the formula of the substance remaining after heating kio3

22.48 ml of 0.024 M HCl was required to . Glucose reacts with oxygen to produce carbon dioxide and water: \[ C_6H_{12}O_6 (s) + 6 O_2 (g) \rightarrow 6 CO_2 (g) + 6 H_2O (l) \label{3.6.1} \]. nH2O is present. To perform the analysis, you will decompose the potassium chlorate by heating it. Exponential decay formula proof (can skip, involves calculus) Exponential decay problem solving. 4.6 The rate and extent of chemical change. It is a compound containing potassium, oxygen, and chlorine. 4) Determine the mass of 0.0112 mol of Na2CO3. mass of anhydrous MgCl 2 = 23.977 22.347 = 1.630 g 1.630 g MgCl 2 2 2 1 mol MgCl 95.20 MgCl g = 0.01712 mol MgCl 2 2 2 Half Life formula =Substance which has not decayed after time t =initial amount of Substance =Half life of Substance (a) Amount remaining after 60 hours= 0.125 gm (b) Amount remaining after t hours. Lactating women are encouraged to take an additional 40 mg/day in order to assure an adequate supply of Vitamin C in breast milk. Then calculate the number of moles of [Au(CN). AQA Chemistry. : 7758-05-6 Product code : LC19590 Formula : KIO3 Synonyms : iodic acid, potassium salt / potassium iodine oxide / potassium triodate . Using the molar mass of O2 (32.00 g/mol, to four significant figures), we can calculate the number of moles of O2 contained in this mass of O2: \[ mol \, O_2 = 9.07 \times 10^5 \, g \, O_2 \times {1 \, mol \, O_2 \over 32.00 \, g \, O_2} = 2.83 \times 10^4 \, mol \, O_2 \nonumber \]. You will have to heat your sample of potassium chlorate at least twice. Why? To compare your results for the commercial product with those published on the label. Observations (after the addition of both nitric acid and silver nitrate). What mass of potassium chloride residue should theoretically be left over after heating. We use the same general strategy for solving stoichiometric calculations as in the preceding example. If so, why might they do this? After 12.3 y, half of the sample will have decayed from hydrogen-3 to helium-3 by emitting a beta particle, so that only 50.0 g of the original tritium remains. From Roberts, Hollenberg, and Postman, General Chemistry in the Laboratory. Thanks! In Part A you will be performing several mass measurements. To calculate the quantities of compounds produced or consumed in a chemical reaction. However, all unused $\ce{KIO3}$ (after finishing parts A-C) must go in a waste container for disposal. The history of Vitamin C revolves around the history of the human disease scurvy, probably the first human illness to be recognized as a deficiency disease. As per the activity of radioactive substance formula, the average number of radioactive decays per unit time or the change in the number of radioactive nuclei present is given as: A = - dN/ dt. Discrepancies between the two values are attributed to rounding errors resulting from using stepwise calculations in steps 13. An elementary entity is the smallest amount of a substance that can exist. To experimentally determine the mass percent of oxygen in the compound potassium chlorate ( KClO 3) via the thermal decomposition of a sample of potassium chlorate. All these questions can be answered using the concepts of the mole, molar and formula masses, and solution concentrations, along with the coefficients in the appropriate balanced chemical equation. Namrata Das. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. NH4N03 is added to the water in the calorimeter. This table lists a few countries with the potassium compound . As the name suggested, chemical formula of hypo solution is Na2S2O3. Some of the potassium chloride product splattered out of the crucible during the heating process. Converting amounts of substances to molesand vice versais the key to all stoichiometry problems, whether the amounts are given in units of mass (grams or kilograms), weight (pounds or tons), or volume (liters or gallons). from NaHSO3 reduce KIO3 to form iodide anions (I-), which further react with KIO3 to form iodine (I2). Legal. Question #fee47 Question #c5c15 Question #19eb9 Question #e2ea2 Question #bc751 Question #e2ea6 . Even though 2 mol of H2 are needed to react with each mole of O2, the molar mass of H2 is so much smaller than that of O2 that only a relatively small mass of H2 is needed compared to the mass of O2. At a 2011 market price of over $1400 per troy ounce (31.10 g), this amount of