The substance to be analyzed – is white, highly soluble in water salt. Interaction with concentrated sulfuric acid leads to evolving of reddish-brown gas with pungent odour. Addition of ammonium oxalate leads to formation of white precipitate, which is insoluble in acetic acid. Diphenylamine reaction turns color of the solution to violet. What kind of salt is this? Ca(NO3) 2 NaNO2 KBrO3 MgCl2
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- Give a list of laboratory apparatus and equipment that are to be utilized for the preparation of 500 mL of 0.2 M K4 Fe (CN) 6. Also give the procedure of preparation.You are assigned an unknown solution that contains Group III cations. To -1 mL of this solution was added 6 M NH3 the solution was agitated to mix well, and a reddish-brown precipitate with a gelatinous solid clinging to the inner walls of the test tube was observed. The solution was centrifuged and the supernatant was tested for completeness of precipitation by adding an additional drop of 6 M NH3. No cloudiness was observed as the drop of reagent diffused through the solution. The supernatant was then carefully decanted into a clean test tube, labeled (1st solution), and saved for further testing later. The precipitate remaining in the test tube was washed with a small amount of water, centrifuged, and the wash decanted and discarded. To the precipitate was added about 10 drops of 6 M NAOH plus ~1 mL H20 and the test tube was vigorously agitated. The resulting suspension was centrifuged and the supernatant liquid was transferred to another clean test tube and clearly labeled (2nd…A 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to CaCO3and MgCO3. The sample weighs 465.0 mg. If the sample had been heated at 900oC where the products are CaO and MgO, what would the mixture of oxides weigh? Show the clear and complete solution
- The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L-1Firstly, What is the final molar concentration of a 500.0ml solution prepared from 15.0 ml of a 12.0 M solution of sulfuric acid? Secondly, solid potassium permanganate and standard laboratory equipment are available. Briefly describe how you prepare 100.0 ml solution of 0.050 M potassium permanganate? Potassium permanganate Mr= 158.03 g mol-1 Thirdly, are methonal (CH3OH) and acetic acid (CH3COOH) expected to be miscible? explain with reasoningUsing the concept of IMFA, account for the difference in boiling point and melting point
- Calculate the saturation indices of this solution. Then classify as: undersaturated, supersaturated, or in equilibrium. Why? Saturation state with respect to: “Amakinite” (Fe(OH)2) [Fe2+] = 0.1 mM; [OH-] = 0.0001 mM1.1 WHEN A FEW DROPS OF BARIUM CHLORIDE SOLUTION ARE ADDED TO DILUTE SODIUM SULPHATE SOLUTION , A WHITE PRECIPITATE FORMS. a) Write chemical equations to show the dissociation of barium chloride and sodium sulphate in aqueous solution. b) Name and give the formula of the white precipitate. 1.2 Diethyl ether (C2H5)20 vaporizes easily at room temperature if the vapour exerts a pressure of 250 mmHg in a flask at 28 degree celsuis , what is the density of the vapour? 1.3 How many electrons , protons and protons are there in carbon-13 , 13C 1.4 What is the trend in ionization energy when proceeding down a group in the periodic table . Rationalize this trend 1.5 If you dilute 30.0 mL of 2.50 M hydrochloric acid to 500 mL ,what is the molar concerntration of the dilute acid?Why is phthalic acid soluble in water and what type of IMFs are involved in the solubility of it in water?
- Describe preparation of 400. mL of a solution that is 0.0500 M in I2, starting with solid MgI2.M is a cation which exists as a nitrate compound in an aqueous solution. Part of this solution is separated andH2S gas is sent. Then a black precipitate is given. Next, another part of this M's nitrate solution is separated.When NaOH is added, white precipitate is given. With excess NaOH, white precipitate dissolve and givecolourless solution. What could be the cation?(b) Using appropriate chemical reactions for illustration, show how calcium present as the dissolved HCO3- salt in water is easier to remove than other forms of hardness, such as dissolved CaCl2. (c) A water has the following analysis: mg/l mg/l Na+ - 20 Cl- - 40 K+ - 30 HCO3- - 67 Ca2+ - 5 CO32- - 0 Mg2+ - 10 SO42- - 5 Sr2+ -2 NO3- - 10 What is the total hardness, carbonate hardness and noncarbonated hardness in mg/l as CaCO3.