Classify the given as direct, indirect, or back titration problems. A 50.00-mL sample of a citrus drink requires 17.62 mL of 0.04166 M NaOH to reach the phenolphthalein end point. Express the sample’s acidity as grams of
Classify the given as direct, indirect, or back titration problems.
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A 50.00-mL sample of a citrus drink requires 17.62 mL of 0.04166 M NaOH to reach the phenolphthalein end point. Express the sample’s acidity as grams of citric acid, C6H8O7, per 100 mL. |
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Limestone consists mainly of CaCO3, with traces of iron oxides and other metal oxides. To determine the purity of a limestone, a 0.5413-g sample is dissolved using 10.00 mL of 1.396 M HCl. After heating to expel CO2, the excess HCl was titrated to the phenolphthalein end point, requiring 39.96 mL of 0.1004 M NaOH. Report the sample’s purity as %w/w CaCO3 |
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The concentration of SO2 in air is determined by bubbling a sample of air through a trap that contains H2O2. Oxidation of SO2 by H2O2 results in the formation of H2SO4, which is then determined by titrating with NaOH. In a typical analysis, a 3.5 L sample of air is passed through the peroxide trap and required 10.08 mL of 0.0244 M NaOH to reach the phenolphthalein end point. Calculate the % w/v SO2 in the sample of air. |
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50.25 mL of primary standard K2Cr2O7, dissolved in acid, was treated with excess KI. The liberated iodine required 17.41mL of 0.1321M Na2S2O3 solution for titration. What is the molar concentration of K2Cr2O7? (MM K2Cr2O7 is 294.185 g/mol) |
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A 0.2521-g sample of an unknown weak acid is titrated with 0.1005 M NaOH, requiring 42.68 mL to reach the phenolphthalein end point. Determine the compound’s equivalent weight. |
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