gold is worth $1170. This will be provided by adding solid potassium iodide, $\ce{KI}$ (s), to the reaction mixture. Oxygen is the limiting reactant. As the $\ce{KIO3}$ solution is added, you will see a dark blue (or sometimes yellow or black depending on the color of your sample) color start to form as the endpoint is approached. From this data, the experimental mass percent of oxygen in potassium chlorate will be determined: \[\text{Mass Percent of Oxygen (experimental)} = \frac{ \text{Mass of Oxygen Released}}{ \text{Mass of Potassium Chlorate Used}} \times 100\]. Only if you know the approximate end-point of a titration should you add titrant faster, but when you come within a few milliliters of the endpoint you should begin to slow down and add titrant dropwise. The large cylinder in the middle contains the oxygen and hydrogen that fueled the shuttles main engine. Resultant death was common. The molar mass of H2 (2.016 g/mol) allows us to calculate the corresponding mass of H2: \[mass \, of \, H_2 = 5.66 \times 10^4 \, mol \, H_2 \times {2.016 \, g \, H_2 \over mol \, H_2} = 1.14 \times 10^5 \, g \, H_2 \nonumber \]. The mass of water is found by weighing before and after heating. After the NH4N03 has dissolved, the temperature of the water is 16.90C. - iodine (as KI or KIO3) WASTE DISPOSAL: You may pour the blue colored titrated solutions into the sink. Overshooting an end-point by even one drop is often cause for having to repeat an entire titration. 22.4 cm3 of the acid was required. Oferta indywidualna; Kontakt; the formula of the substance remaining after heating kio3 Strona gwna / . Add some distilled water to your crucible and. Explain how your observations in the table above verify that the residue in your crucible after heating is potassium chloride. Table 1: Vitamin C content of some foodstuffs. the observed rate of decay depends on the amount of substance you have. Calculate the enthalpy change for the dissolution of ammonium nitrate in units ofkJ/mol. Both the time of death and the chemical processes that take place after a person dies are of great interest to an investigator. We need to know two things in order to calculate the numeric value of the equilibrium constant: the balanced equation for the reaction system, including the physical states of each species. This reaction takes place at a temperature of 560-650C. Write a balanced chemical equation for the following reaction, identifying the phase of each substance. &= 0 .132\: \cancel{mol\: Au} \left( \dfrac{196 .97\: g\: Au} {1\: \cancel{mol\: Au}} \right) = 26 .0\: g\: Au \end{align}\). 10 NaHso3+4kIo3-----5Na2s2o5+2I2+3H2so4+2k2so4+2H2o. Use your data to determine the experimental mass percent of oxygen in $\ce{KClO3}$. By heating the mixture, you are raising the energy levels of the . Which of the following sources of error could be used to explain this discrepancy (circle one)? Explain below. You can manipulate this formula if you want to find the change in the amount of heat instead of the specific heat. The amount of substance (n) means the number of particles or elementary entities in a sample. In this titration, potassium iodate, KIO3, is used as an oxidizing agent. Add titrant from the buret dropwise, swirling between drops to determine if a color change has occurred. 2. 5. Mass of sample and container after third heating 23.977 g (a) Explain why the student can correctly conclude that the hydrate was heated a sufficient number of times . How do you account for any discrepancies? With juices it sometimes takes a little longer for the blue color to fade, in which case the endpoint is where the color is permanent. Swirl to thoroughly mix reagents. T = time taken for the whole activity to complete Refilling the buret in the middle of a trial introduces more error than is generally acceptable for analytical work. Dilute the solution to 250 mL with . Throughout your scientific careers you will probably be expected to perform titrations; it is important that you learn proper technique. Because the amount of oxygen is given in tons rather than grams, however, we also need to convert tons to units of mass in grams. Using molar masses along with the known formula of potassium chlorate, calculate the theoretical mass percent of oxygen in $\ce{KClO3}$. Label them tube #1, tube #2 and tube # 3. b) Write a balanced equation for the reaction. It is not necessary that you weigh out the exact mass you