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- ow do the properties of a nonhomogeneous (heterogeneous) mixture differ from those of a solution? Give two examples of nonhomogeneous mixtures.A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O. a.Write the ionic equation for the reaction. b.Write the net ionic equation for the reaction. c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture? d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture? e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)? f.What is the percent by mass of each salt in the mixture1)Please express the normal salt (NaCl) concentration in body fluid into molarity (mM).2) Commercial fuming Sulphuric acid (Oleum-H2S2O6) is 99.9%. solution. Please convert it into molarity.3) Find out the Volume (dm3) of product (gas) at RTP when 0.58 M, 150 mL NaOH (aq.) reacts with 350 mL, 0.25 NH4Cl.4) The above reaction has the product Ammonia, which when dissolved in 650 mL ethanol makes an alkaline ethanolic solution. Find its molarity (M) 5) Calculate the adult dose as per the BW of the baby. (Child dose-50 mg and the BW of the baby is 48 lb (British pound) (1lb=0.453 Kg)
- The organic base, tris-(hydroxymethyl)aminomethane (or simply TRIS or THAM) is an excellent primary standard. A 0.2486 g sample of the primary standard grad TRIS, (CH2OH)3CNH2 (M.M. = 121.14) was dissolved in distilled water and required 24.88 mL of a hydrochloric acid solution. Calculate the molarity of the solutionAlthough other solvents are available, dichloromethane(CH₂Cl₂) is still often used to “decaffeinate” drinks because thesolubility of caffeine in CH₂Cl₂ is 8.35 times that in water.(a) A 100.0-mL sample of cola containing 10.0 mg of caffeine is extracted with 60.0 mL of CH₂Cl₂. What mass of caffeine re-mains in the aqueous phase? (b) A second identical cola sampleis extracted with two successive 30.0-mL portions of CH₂Cl₂.What mass of caffeine remains in the aqueous phase after each extraction? (c) Which approach extracts more caffeine?What volume of 0.08892 M HNO3 is required to react completely with 0.352 g of K2HPO4 (aq)? The balanced chem. eq. is: 2HNO3 (aq) + K2HPO (aq) = H3PO4 (aq) + 2KNO3 (aq)
- 50.00 cm3 of a 1.5784 mol.dm-3 solution of potassium hydroxide is transferred to an empty 700.00 cm3 volumetric flask. This flask is made up to the mark with distilled water and then shaken well. The concentration of the potassium hydroxide in this second flask is:25.0mL of a 0.515 M K2S solution is mixed with 30.0 mL of 0.833 M HNO3 acid solution to give the following reaction: K2S(aq) + 2HNO3(aq) → 2KNO3(aq) + H2S(g) H2S is an unwanted by-product in a pulp and paper industry. To capture H2S gas, it is bubbled through a NaOH solution to produce Na2S with a yield of 94%. H2S(g) + 2NaOH (aq) → Na2S (aq) + 2H2O(l) The mass of H2S(g) that was processed (in kg) if 10.76 kg of Na2S was collected is1. A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer? 2. Data in the table below were collected at 25°C for the following reaction:2 I–(aq) + S2O82–(aq) I2 (aq) + 2 SO42-(aq) a) Determine the rate law for the reaction. b) Calculate the rate constant, giving the correct units for k.
- The calcium (AW= 40.08 g/mol) from a sample of limestone weighing 607.4 mg was precipitated as calcium oxalate hydrate (CaC204.H20, FW 146.12 g/mol) and ignited to calcium carbonate (CaCO3, FW= 100.09 g/mol) weighing 246.7 mg. (c) If the precipitate had been ignited at a higher temperature giving calcium oxide (CaO, FW= 56.08 g/mol), what would be its weight?You have a container of 17.42 M conc. acetic acid (CH3COOH(aq)) with density 1.05 g/mL, find the molality of a 150ml sample of the solution. molality = moles solute/Kg solvent moles solute = (0.150 L)(17.42 mol/L) = 2.613 mol CH3COOH molar mass of CH3COOH = 60.06 g/mol grams of solution = (150mL)(1.05 g/mL) = 157.5 g solution grams of solute = (2.613 mol)(60.06 g/mol) = 156.9 g CH3COOH so the total grams of water in this solution would be: g H2O = g solution - g CH3COOH = 157.5g - 156.9 g = 0.6g H2O 0.6g H2O = 0.0006 Kg H2O so molality = (2.613 mol CH3COOH) /(0.0006 kg H2O) = 4355 molal this seems rather high to me but if its 'concentrated' acetic acid, I know that you can get it to about 98% as glacial acetic acid so perhaps there is 4355 moles of acetic acid per kg of water. Did I do this correctly? I know that typically the solvent is the larger component of a solution but the fact that it gives me CH3COOH(aq) would imply that H2O is the solvent still in this situation, I have…A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.