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Q: f 145 mL of a 0.0078 mol/L solution of CuNO3 was mixed with 195 mL of a 1.48 x 10-3 mol/L solution…
A: Solution -
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- Why homogenously formed precipitates are better suited for analysis than a precipitate formed by direct addition of a precipitating agent?What do the ions that gave a precipitate when mixed with AgNO3 have in common? Hint given: Identify the ions and the Group of the Periodic Table to which they belongFor µ=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X- is 0.75. Calculate how many micrograms of MX2 dissolve in 324 mL of 0.10 M NaX solution. The molar mass of MX2 is 201 g/mol, and its Ksp is 3.8 x 10-9. Note that NaX is a salt of X-, an ion that participates in the equilibrium that applies to the solubility of MX2. a. 110 µg b. 27 µg c. 9.7 µg d. 44 µg e. 1000 µg
- What do the ions that gave a precipitate when mixed with AgNO3 have in common?Mixing 20.0 mL of 5.00 M magnesium chloride solution with 40.0 mL of 2.00 M silver (I) nitrate solution results in a precipitate. The resulting mixture contains a total free chloride ion concentration of: a) 2.86M Cl- b) 2.00M Cl- c)0.120M Cl- d) 0.500M Cl- e) not enough information is provided1. How quantity Qsp and Ksp can be used in predicting precipitate formation? 2. How precipitation titrations work? 3. How will you differentiate Mohr method, Volhard method and Fajans method?
- 500 mL of river water was subjected to sulfate determination by the barium gravimetric method. The final weight of the precipitate was 74.3 mg. What was the sulfate concentration in mg/L?Write all the reactions involved in the Mohr's method, if an unknown solution containing chloride ions is titrated against silver nitrate solution. Suggest an indicator and what is its colourin the unknown chloride solution ? and Why is KSCN solution used as burette solution and not in conical flask in Volhard's method?Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a precipitate containing NiCO3 be washed to dissolve 0.100 g of this compound? Assume that the wash water becomes saturated with NiCO3 (Ksp = 1.36 × 10–7).(b) If the NiCO3 were a contaminant in a sample of CoCO3 (Ksp = 1.0 × 10–12), what mass of CoCO3 would have been lost? Keep in mind that both NiCO3 and CoCO3 dissolve in the same solution.
- If 2 mL of 0.02 M AgNO3 is added to 2 mL 0.011 M K2CrO4, which reagent is in excess? should a precipitate occur?3. Fill in the boxes in the following flowsheet by indicating the identities of ions or complexes found in the various precipitates (ppt) and supernatants (snt).Briefly explain why the sparingly soluble product mustbe removed by filtration before you back-titrate the excesssilver ion in the Volhard determination of a) chloride ion. b) cyanide ion. c) carbonate ion.