calculated, so long as you record the actual mass of ascorbic acid added in each trial for your final calculations. votality. B Because the coefficients of gold and the [Au(CN)2] ion are the same in the balanced chemical equation, assuming that Zn(s) is present in excess, the number of moles of gold produced is the same as the number of moles of [Au(CN)2] (i.e., 0.132 mol of Au). Legal. (This information is crucial to the design of nonpolluting and efficient automobile engines.) What can you conclude about the labeling of this product or reference value? Do not use another container to transfer the ascorbic acid as any loss would result in a serious systematic error. This amount of gaseous carbon dioxide occupies an enormous volumemore than 33 L. Similar methods can be used to calculate the amount of oxygen consumed or the amount of water produced. From the mole ratio in the balanced chemical equation, determine the number of moles of hydrogen required. ( for ionic compound it is better to use the term 'unit' Record the mass added in each trial to three decimal places in your data table. A The equation is balanced as written; proceed to the stoichiometric calculation. Preliminary Calculations Involving the "Clock" Reaction Using the dilution formula, the concentration of S2O3 2-in the mixture is 1.2 x10-3 M . the formula of the substance remaining after heating kio3 | mycie, pielgnacja wntrza, zabezpieczanie lakieru, renowacja szyb i lamp. Stoichiometry is a collective term for the quantitative relationships between the masses, the numbers of moles, and the numbers of particles (atoms, molecules, and ions) of the reactants and the products in a balanced chemical equation. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Given: chemical equation and molarity and volume of reactant. The equation is y=3e2x y = 3 e 2 x. Exponential growth and decay often involve very large or very small numbers. I3- is immediately reduced back to I- by any remaining HSO3-. All compounds consist of elements chemically . Use the back of this sheet if necessary. The . Both of these reactions require acidic conditions and so dilute hydrochloric acid, $\ce{HCl}$ (aq), will be added to the reaction mixture. Briefly describe the sample you chose to examine and how you prepared it for analysis. 16) a) What of particles (atoms , molecules, cations, aNons, or canons anions) occupy the lattice in each of the crystalline solids given below. 3. In Part B of this lab, the residue left after heating will be qualitatively analyzed in order to demonstrate that it is chemically different from the initial potassium chlorate sample. Then weigh and record the mass of the crucible, lid, plus the residue that remains. What is the value of n? Here's a video of the reaction: Answer link. According to the balanced chemical equation, 6 mol of CO2 is produced per mole of glucose; the mole ratio of CO2 to glucose is therefore 6:1. - an antikaking agent. To do this, the potassium chlorate must be heated to temperatures greater 400 C, causing it to thermally decompose into potassium chloride and free oxygen: \[\ce{2KClO3 (s) ->[heat] 2KCl(s) + 3O2 (g)}\], \[\text{Potassium Chlorate} \ce{->} \text{Potassium Chloride} + \text{Oxygen}\]. In performing a titration generally an indicator that changes color is added to a solution to be titrated (although modern instruments can now perform titrations automatically by spectroscopically monitoring the absorbance). Hint: you will need to use the approximate $\ce{KIO3}$ molarity given in the lab instructions and the mole ratio you determined in the prior problem. Remember that your buret holds a maximum of 50.00 mL of solution and ideally you would like to use between 25-35 mL of solution for each titration (enough to get an accurate measurement, but not more than the buret holds). Negative - ordering effect of ion on solvent is greater than the entropy increase of the crystal (highly ordered) lattice breaking down. When the vitamin C (ascorbic acid) is completely oxidized, the iodine, $\ce{I2}$ (aq), will begin to build up and will react with the iodide ions, $\ce{I^-}$ (aq), already present to form a highly colored blue $\ce{I3^-}$-starch complex, indicating the endpoint of our titration. Proper use of a buret is critical to performing accurate titrations. Use of the substance/mixture : Pharmaceutical product: component Veterinary medicine If a typical 2 oz candy bar contains the