B. The number of moles ef NaOH is multiplied to the molar concentration ofNAOH.C. The number of moles of Al(NOs is multiplied to the molar mass of NaOH.D. The number of moles of AI(NO)s is added to the molat concentration af NaOH.2. P1 NaL.7. Which steps are helpful in solving problems on chemical reactions insolution? L. The chemical equation must be balanced.II. Find the number of moless one mibatance.3. CII. Relate the number of moles te the stoichiometrically equivalent numberof moles of another subatance.IV. Convert to the desired unit.C. I, & IIID. I, II, III & IVAl& IIB. I, I1 & IIFor numbers 8-10 (3pts) Show your solution to the following and box youranswer. A soda mint tablet contains NaHCO, as an antacid. One tabletrequires 30.5 mL of 0.135 M HCI for complete reaction. Determine thenumber of grams of NaHCo, that one tablet contains. The chemical equationfor the reaction is:NaHCO, (s) + HCI (aq) - NaCl (aq) + CO2 (g) + H2O (1)IV. ReflectionNow that you have learned the basic stoichiometry calculation for reactionin the solution, how can you apply this principle of stoichiometry in real life?V. Answer KeyActivity 1:1. Pmole NaOH = 300 mb-NaOH 0.150 mole NaOH- 0.045 mole(1000 mt-NaoiPmole Fe(OH)3 - 0.045 mele NAOH 1mole Fe(OH), J-0.015 mole3 moles-NaH7g Fe(OH)3-0.045 mele Fe(OH 106.84 g FelOHI, - 1.60 g1 mele FefOH)a12 Bernie Fabela Protacio Jr.Guide Questions:1. How can you lift an ice cube, using only one teothpick?2. Based on the activity, discuss why you can lift the ice cube using atoothpick.Activity 2Directions: Read and understand the given background information aboveand answer the guide questions. Write your answer on a separatesheet of paper.1. Why do ionie compounds like sodium chloride has greater effect on thecolligative properties of solution?2. Describe the effect of electrolyte and nonelectrolyte solutes in freezingpoint depression.3. NaCl is an ionic compound, what effect would it have on the boiling pointof water?IV. ReflectionWhy ice cream vendors used crushed ice sprinkled with salt around the metalcanister that contain ice cream?VI.ReferencesEmil F. Soriano, Celente Joan C. Santisteban, and Erla Rhysa R. Elauria.Chemistry for the New MilleaniumMarissa F. Ayson, Rebecca S. De Borja. General Chemistry 2Whitten, Davis, Peck, and Stanley. General ChemistryTeaching Guide for Senior High School published by the Commission on HigherEducation, 2016.2021 Clutch Learning, Inc.Edit

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solution? 1. The chemical equation must be balanced. II. Find the number of moles one mubatance. II. Relate the number of moles te the stoichiometrically equivalent of moles of another subatance. IV. Convert to the desired unit

solution? 1. The chemical equation must be balanced. II. Find the number of moles one mubatance. II. Relate the number of moles te the stoichiometrically equivalent of moles of another subatance. IV. Convert to the desired unit

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter11: Stoichiometry

Section: Chapter Questions

Problem 108A: Apply Students conducted a lab to investigate limiting and excess reactants. The students added...

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When yeast is added to a solution of glucose or fructose, the sugars are said to undergo fermentation, and ethyl alcohol is produced. :math>C6H12O6(aq)2C2H5OH(aq)+2CO2(g) is is the reaction by which wines arc produced from grape juice. Calculate the mass of ethyl alcohol, C2H5OH. Produced when 5.25 g of glucose, C6H12O6, undergoes this reaction.
In the reaction CaCl2+Na2CO3CaCO3+2NaCl, if 0.5mole of NaCl is to be formed, then: a. 1mole of Na2CO3 is needed. b. 0.5mole of CaCO3 is also formed. c. 0.5mole of Na2CO3 is needed. d. 0.25mole of CaCl2 is needed.
The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride ¡s very insoluble in water, and by adding a slight excess of silver nitrate, it is possible to effectively remove all chloride ion from the sample. :math>Ag+(aq)+Cl+(aq)AgCl(s) ppose a 1.054-g sample is known to contain 10.3% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample? What mass of silver chloride will be obtained?
A common method for determining how much chloride ion is present in a sample is to precipitate the chloride from an aqueous solution of the sample with silver nitrate solution and then to weigh the silver chloride that results. The balanced net ionic reaction is :math>Ag+(aq)+Cl(aq)AgCl(s) ppose a 5.45-g sample of pure sodium chloride is dissolved in water and is then treated with a solution containing 1.15 g of silver nitrate. Will this quantity of silver nitrate be capable of precipitating all the chloride ion from the sodium chloride sample?
The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2O
A weighed sample of a metal is added to liquid bromine and allowed to react completely. The product substance is then separated from any leftover reactants and weighed. This experiment is repeated with several masses of the metal but with the same volume of bromine. This graph indicates the results. Explain why the graph has the shape that it does.
Apply Students conducted a lab to investigate limiting and excess reactants. The students added different volumes of sodium phosphate solution (Na3PO4) to a beaker. They then added a constant volume of cobalt(ll) nitrate solution (CO(NO3)2) stirred the contents, and allowed the beakers to sit overnight. The next day, each beaker had a purple precipitate at the bottom. The students decanted the supernatant from each beaker, divided it into two samples, and added one drop Of sodium phosphate solution to one sample and one drop of cobalt(ll) nitrate solution to the second sample. Their results are shown in Table 11.5. a. Write a balanced chemical equation for the reaction. b. Based on the results, identify the limiting reactant and the excess reactant for each trial.
Many over-the-counter antacid tablets are now formulated using calcium carbonate as die active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting die stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a burp). Write die balanced chemical equation for this process.
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4-89 If 7.0 kg of is added to 11.0 kg of to form which reactant is in excess?