Concept explainers
(a)
Interpretation: The chloride salt of lead is converted to its chromate salt to test its presence, the reason has to be confirmed.
Concept introduction: Metal ions present in a solution can be identified by a set procedure known as qualitative analysis. Different metal ions show different reactions with different reagent and thus either through the color of the precipitate formed or by smell the gas evolved the metal ion present can be identified.
Some metal ions when present in an aqueous solution containing anions or neutral species called Lewis base or ligands having a tendency to donate electron pairs to metal ions then complex ion formation will take place. Complex ions are stable and thus formation of these increase the solubility of the salt containing the metal ions same as in complex ions.
Example of metal ions that form complex ions includes
Example of Lewis bases includes,
(b)
Interpretation: The presence of
Concept introduction: Metal ions present in a solution can be identified by a set procedure known as qualitative analysis. Different metal ions show different reactions with different reagent and thus either through the color of the precipitate formed or by smell the gas evolved the metal ion present can be identified.
Some metal ions when present in an aqueous solution containing anions or neutral species called Lewis base or ligands having a tendency to donate electron pairs to metal ions then complex ion formation will take place. Complex ions are stable and thus formation of these increase the solubility of the salt containing the metal ions same as in complex ions.
Example of metal ions that form complex ions includes
Example of Lewis bases includes,
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Chemistry & Chemical Reactivity
- A 0.8000-g sample of iron ore containing 21.00% Fe is analyzed gravimetrically. If the final precipitate (assumed to be Fe,03) contains 20.0 mg of Al,O3 by mistake, what percentage of Fe does the analyst find?arrow_forward3. 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).arrow_forwardQuantitative analysis of Cl⁻ ion is often performed by atitration with silver nitrate, using sodium chromate as an indica-tor. As standardized AgNO₃ is added, both white AgCl and red Ag₂CrO₄ precipitate, but so long as some Cl⁻ remains, the Ag₂CrO₄ redissolves as the mixture is stirred. When the redcolor is permanent, the equivalence point has been reached.(a) Calculate the equilibrium constant for the reaction 2AgCl(s)+CrO₄²⁻(aq)⇌Ag₂CrO₄(s)+2Cl⁻(aq) (b) Explain why the silver chromate redissolves.(c) If 25.00 cm³ of 0.1000 M NaCl is mixed with 25.00 cm³ of 0.1000 M AgNO₃, what is the concentration of Ag⁺ remaining insolution? Is this sufficient to precipitate any silver chromate?arrow_forward
- 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?arrow_forward1. In using the centrifuge machine, how will this be remedied if there are only 3 separate liquid mixtures, in order to separate their respective precipitates 2. what is the extracting solvent for iodide and bromide ions? 3.What is the oxidation number of molybdenum in (NH4)3PO4.12MoO3 ? 4. Give the change in oxidation number for the element in the anion in group V which shows extensive change in color because it has undergone oxidation? 5. Determine the oxidation number of the Arsenic in Magnesium Ammonium Arsenate?arrow_forwardHow would you use an experimentally determined Ksp value to calculate that Ag2CrO4 should precipitate when 5ml of 0.0040 M AgNO3 are added to 5ml of 0.0024 M K2CrO4. You can come up with your own experimentally Ksp value. I just want to see steps in solvingarrow_forward
- Write the expression for the solubility-product constant for CaF2, and look up the corresponding Ksp value.arrow_forwardA student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?arrow_forwardSometimes it is not possible to indicate the end point of a titration.a) How can one proceed then and what is the name of the type of titration that can be performed? Briefly describe. An example in which this method can be used is in the determination of mercury, which forms strong complexes with EDTA, but for which there is no suitable indicator that can indicate the end point. b) You are given the task of determining the Hg2 + concentration in a sample solution? After adding an excess of EDTA, the sample solution is titrated with a magnesium solution. 20.00 ml of a 0.0452 M EDTA solution was added to 30.00 ml of sample solutionThe excess EDTA was determined by adding 0.0500 M Mg 2+ solution, consuming 4.37 ml to the end point.arrow_forward
- The standardization of same titrant during the determination of BOD5 of water sample was done separately for Day 1 and Day 5. Upon standardization, it turned out that the concentration of the titrant in Day 1 is higher than the concentration of the same batch of titrant in Day 5. How would you explain this discrepancy? The water used to prepare the Na2S2O3 solution was not boiled resulting to proliferation of bacteria. Too much starch indicator was added in the conical flask. Sulfuric acid was added first before potassium iodide. There were bubbles at the tip of the burette during titration.arrow_forwardPrecipitation of Ag+ with KOH a) Using the Ksp values provided in Table 2, predict whether it would form using 3 M KOH and 0.10 M of the metal nitrate solution. b) Using calculated Qsp values, now predict whether a precipitate would form after adding an additional 2 mL (excess) of 3 M KOH to each cation solution.arrow_forwardWrite a balanced equation and expression of Ksp for the dissolution of PbCl2arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning