For a 25 mL, 0.1 M solution of the following metal ion solutions, which one gives the heaviest precipitate when an excess of precipitating agent has been added to ensure complete precipitation? Ba (II) Fe (II) Hg (II) Zn (II) Which of the following metal ions best interferes with Ba(ll) precipitation with sulfate? Be (II) Ca (II) Mg (II) Sr (II)

For a 25 mL, 0.1 M solution of the following metal ion solutions, which one gives the heaviest precipitate when an excess of precipitating agent has been added to ensure complete precipitation? Ba (II) Fe (II) Hg (II) Zn (II) Which of the following metal ions best interferes with Ba(ll) precipitation with sulfate? Be (II) Ca (II) Mg (II) Sr (II)

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 115E: A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of...

See similar textbooks

Similar questions

If Sn3(PO4)2 solution is to be subjected to argentometric titration, a) Write the balanced titration reaction. (products are Ag3PO4(s),, other ions are spectator ions b) Write the stoichiometric relationship (fundamental eqn) between the titrant (AgNO3) and the titrand (Sn3(PO4)2. c) Is this a feasible titration technique? Why?
If a sample of silver coin weighing 0.2500 g gives a precipitate of AgCl weighing 0.2991 g, What wt of AgI could have been obtained from the same wt of sample?
An analytical chemist has a solution containing chloride ion, Cl−. She decides to determine the amount ofchloride ion in the solution by titrating 50.0 mL of this solution by 0.100 M AgNO3. As a way to indicate theendpoint of the titration, she added 1.00 g of potassium chromate, K2CrO4 (see Figure 1). As she slowly addedthe silver nitrate to the solution, a white precipitate formed. She continued the titration, with more whiteprecipitate forming. Finally, the solution turned red, from another precipitate. The volume of the solution atthis point was 60.3 mL. How many moles of chloride ion were there in the original solution? How many molesof chloride ion were there in the final solution? You may make any reasonable approximations
The purity of a pharmaceutical preparation of sulfanildamide (C6H4N2O2S), is prolonged oxidizing the sulfur in the sample to SO2 and bubbling this SO2 through a solution of H2O2 which converts it to H2SO4. The acid is titrated with a standard solution of NaOH (0.1251 M) until the end point with bromothymol blue, which changes color when both protons of the acid sulfuric have been neutralized. Calculate the purity of the preparation in % by weight given that a sample of 0.5136 g required 50.00 mL of the NaOH solution
What volume of 0.100 M Na3PO4 is required to precipitate all the lead (II) ions from 350.0mL of 0.250 M Pb(NO3)2?
If a solution contains 0.0020 mol of CrO4 2− per liter, what concentration of Ag+ ion must be reached by adding solid AgNO3 before Ag2CrO4 begins to precipitate? Neglect any increase in volume upon adding the solid silver nitrate.
Suppose that 150 mL of 0.200 M K2CO3 and 100 mL of 0.400 M Ca(NO3)2 are mixed together. Assume that the volumes are additive, that CaCO3 is completely insoluble, and that all other substances that might be formed aresoluble. Calculate the mass of CaCO3 precipitated, and calculate the concentrations in the final solution of the four ions that were present initially.
Three solutions are mixed together to form a single solution;in the final solution, there are 0.2 mol Pb(CH3COO)2,0.1 mol Na2S, and 0.1 mol CaCl2 present. What solid(s) willprecipitate?
The solubility of Mn(OH)2 in water is 0.0002 g/100 mL. What is the solubility in gramformula weights per liter in a solution which is 0.01F with respect to the hydroxide ions?
If a solution containing 0.10 M Cl2, Br2, I2, and CrO4 is treated with Ag1, in what order will the anions precipitate?
Suppose you have a solution that might contain any or allof the following cations: Ni2+, Ag+, Sr2+, and Mn2+. Additionof HCl solution causes a precipitate to form. After filteringoff the precipitate, H2SO4 solution is added to the resultingsolution and another precipitate forms. This is filtered off,and a solution of NaOH is added to the resulting solution.No precipitate is observed. Which ions are present in each ofthe precipitates? Which of the four ions listed above must beabsent from the original solution?
7) Write the net ionic equations for the reaction with OH- by whicha) Al3 + forms a complex ionb) Al (OH) 3 dissolvesc) Fe3 + forms a precipitate