**Example Calculation Using Stoichiometry****Objective:**Provide an example calculation for converting grams of CO₂ to grams of NaHCO₃ using stoichiometry.**Instructions:**1. **Equation Reference:** - Use Equation 2, which is a net ionic equation for the reaction involving: - Acid, H₃O⁺ (from acetic acid, CH₃COOH in vinegar) - Bicarbonate (from NaHCO₃ in a pill) 2. **Determine the Molar Ratio:** - The calculation will require determining the molar ratio from the given reaction.3. **Consider Spectator Ions:** - Note that Na⁺ (aq) does not appear in the equation as it is a spectator ion.By following these steps, you'll be able to calculate the conversion efficiently using the principles of stoichiometry. **Table 1: Experimental Data**| | Run 1 | Run 2 | Run 3 | Run 4 | Run 5 | Run 6 | Run 7 | Run 8 ||---------------------|-------|-------|-------|-------|-------|-------|-------|-------|| **1. Volume of vinegar (mL)** | 0.00 | 5mL | 10mL | 15mL | 20mL | 25mL | 30mL | 35mL || **2. Volume of water (mL)** | 30mL | 30mL | 25mL | 20mL | 15mL | 10mL | 5mL | 0.00 || **3. Mass of beaker with liquid (g)** | 136.923 | 140.243 | 140.459 | 140.522 | 146.387 | 149.912 | 146.654 | 140.521 || **4. Mass of Alka Seltzer tablet (g)** | 3.243g | 3.253g | 3.249g | 3.250g | 3.249g | 3.249g | 3.246g | 3.249g || **5. Total starting mass (g)** = 3. + 4. | 139.87 | 149.486 | 149.708 | 149.772 | 150.207 | 153.161 | 149.9 | 143.77 || **6. Mass of beaker with liquid after bubbles cease (g)** | 139.17 | 148.714 | 148.784 | 148.843 | 149.29 | 153.679 | 148.396 | 142.87 || **7. Calculated mass of CO₂ lost (produced) (g)** = 5. - 6. | 0.7 | 0.772 | 0.926 | 0.929 | 0.917 | 1.987 | -0.041 | 0.9 || **8. Calculated mass of NaHCO₃ reacted (

8. The chemical equation is CH3COOH + NaHCO3→CH3COONa + CO2+ H2O The stoichiometry ratio of CO2 and…

2. Provide an example calculation for row 8. This requires you to go from g CO2 to g NaHCO3 using stoichiometry. Use equation 2, a net ionic equation for the reaction of acid, H3O+ (from acetic acid, CH3COOOH in vinegar) with the bicarbonate (from NaHCO3 in pill) to determine the molar ratio for your calculation. Note that Na+ (aq) doesn't show up in this equation because it is a spectator ion.

2. Provide an example calculation for row 8. This requires you to go from g CO2 to g NaHCO3 using stoichiometry. Use equation 2, a net ionic equation for the reaction of acid, H3O+ (from acetic acid, CH3COOOH in vinegar) with the bicarbonate (from NaHCO3 in pill) to determine the molar ratio for your calculation. Note that Na+ (aq) doesn't show up in this equation because it is a spectator ion.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