equivalent of 45.3 g of glucose and the glucose is completely converted to carbon dioxide during the exam, how many grams of carbon dioxide will you produce and exhale into the exam room? This is the correct number of moles of water released from this sample. Now the newly formed iodide ions are oxidized to iodine by reaction with more iodate ions. How long must the sample be heated the second time? To qualitatively demonstrate that the residue resulting from the decomposition of potassium chlorate is potassium chloride. In 1934, Rechstein worked out a simple, inexpensive, four-step process for synthesizing ascorbic acid from glucose. Upon analysis of this mixture, would you obtain a larger or smaller mass percent of oxygen than you would for an equal mass of pure sample of potassium chlorate (circle one)? Filterate- water+nitre Residue - sulphur+charcoal 3) Perform evaporation on the filterate. The formula of the substance remaining after heating KIO, heat 7. This can be given in units of %RDA, mg/g, mg/mL, mg/serving, or %RDA per serving. While adding the $\ce{KIO3}$ swirl the flask to remove the color. Assigning a coefficient of 2 to both H2O and H2 gives the balanced chemical equation: \[ 2 H_2 (g) + O_2 (g) \rightarrow 2 H_2O (g) \nonumber \]. Your final calculated results for each trial of this experiment should differ by less than 0.0005 M. Any trials outside this range should be repeated. In solution I2 reacts with I to form triiodide anions (I3-). Note that the total volume of each solution is 20 mL. A stoichiometric quantity is the amount of product or reactant specified by the coefficients in a balanced chemical equation. To describe these numbers, we often use orders of magnitude. As the $\ce{KIO3}$ solution is added, you will see a dark blue (or sometimes yellow) color start to form as the endpoint is approached. Positive - increase in entropy because the solvent hydrogen bonding is disrupted. Clean both crucibles and their lids (obtained from the stockroom) by thoroughly rinsing with distilled water then drying as completely as possible with a paper towel. From the balanced chemical equation, obtain the number of moles of another substance (B) from the number of moles of substance A using the appropriate mole ratio (the ratio of their coefficients). Calculate the milligrams of ascorbic acid per milliliter of juice. Refill the buret between titrations so you wont go below the last mark. The following steps should be carried out for two separate samples of potassium chlorate. KIO3(s) . Bookmark. Show all your calculations on the back of this sheet. If an average lemon yields 40 mL of juice, and the juice contains 50 mg of Vitamin C per 100 mL of juice, how many lemons would one need to eat to consume the daily dose of Vitamin C recomended by Linus Pauling? Cinnabar, (or Cinnabarite) $HgS$ is the common ore of mercury. . This should be enough $\ce{KIO3}$ for your group for. Show your calculations clearly. Calculate milligrams of ascorbic acid per gram of sample. Both reaction are endothermic - heat must be supplied in order for the reaction to take place. Its symptoms include exhaustion, massive hemorrhaging of flesh and gums, general weakness and diarrhea. A balanced chemical equation gives the identity of the reactants and the products as well as the accurate number of molecules or moles of each that are consumed or produced. Amount remaining after 4 days that is 96 hours=0.012 grams Finding Mols and Masses of Reactants and Products Using Stoichiometric Factors (Mol Ratios): Finding Mols and Masses of Reactants and Products Using Stoichiometric Factors, YouTube(opens in new window) [youtu.be]. Begin your titration. Vitamin C, known chemically as ascorbic acid, is an important component of a healthy diet. Formality. Write the word equation and the balanced formula equation for this decomposition reaction. Chemical Formula of Potassium iodate. When sulphite ions react with potassium iodate, it produces iodide ions. As you become proficient in performing titrations you will get a "feeling" for how much to open the stopcock to deliver just one drop of titrant. . [ Check the balance ] The thermal decomposition of potassium iodate to produce potassium iodide and oxygen. temperature of the solution. unit. If this mass is within 0.050 grams of your mass measurement after the first heating (see step 6), no further heating is necessary and you may begin Part B. Dissolve