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12 Nov 2019
ngs AaBbCcDdEe AaBbCcDdEe A Normal You need to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. You have a 0.1421 M standard solution. You take a 25.00 mL sample of the original acid solution and dilute it to 250.0 ml. You then take a 10.00 mL sample of the dilute acid solution and titrate it with the standard solution. You need 18.41 mL of the standard solution to reach the endpoint. What is the concentration of the original acid solution? 1. 2. How many grams of 02(g) are needed to completely burn 62.1 g of C3H8(8)? 3. In the following reaction, 451.4 g of lead reacts with excess oxygen forming 391.8 g of lead(II) oxide. Calculate the percent yield of the reaction. 2Pb(s)+02(g) â 2Pb09(s) 4. A) The active ingredient in a zinc nutritional supplement is ZnSO4-7H20 (molar mass- 287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these ten tablets was 11.190 g. A 1.538 g sample of the finely ground tablets was dissolved in an acidic solution. The solution was neutralized with ammonia and subsequently warmed in a water bath. Addition of (NH4)3PO4 to the solution resulted in the precipitation of ZnNH4PO4. The precipitate was filtered and dried, then ignited to produce 0.208 g of Zn2P207 (molar mass -304.76 g/mol). What is the mass percent of ZnSO4.7H20 in each tablet? B) What is the average mass of the active ingredient ZnSO4-7H20 and inactive filler in each tablet?
ngs AaBbCcDdEe AaBbCcDdEe A Normal You need to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. You have a 0.1421 M standard solution. You take a 25.00 mL sample of the original acid solution and dilute it to 250.0 ml. You then take a 10.00 mL sample of the dilute acid solution and titrate it with the standard solution. You need 18.41 mL of the standard solution to reach the endpoint. What is the concentration of the original acid solution? 1. 2. How many grams of 02(g) are needed to completely burn 62.1 g of C3H8(8)? 3. In the following reaction, 451.4 g of lead reacts with excess oxygen forming 391.8 g of lead(II) oxide. Calculate the percent yield of the reaction. 2Pb(s)+02(g) â 2Pb09(s) 4. A) The active ingredient in a zinc nutritional supplement is ZnSO4-7H20 (molar mass- 287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these ten tablets was 11.190 g. A 1.538 g sample of the finely ground tablets was dissolved in an acidic solution. The solution was neutralized with ammonia and subsequently warmed in a water bath. Addition of (NH4)3PO4 to the solution resulted in the precipitation of ZnNH4PO4. The precipitate was filtered and dried, then ignited to produce 0.208 g of Zn2P207 (molar mass -304.76 g/mol). What is the mass percent of ZnSO4.7H20 in each tablet? B) What is the average mass of the active ingredient ZnSO4-7H20 and inactive filler in each tablet?
Sixta KovacekLv2
2 Feb 2019