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 (11th Edition)
- You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4. The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. In terms of Mg(OH)2 content, does the sample product conform to the USP requirement? Justify your answer through calculations.arrow_forwardCa(OH)2(aq)+2HCl(aq)CaCl2(aq)+H2O(l)An aqueous solution of Ca(OH)2with a concentration of 0.209 M was used to titrate 25.00 mL of aqueous HCl. 15.93 mL of the Ca(OH)2was required to reach the endpoint of the titration. A. How many moles of base were required to react completely with the acid in this reaction? _____mol Ca(OH)2 B. How many moles of HCl were present in the original 25.00 mL of acid?______mol HClarrow_forwardA sample of material contains the components NaOH, Na2CO3, NaHCO3 , or possible mixtures of these. Two samples, each weighing 1 .000 gram, are dissolved in water. To one sample phenolphthalein is added and the solution is titrated cold with 1.038 N acid, of which 17.96 ml are required. The other sample is titrated cold with methyl orange as an indicator, and 21.17 ml of the same acid is required. Calculate the percentage of alkalies present.arrow_forward
- Caculate the volume (mL) of 1.0 M potassium carbonate (K₂CO₃) needed to prepare 5.0g of the COPPER pigment. This is where the balanced chemical equation come in. You should be able to relate the moles of pigment to the moles of K₂CO₃, and from that calculate the volume of 1.0 M K₂CO₃ solution needed. Please report your value as XX.X mL (one deicmal point and no units).arrow_forwardThe active ingredient in a certain toilet cleaner that claims to ‘remove lime scale and rust’ is hydrochloric acid of approximate concentration 11.6 mol/L. To analyze this toilet cleaner, a quality control chemist first delivered a 10-mL aliquot of the toilet cleaner into a 250-mL volumetric flask, then made up the diluted solution. She then titrated a 27 mL aliquot of this diluted solution against standard sodium hydroxide solution of concentration 0.1705 mol/L. The expected titre (or volume of the titrant in mL) would be approximately:arrow_forwardA saturated solution of an unknown solid reacted with AgNO3 to give a pale yellow precipitate and also reacted with Pb(NO3)2 to give a white precipitate. Based on only these two results, you can conclude that the unknown solid contains which anion? Write the correct balanced equations for the reaction of the anion with each of these reagents.arrow_forward
- Caustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?arrow_forward1. A 0.3516 g sample of commercial phosphate detergent was ignited at a heat to destroy the organic matter. The residue was taken up in hot HCI which converted P to H3PO4. The phosphate was precipitated as MGNH4PO4.6H2O by addition of Mg+ followed by aqueous NH3. After being filtered and washed, the precipitate was converted to Mg2P2O7 by ignition at 1000 OC. This residue weighed 0.2161 g. Calculate the percent P (30.974) in the sample? Ans 17.11%arrow_forwardA fertilizer railroad car carrying 34,300 gallons of commercialaqueous ammonia (30% ammonia by mass)tips over and spills. The density of the aqueous ammoniasolution is 0.88 g>cm3. What mass of citric acid,C(OH21COOH21CH2COOH22, (which contains three acidicprotons) is required to neutralize the spill? 1 gallon = 3.785 L.arrow_forward
- Hw.1.arrow_forwardA 3650-mg sample containing bromate and bromide was dissolved in sufficient water to give 250.0 mL. After acidification, silver nitrate was added to a 25.00 mL aliquot where the resulting precipitate was filtered, washed and then redissolved in an ammoniacal solution of potassium tetracyanonickelate(II) according to the reaction: Ni(CN), + 2 AgBr) → 2 Ag(CN), + Ni? + 2 Br The liberated nickel ion required 26.73 mL of 0.02089 M EDTA. The bromate ion in a 10.00 mL aliquot was reduced to bromide with As* prior to the addition of silver nitrate. The same procedure was followed and the released nickel ion was titrated with 21.94 mL of the EDTA solution. Calculate the percentage of impurity in the sample. Br (79.904) a. 24.45% b.34.38% c. 41.17% d. 65.62%arrow_forward1. Calcium in a sample solution is determined by atomic absorption spectroscopy (AAS). A stock solution of calcium is prepared by dissolving 1.834 g CaCl, 2H,0 in water and diluting to 1 litre. From this stock solution, the second stock solution is prepared by the dilution factor of 10. Three standard solutions of calcium are prepared from the second stock solution with the following dilution factor: 20 (first standard solution), 10 (second standard solution) and 5 (third standard solution). A blank solution is prepared as well. Absorbance signals of AAS are as follows: 1.5 (blank solution), 10.6 (first standard solution), 20.1 (second standard solution), 38.5 (third standard solution), 29.6 (sample solution). (Molar mass; Ca = 40.00 g mol-, CI = 35.45 g mol-, 0 = 16.00 g mol-', H = 1.00 g mol-1) a. Construct ONE (1) plot that could be used to represent the calibration curve. b. From the plot of Q1a, determine the amount of calcium in parts per million.arrow_forward