Compound |
Active ingredient |
Salt substitute | KCl |
Sugar | sucrose |
Salt Petre | KNO3 |
Vitamin C | ascorbic acid |
Cornstarch | Cornstarch |
Tums | CaCO3 |
what are their flame test?
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Compound Active ingredient Salt substitute KCl Sugar sucrose Salt Petre KNO3 Vitamin C ascorbic acid Cornstarch...
What are the flame test results for each of the compounds listed above in top image in the table? Experiment 16 involves determining the identity of 6 unknown household products. Available tests: 1: Solubility in water 2: pH 3: AgNO3 (aq) 4: PbNO3 (aq) 5: BaCl2 (aq) 6: 1M HCI (aq) 7: TM NaOH (aq) 8: Iodine 9: Acetic acid (aq) 10: Flame test Complete the required portions of the table in blue, and any number of additional experiments in...
Ascorbic acid or Vitamin C is a simple compound with the following chemical formula C6H8O6. Besides being an acid, it is also a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, a good oxidizing agent based on the following chemical equation: Br2 (aq) + C6H8O6 (aq) --> 2HBr (aq) + C6H6O6 (aq) Suppose a 1.00-g “chewable” vitamin C tablet requires 27.85 mL of 0.102 M...
Ascorbic acid or Vitamin C is a simple compound with the following chemical formula C6H8O6. Besides being an acid, it is also a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, a good oxidizing agent based on the following chemical equation: Br2 (aq) + C6H3O6 (aq) → 2HBr (aq) + C6H6O6 (aq) Suppose a 1.00-g “chewable” vitamin C tablet requires 27.85 mL of 0.102...
Government and industry analysts routinely measure the quantity of ascorbic acid (vitamin C, C6H8O6) in commercial products such as fruit juices and vitamin tablets. The ascorbic acid reacts with excess iodine, and the amount of I2 remaining is determined with sodium thiosulfate (Na2S2O3). It is suspected by the Montreal Fraud Division that a prominent natural foods importer is defrauding his customers by claiming that his vitamin C tablets contain 45% of the active ingredient ascorbic acid. In one analysis, a...
Ascorbic acid also known as Vitamin C, is an organic compound containing C, H and O. The combustion of a 28.1 g sample of ascorbic acid produces 42.1 g CO2 and 11.5 g H2O. Determine the empirical and molecular formula of ascorbic acid. The molar mass is 176 g/mol.
Ascorbic acid, or vitamin C (C6H8O6, molar mass = 176 g/mol), is a naturally occurring organic compound with antioxidant properties. A healthy adult’s daily requirement of vitamin C is 70-90 mg. A sweet lime contains 2.81×10−4 mol of ascorbic acid. To determine whether the ascorbic acid in a sweet lime meets the daily requirement, calculate the mass of ascorbic acid in 2.81×10−4 mol of ascorbic acid. Express the mass in grams to three significant figures.
Ascorbic acid, or vitamin C (C6H8O6, molar mass = 176 g/mol), is a naturally occurring organic compound with antioxidant properties. A healthy adult’s daily requirement of vitamin C is 70-90 mg. A sweet lime contains 2.85×10−4 mol of ascorbic acid. To determine whether the ascorbic acid in a sweet lime meets the daily requirement, calculate the mass of ascorbic acid in 2.85×10−4 mol of ascorbic acid. Express the mass in grams to three significant figures.
Vitamin C (ascorbic acid) from foods can be measured by titration with I3-If 29.41 mL of I3- solution are required to react with 0.1970 g of pure ascorbic acid, what is the molarity of the I3- solution? A vitamin C tablet containing ascorbic acid plus inert binder was ground to a powder, and 0.4242 g was titrated by 31.63 mL of I3-. How many moles of ascorbic acid are present in the 0.4242 g sample? Find the weight percent of...
Sample question: diprotic acid 24) Ascorbic acid, H2C6H6O2, a diprotic acid, better known as vitamin C has acid hydrolysis constants of Kal = 7.9 x 10-5 and Ka2 = 1.6 x 10-12 What is the [HC6H6O2-) of a solution labeled "0.10 M Ascorbic Acid"?
16 7-2 Titration Calculations Ascorbic acid (vitamin C) reacts with according to the equation Starch is used as an indicator in the reaction. The end point is marked by the appearance of a deep blue starch-iodine complex when the first fraction of a drop of unreacted remains in the solution. TI (a) Stundurdization: If 29.41 mL of iodine solution is required to react with 0.197 0 g of pure ascorbic acid, what is the molarity of the iodine solution?! (b)...