the solid ascorbic acid in 50-100 mL of deionized water in an Erlenmeyer flask. Repeat any trials that seem to differ significantly from your average. Explain your choice. - sodium chloride (NaCl) Will this container be covered or uncovered while heating? This is how many grams of anhydrous sodium carbonate dissolved. Add approximately 1 gram of potassium chlorate to the crucible. Developed countries use both potassium iodide (KI) and potassium iodate (KIO3) extensively for iodization of refined table salt. Place three medium-sized test tubes in the test tube rack. After another 12.3 y making a total of 24.6 y another half of the remaining tritium will have decayed, leaving 25.0 g of tritium. In Part A of this lab, you will analyze a sample of potassium chlorate to determine the mass percent of oxygen present in it. Clean and rinse three burets once with deionized water and then twice with small (5-10 ml) aliquots of standard $\ce{KIO3}$ from your large beaker. It contains one potassium ,one iodine and three oxygen atoms per After heating, the mass of the anhydrous compound is found to be 3.22 g. Determine the formula of the hydrate and then write out the name of the hydrate. Titration 1. Linus Pauling, winner of both a Nobel Prize in Chemistry and the Nobel Peace Prize, has argued in his book, Vitamin C and the Common Cold, that humans should be consuming around 500 mg of Vitamin C a day (considered by many doctors to be an excessive amount) to help ward off the common cold and prevent cancer. A We first use the information given to write a balanced chemical equation. The density of Potassium iodate. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. The formula of the substance remaining after heating KIO, heat 7. The initial step in solving a problem of this type is to write the balanced chemical equation for the reaction. Clean and rinse a large 600-mL beaker using deionized water. If the first titration requires less than 20 mL of $\ce{KIO3}$, increase the volume of unknown slightly in subsequent trials. Thus, the theoretical mass percent of oxygen in potassium chlorate would be calculated using the expression: \[ \text{Mass Percent of Oxygen (theoretical)} = \frac{3 \times \text{(Molar Mass of O)}}{ \text{Molar Mass of } \ce{KClO3}} \times 100\]. Be especially careful when using the Bunsen burner and handling hot equipment. What will you observe if you obtain a positive test for chloride ions? It was first isolated in 1928 by the Hungarian-born scientist Szent-Gyorgi and structurally characterized by Haworth in 1933. The stoichiometric ratio measures one element (or compound) against another. The test tubes should be thoroughly cleaned and rinsed with distilled water. For example, if a substance reacts with the oxygen in air, then oxygen is in obvious (but unstated) excess. (Note: If your sample is highly colored, you might want to dissolve the KI in the water before adding the mix, so that you can be sure it dissolves). Here, A is the total activity. Sr(NO3)2 (aq) + 2*KIO3 (aq) > 2* KNO3 (aq) + Sr(IO3)2-H2O Because we know the identity of both the reactants and the product, we can write the reaction as follows: \[ H_2 (g) + O_2 (g) \rightarrow H_2O (g) \nonumber \]. As early as 1536, Jacques Cartier, a French explorer, reported the miraculous curative effects of infusions of pine bark and needles used by Native Americans. Separates a substance that changes directly from solid into gaseous state from a mixture. It is seen that in an acidic medium sulphite reduces potassium iodate to iodide. Potassium iodate (KIO3) is an ionic compound. This is a class experiment suitable for students who already have . (which is specified by the big number before a chemical formula), you can find out the theoretical yield by multiplying the number of moles by the Relative atomic mass (Mr) of the product . You will need to calculate in advance how many grams of pure Vitamin C powder (ascorbic acid, $\ce{C6H8O6}$) you will need to do this standardization (this is part of your prelaboratory exercise). 