7 t sample of 0.05 mol dm sodium chloride is mixed with a 5 cm3 sample of 0.05mol dm potassium iodide..10 cm3 of acidified o 05 moldm3 silver nitrate is then added, followed by concentrated ammonia solution. What is seen after the addition of an excess of concentrated ammonia solution? a cream precipitate a white precipitate a yellow precipitate D no precipitate

7 t sample of 0.05 mol dm sodium chloride is mixed with a 5 cm3 sample of 0.05mol dm potassium iodide..10 cm3 of acidified o 05 moldm3 silver nitrate is then added, followed by concentrated ammonia solution. What is seen after the addition of an excess of concentrated ammonia solution? a cream precipitate a white precipitate a yellow precipitate D no precipitate

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 73E: A roll of 35-mm black and white photographic film contains about 0.27 g of unexposed AgBr before...

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A roll of 35-mm black and white photographic film contains about 0.27 g of unexposed AgBr before developing. What mass of Na2S2O35H2O (sodium thiosulfate pent hydrate or hypo) in 1.0 L of developer is required to dissolve the AgBr as Ag(S2O3)23- (Kf=4.71013)?
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
Which would precipitate first upon addition of the sodium salts of the following anions to solutions 0.10 M in Pb(NO3)2?ion Ksp of lead saltA. IO3- 3.2 x 10-13B. Cl- 1.6 x 10-5C. Br- 4.0 x 10-5D. C2H3O2- 1.8 x 10-3E. OH- 1.2 x 10-15 The answer is E
The Ksp for BaCrO4 is 1.2×10−10.1.2×10−10. Will BaCrO4 precipitate upon mixing 10 mL of 1×10−41×10−4 M Ba(NO3)2 with 10 mL of 1×10−41×10−4 M K2CrO4?
If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/L
What is the Cl- concentration just as Ag2CrO4 begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.015 M Cl- and 0.015 M I-? Ksp for Ag2CrO4 is 1.2 x 10-12.
A 45.0 mL sample of 0.0015 M BaCl2 was added to a beaker containing 75.0 mL of 0.0025 M KF. Will a precipitate form. Ksp BaF2 = 1.7 x10-6
The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.
Magnesium fluoride (MgF2, MW = 62.30 g/mol) is slightly soluble in water, with Ksp = 7.4 x 10^-11 at T= 25. C.a) Give the correctly balanced solubility reaction and expression for Ksp for MgF2.b) What mass of magnesium fluoride will dissolve in 1.000 L of pure water?
The Ksp of Fe3(PO4)2 is 2.70⋅10−252.70⋅10-25 M. Calculate the solubility of each ion in a saturated solution: M Fe2+ M PO43-
A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br- The liberated nickel ion required 11.70 mL of 0.002146 M EDTA. Calculate mmol Ni in the 50.00 mL aliquot. Calculate mmol Br- in the 50.00 mL aliquot. Calculate the percentage of NaBr (102.894) in the 1.000 g sample.
A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br- The liberated nickel ion required 11.70 mL of 0.002146 M EDTA The other 50.00 mL remaining solution was also analyzed for its Br- content by potentiometry using a metallic electrode of the second kind. Ecell recorded in running the solution using the potentiometric set-up was Ecell = 0.0286 V. (E0Ag/AgBr = 0.095 V) g) Compute for Eind. h) Compute pBr in the 50.00 mL aliquot. i) Compute for % NaBr ( in the potentiometric technique). j) Calculate the error between the obtained % NaBr fr the EDTA titration technique and the % NaBr from the potentiometric technique.