) end point. The mixed solution requires 28.55 mL of the EDTA solution to reach the end point. A similar amount of MgCl2 solution requires 2.60 mL to reach the endpoint. A 100-mL sample of hard water is titrated with 22.4 mL of the EDTA solution created above. The same amount of MgCl2 is added as previously and the total volume of EDTA solution required is 22.44 mL. a) Assume all of the Ca2+ in the water comes from CaCO3. How many moles of CaCO3 are in 1 L of water? How many grams of CaCO3 are in 1 L of water? c) If 1 ppm CaCO3 = 1 mg/liter, what is the water hardness in ppm CaCO3 ?A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A small amount of MgCl2 solution is added to a 25 mL aliquot of the solution., and the mixture is titrated with (ethylenediaminetetraacetic acid) EDTA to the Eriachrome Black T (with MgCl2 is used as indicator) end point. The mixed solution requires 28.55 mL of the EDTA solution to reach the end point. A similar amount of MgCl2 solution requires 2.60 mL to reach the endpoint. A 100-mL sample of hard water is titrated with 22.4 mL of the EDTA solution created above. The same amount of MgCl2 is added as previously and the total volume of EDTA solution required is 22.44 mL. a) What volume of EDTA is used in titrating the Ca2+ in the hard water? b) How many moles of EDTA are there in that volume? c) How many moles of Ca2+ are in 100 mL of water?
- A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A small amount of MgCl2 solution is added to a 25 mL aliquot of the solution., and the mixture is titrated with (ethylenediaminetetraacetic acid) EDTA to the Eriachrome Black T (with MgCl2 is used as indicator) end point. The mixed solution requires 28.55 mL of the EDTA solution to reach the end point. A similar amount of MgCl2 solution requires 2.60 mL to reach the endpoint. A 100-mL sample of hard water is titrated with 22.4 mL of the EDTA solution created above. The same amount of MgCl2 is added as previously and the total volume of EDTA solution required is 22.44 mL. How many moles of Ca2+ are in 100 mL of water?A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A small amount of MgCl2 solution is added to a 25 mL aliquot of the solution., and the mixture is titrated with (ethylenediaminetetraacetic acid) EDTA to the Eriachrome Black T (with MgCl2 is used as indicator) end point. The mixed solution requires 28.55 mL of the EDTA solution to reach the end point. A similar amount of MgCl2 solution requires 2.60 mL to reach the endpoint. How many milliliters of EDTA are needed to titrate the Ca2+ ion in the sample? How many moles of EDTA are there in the volume calculated for the question above? What is the molarity of the EDTA solution?An aqueous solution of 0.2100 g of a mixture containing potassium cyanide and potassium chloride required 14.56 mL of 0.1000 M silver nitrate to produce a faint permanent turbidity; 30.00 mL more of the silver nitrate was added (an excess) and the precipitate of AgCl and AgCN filtered off from the solution. The filtrate and washings were titrated with 13.06 mL 0.1000 M thiocyanate solution. Calculate the percentages of KCl and KCN in the sample.