5) Mass of hydrated salt mass of anhydrous salt = mass of water. Repeat any trials that seem to differ significantly from your average. Repeat all steps for your second crucible and second sample of potassium chlorate. Calculate the approximate mass of ascorbic acid you will need and have your instructor initial your calculations on the data sheet. a. The reverse reaction must be suppressed. Inspection shows that it is balanced as written, so the strategy outlined above can be adapted as follows: 1. Add approximately 0.5-0.6 g of $\ce{KI}$, 5-6 mL of 1 M $\ce{HCl}$, and 2-3 drops of 0.5% starch solution to the flask before beginning your titration. Weigh each tablet and determine the average mass of a single tablet. Potassium chlorate is added to tube #1, potassium chloride to tube #2, and the residue to tube #3. Students can therefore evaluate their accuracy in this experiment by comparing their experimental results to the true theoretical value, and by calculating their percent error. A graph showing exponential decay. Explanation: . Remember that most items look exactly the same whether they are hot or cold. It is also called the chemical amount. A sample of NaClO3 is converted by heat to NaCl with a loss of 0.16 g of oxygen. Convert the mass of one substance (substance A) to the corresponding number of moles using its molar mass. $ 26 .0\: \cancel{g\: Au} \times \dfrac{1\: \cancel{troy\: oz}} {31 .10\: \cancel{g}} \times \dfrac{\$1400} {1\: \cancel{troy\: oz\: Au}} = \$1170 $. The empirical formula of compound CXHYOZ is : [Main 2018] (a) (b) (c) (d) 7. . In Part B of this lab, you will analyze the residue in left the "container" in order to experimentally verify its identity. The two reactions we will use in this experiment are: \[\ce{KIO3(aq) + 6 H+(aq) +5 I- (aq) 3 I2(aq) + 3 H2O(l) + K+(aq) } \quad \quad \text{generation of }\ce{I2} \label{1}\], \[\underbrace{\ce{C6H8O6(aq)}}_{\text{vitamin C(ascorbic acid)}}\ce{ + I2(aq) C6H6O6(aq) +2 I- (aq) + 2 H+(aq) } \quad \quad \text{oxidation of vitamin C}\label{2}\]. 3.89 g/cm. Larger Smaller. A suitable method for the determination of vitamin C (C 6 H 8 O 6) is a titration with potassium iodate (KIO 3).Potassium iodate is used as a titrant and is added to an ascorbic acid solution that contains strong acid and potassium iodide (KI). This page titled 10: Vitamin C Analysis (Experiment) is shared under a CC BY-NC license and was authored, remixed, and/or curated by Santa Monica College. Then, once again, allow it to cool to room temperature. Sodium thiosulphate acts as reducing agent an at the same time it undergoes oxidation and release electron. Perform two more trials. Name of Sample Used: ________________________________________________________. When carrying out a reaction in either an industrial setting or a laboratory, it is easier to work with masses of substances than with the numbers of molecules or moles. When sulphite ion is fully consumed, the blue colour by the leftover liberated iodine. The specific gravity of Potassium iodate. If a spill of either chemical occurs, rinse under running water and report the accident to your instructor. Now heat the sample a second time for an additional 6 minutes using a high temperature flame. Calculating Equilibrium Constants. Note: You will need to bring a powdered or liquid drink, health product, fruit samples, or other commercial sample to lab for vitamin C analysis. in aqueous solutions it would be: Water will . Swirl to mix. Then convert the moles of hydrogen to the equivalent mass in tons. 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\newcommand{\Span}{\mathrm{span}}$ $\newcommand{\id}{\mathrm{id}}$ $ \newcommand{\Span}{\mathrm{span}}$ $ \newcommand{\kernel}{\mathrm{null}\,}$ $ \newcommand{\range}{\mathrm{range}\,}$ $ \newcommand{\RealPart}{\mathrm{Re}}$ $ \newcommand{\ImaginaryPart}{\mathrm{Im}}$ $ \newcommand{\Argument}{\mathrm{Arg}}$ $ \newcommand{\norm}[1]{\| #1 \|}$ $ \newcommand{\inner}[2]{\langle #1, #2 \rangle}$ $ \newcommand{\Span}{\mathrm{span}}$$\newcommand{\AA}{\unicode[.8,0]{x212B}}$, Standardization of your $\ce{KIO3}$ solution, Vitamin C Unknown (internal control standard), Fruit juices, foods, health-products, and powdered drink mixes, 9: Evaluating the Cost-Effectiveness of Antacids (Experiment), 11A: The Molecular Weight of Carbon Dioxide (Experiment), Vitamin C: An Important Chemical Substance, Part A: Standardization of your $\ce{KIO3}$ solution, Part B: Vitamin C Unknown (internal control standard), Part C: Fruit juices, foods, health-products, and powdered drink mixes, Pre-laboratory Assignment: Vitamin C Analysis, status page at https://status.libretexts.org, Chili peppers, sweet peppers, parsley, and turnip greens, Citrus juices (oranges, lemons, etc.

the formula of the substance remaining after heating kio3 2023