An unknown whitesolid consists of two compounds, each containing a different cation. As suggested in the illustration, the unknown is partially soluble in water. The solution is treated with NaOH(aq) and yields awhite precipitate. The part of the original solid that is insoluble in water dissolves in HCI(aq) with the evolution of a gas. The resulting solution is then treated with
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General Chemistry: Principles and Modern Applications, Loose Leaf Version (11th Edition)
- The mass of K3PO4 needed to prepare 250.0mL of an aqueous solution in which PO4-3 concentration is 0.0550M. The answer is ……………………… How many grams of silver sample is equal to 0.0417 mole of silver The answer is ……………………… When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of PbI2, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the recovered PbSO4 is found to have a mass of 0.0471g, what was the concentration of iodide ions in the original solution The answer is ……………………………… Express 96.342 m using 2 significant figures The answer is ………………………………. The oxidation number of sulfur in (Na2S2O5) is? The answer is ………………………………arrow_forwardTo determine the fluoride content in an aqueous and chloride-containing preparation of ammonium fluoride, the following analysis was performed. 105.2 mg of the preparation was dissolved in 100.0 mL of water. Then a 300 mL 40 mM lead chloride solution was added, whereby all fluoride ions were precipitated out of the solution in the form of the sparingly soluble salt PbClF (s). The precipitate was separated and washed at 15 degrees with a lead fluoride chloride saturated solution and dried at 130 degrees. The precipitate weighed 651.3 mg. a) Calculate the fluoride content (as % by weight F) in the preparation.b) Determine the purity of the ammonium fluoride preparationarrow_forwardAs part of the analysis of water samples, the hardness of water is commonly measured and calculated. It is commonly expressed in ppm by mass (parts per million) of CaCO3. Parts per million is also equivalent to milligrams of CACO3 per liter of water. In a sample taken by an environmentalist, he was able to observe a hardness count of 205 mg CacO3/L. Given this hardness count of the sample, what is the molar concentration of Ca2+ ions in the water sample?arrow_forward
- 0.1 g of the mixture of na2so4 and k2so4 is taken and 100 ml of solution is prepared. 10 ml of this prepared solution is placed in a beaker and some distilled water is added. A mass of 15.5 mg is obtained by precipitation with Bacl2 at PH=5, then filtering and bringing to a constant weight at 800 °C. Calculate the percentages of Na2so4 and K2so4 in the mixture accordingly.arrow_forwardAn unknown salt X reacts with hot conc. H2SO4 to produce a brown coloured gas which intensifies on addition on copper turnings. On adding dilute ferrous sulphate solution to an aqueous solution of X and then carefully adding conc. H2 SO4 along the sides of the test tube, a brown complex Y is formed at the interface between the solution and H2 SO4. Identify X and Y and write the chemical equation involved in the reaction.arrow_forwardWhile working in a metal processing facility, Letlen had accidentally mixed two metal vatstogether creating an alloy. One vat was labeled for cadmium, while the other was not. It canbe assumed that these are of pure metal composition. To identify this metal, Letlen took 1.000 g of the homogenous alloy sample composed ofcadmium and the unknown metal, dissolved, and diluted it to exactly 100.0 mL in avolumetric flask. A 20.00-mL aliquot was taken and titrated this using 22.82 mL of 0.05000M EDTA. In a second 20.00-mL aliquot, the Cd was masked through the addition of HCN/NaCN buffer.The titration of the unknown metal in the aliquot required 15.13 mL of EDTA.MW: Cd (112.411 g/mol) a. Calculate the moles of Cd and the moles of unknown metal in the 20.00-mL aliquot.b. Calculate the moles of Cd and the moles of unknown metal in the sample.arrow_forward
- A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe2O3 (aq) to elemental iron: I. Enough sulfur trioxide gas was bubbled to Fe2O3 aqueous suspension to completely yield ferric sulfate. II. Then, 5.00 M nitric acid was added to ferric sulfate yielding an aqueous solution of ferric nitrate. III. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron ----- a. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, l, g).(CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express final answers in 3 significant figures. c. High-concentration HCl is supposed to be added at the last part of the procedure. Briefly state its purpose.arrow_forward(TOPIC: Gravimetry multi-component analysis) A 0.8612-g sample of a mixture of sodium bromide, sodium iodide, and sodium nitrate is analyzed by adding silver nitrate and precipitating a 1.0186-g mixture of silver bromide and silver iodide. The precipitate is then heated in a stream of chlorine gas, which converts it to 0.7125 g of silver chloride. Calculate the %w/w nitrate in the sample.arrow_forwardIs AgC2H3O2 soluble in water? The solubility rules are leading me to believe it is, given Ag is a cation and all cations are soluble when combined with C2H3O2. Is this assumption correct?arrow_forward
- Why is phthalic acid soluble in water and what type of IMFs are involved in the solubility of it in water?arrow_forwardA student measured 20 drops of vinegar and one drop of phenolphthalein solution into a well of her well plate. After she had added 35 drops of NaOH solution to the same well, the well was full, but she had still not reached the titration endpoint. She then took a clean pipet and transferred some of the titration mixture into a second well. She rinsed the pipet with a few drops of distilled water and transferred the rinse water into the titration mixture in the second well. Then she continued adding NaOH solution to both wells until she reached the endpoint in both wells. She then recorded the total number of drops of NaOH solution added to both wells and used it to calculate the data for her vinegar titration. Briefly comment on her procedure and the accuracy of her results.arrow_forwarddescribe how you can prepare 500mL of 0.10 M Fe2O3 (159.69g/mol) from the primary-standard-grade solid.arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning