Q: Ag* 0.0000133038 Cr 0.0000133038
A: Concentration of Ag+ = 0.0000133M Concentration of Cl- = 0.0000133M
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- State in your own words what the abbreviation α Y4- means with regards to EDTA speciation in water. Calculate α Y4- for EDTA at (a) pH 3.50 and (b) 10.50.In order to analyse mercury with AAS, which method will you prefer?Exactly 6.00 ml of acetic acid (density = 1.05 g/mL), MW =60.05) was added to a 1 –liter volumetric flask, and the flask was filled to the mark with distilled water. A portion of the resulting solution was added to a conductance cell (k = 1.25 cm-1), and the conductance was found to be 416 μS. Calculate the dissociation constant Ka of acetic acid. ΛoH+= 349.8 Scm2/mole and ΛoCH3COO- = 41 Scm2/mole
- Find the conc of free Mg2+ in 0.050 M Na2[Mg(EDTA)](i.e. MgY2-) at pH 9.00.Bromine H2O + Cl2 H20 ----- __________. A. violet and reddish brown layered solution B. No reactionPlease answer the following with complete solution. Thank you. A mixture placed in an Erlenmeyer flask comprises 6mL of silica gel and 40mL of a solvent containing, in solution, 100mg of a non-volatile compound. After stirring, the mixture was left to stand before a 10mL aliquot of the solution was extracted and evaporated to dryness. The residue weighed 12mg. Calculate the adsorption coefficient, K=CS/CM, of the compound in this experiment.
- Calculate potentials after the addition of 10.00, 25.00,50.00, and 50.10 mL of the reagent. Where necessary, Assume that [H+]= 1.00 throughout. 50.00 mL of 0.1000 M V2+ with 0.05000 M Sn4+At a pH of 10 what is the fraction of EDTA that is in the form Y4-? I got 0.30 but I believe that is wrong.For each of the following experiments, try to identify the major probable sources of random and systematic errors, and consider how such errors may be minimized: 1. The iron content of a large lump of ore is determined by taking a single small sample, dissolving it in acid, and titrating with ceric sulphate after reduction of Fe (III) to Fe (II). 2. The same sampling and dissolution procedure is used as in (a) but the iron is determined colorimetrically after addition of a chelating reagent and extraction of the resulting colored and uncharged complex into an organic solvent. 3. The sulphate content of an aqueous solution is determined gravimetrically with barium chloride as the precipitant.
- Write a flow chart for the separation and identification of Ag+, Bi3+, and Ni2+Calculate the pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00 and 30.00 mL of 0.0100 M EDTA to 25.00 mL of 0.00250 M Zn2+. Assume that both the Zn2+ and EDTA are 0.0100 M in NH3 to provide a constant pH of 9.0Consider the titration of 25.0ml 0.0100M Sn2+ by 0.0500M Tl3+ in 1M HCl using Pt and saturated calomel electrodes , calculate E at following volumes of Tl3+ : 1, 5 and 10ml