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The thiourea (NH2)2CS in a 1.600 g sample of an unknown organic material was extracted into a dilute acid solution and was titrated with 42.50 mL of 0.0010 M Hg2+.
Equation:
4 (NH2)2CS + Hg2+ → [(NH2)2CS]4Hg2+
Find the percentage thiourea present in the sample.
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- 7. A student performed an acid-base titration in the lab and recorded the results as shown below. Look very carefully at the results and answer the questions which follow. 演定結果 Nasco +2HC1 →Naclt Ca t H20 試験 流定 終結演定管讀數(cm) 開始演定管讀數(em) 所需演定劑的體積 (cm) 15.40 27.40 15,40 12.00 34.40 27.40 12,00 36 12.30 (1.5 1200 1200 tll5 3. 所間滴定劑的平均體積- 標 0.025/M 25 f 2010 (a) Why do we perform acid-base titrations in our labs? (b) In the titration performed by the student, what was the net ionic equation for the chemical reaction occurring? (c) List all the wrong things that the student did when writing the report on his titration experiment. (d) What good thing did this student do?A 500.0-mg sample of waste ground coffee beans used as fertilizer was digested and analyzed for nitrogen using the Kjeldahl method. After digestion, the distilled ammonia was collected in 100 mL of 0.5500 M boric acid. This solution required 19.60 mL of 0.5880 M HCI for titration to the methyl red end point. Calculate the %N in the fertilizer. Prelim Rxn: NH3 + H3BO3 --> NH4: H2BO3 Titration Rxn: NH : H2BO3 + HCI --> H3BO3 CI-In the titration of 25.00 mL of a water sample, it took 20.840 mL of 4.350x 10−3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures) 9.07×10-5 The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures) he total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures)
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