2. Balance the equation below for the reaction of benzil with sodium borohydride. ○ O C-C + BH4 + H₂O HH C-C- | | OH OH + 3. Calculate the number of moles of sodium borohydride and benzil used in the experiment. Considering the balanced equation, which of these is the limiting reactant? B(OH)4
Write the balanced NET ionic equation for the reaction when BaCl₂ and ZnSO₄ are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
You are making 750 mL of a 0.7 M Ca(OH)2 solution. How many moles of Ca(OH)2 will be added? How many grams of Ca(OH)2 will be massed out in a weigh boat?
Sodium hydrogen carbonate (NaHCO,), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI) , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCl through this reaction: HCl(aq) + NaHCO;(aq) → NaCl(aq) + H,O(1) + CO,(g) The CO, gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 100. mL of a 0.048 M HCI solution. What mass of NaHCO, would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits. x10
8. Sodium thiosulfate, Na2S₂O3, is an important reagent for titrations. Its solutions can be standardized by titrating the iodine released when a weighed amount of potassium hydrogen iodate, KH(IO3)2 (389.912 g/mol), is allowed to react with excess potassium iodide in acidic solutions. The net ionic equations are: production of iodine from KH(IO3)2: IO3¯¯ +5 I¯¯+ 6H* → 3 1₂ + 3 H₂O 1₂+2 S₂03² → 2 I¯+S406²- 2- titration of iodine: What is the molarity of a sodium thiosulfate solution if 39.66 mL are required to titrate the iodine released from 0.1022 g of KH(IO3)2?
In the laboratory you are given the task of separating Ca2+ and Co2+ ions in aqueous solution.For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. fill in the blank 1 HCl 2. fill in the blank 3 K2CO3 3. fill in the blank 5 Na2S
In the laboratory you are given the task of separating Ca2+ and Co2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES |1. K2S |2. Na,SO4 3. NaBr
Write the balanced NET ionic equation for the reaction when NH₄Br and Pb(NO₃)₂ are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
Sodium hydrogen carbonate (NaHCO,), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI) , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCl through this reaction: HCl(aq) + NaHCO,(aq) → NaCl(aq) + H,O(1) + CO,(g) The CO, gas produced is what makes you burp after drinking the solution. olo Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 150. mL of a 0.086 M HCl solution. What mass of NaHCO, would Ar he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits. Ox10
Consider the chemical reaction 4 K(s) + O2(g) ──> 2 K2O(s) The molar mass of K is 39.10g/mol, and that of O2 is 32.00g/mol. Without performing any calculations, pick the conditions under which potassium is the limiting reagent and explain your reasoning. 170g K, 31g O2 36g K, 2.5g O2 365kg K, 28kg O2 1.5g K, 0.38g O2
A Carbon dioxide dissolves in water to produce carbonic acid (H;CO;). Under normal atmospheric conditions, the total amount of carbonic acid (in all forms) in water is 1.2 x 10° M. Which is the correct mass balance equation for carbonate? [H;CO3] = [HC05]+ [co5²] Equation 2: [H+]= [0H-]+ [HCO5]+ 2 × [co;?] 1.2 x 10 -8 = [H2CO3:] + [HCO5]+ [cO5²] 1.2 x 10-8 = [OH-]+ [HcO5]+ 2 x [co5?] Equation 5: 1.2 x 10 - = [H¿CO3] + [HCO5]+ 2 × [co;°] Equation 1: Equation 3: Equation 4: What is the predominant form of the triprotic acid, citric acid, at pH 6.2? Answer options: H;A, H;A', HA?, A Calculate cua and a,. for acetic acid in a solution that has a pH of 5.32. Answer options: 0.05 and 0.95; 0.21 and 0.79; 0.56 and 0.44; 0.72 and 0.28
Strong acid-base reactions are a subcategory of double displacement reactions. The hydrogen ion of the acid "switches places" with the cation of the base, while the hydroxide ion of the base "switches places" with the anion of the acid. 1. Write the correct product(s) of the following reaction. Include physical states! Also balance the chemical reaction by writing correct coefficients. NaOH(aq) + HCl(aq) 2. Write the correct product(s) of the following reaction. Include physical states! Also balance the chemical reaction by writing correct coefficients. _NaOH(aq) + H SO (aq) 3. Suppose it takes 10 mL of 0.1 M HCl to neutralize 10 mL of 0.1 M NAOH. (“M" = molarity, which is a unit of concentration.) How many milliliters of 0.1 M H,SO, do you expect will be needed to neutralize 10 mL of 0.1 M NaOH? Explain your choice.