ap chemistry lab manual and syllabus for students elegante

10/19/2022 Page of 115 AP Chemistry Lab Manual Lab Notebook Guidelines QRS lab Qualitative Analysis of the Group III Cations How Much Zinc is in a penny? 11 Predicting Products of Chemical Reactions 12 Redox Titration: The Standardization of Potassium Permanganate .13 The EMF Activity Series .15 Heat of Fusion for Ice 19 Additivity of Heats of Reaction: Hess’s Law .21 Heat of Combustion of a metal-an inquiry based approach 23 VSEPR and Molecular Geometry 25 Formation of a Coordination Complex of Copper (II) 26 Kinetics of a Reaction An Iodine Clock 28 Where did the Crystal Violet go? 30 Chemical Equilibrium: Finding a Constant, Keq or Kc 35 Entropy of a Reaction 37 Catalytic Converter—Hot Copper Catalysis 38 Equilibrium and Le Châtelier's Principle .40 Strong Acid Strong Base Titration 43 Titration of a weak acid 45 Determination of the Ka of Weak Acids 46 Determination of the Ksp of an Ionic Compound 49 Buffer Laptop Palooza 51 Preparation and Properties of Buffer Solutions .53 Corrosion Cells 56 Polyatomic Ions .59 Molecular Geometry 60 Rules of Writing Equations 62 AP Chemistry Syllabus 64 Class Rules .66 Description of Content Covered 67 End of Year Review .70 Solution Practice 79 Redox Practice .80 Thermochemistry: Standard Heats of Formation Worksheet 82 Gas laws practice 83 and Practice worksheet 85 Equilibrium and Entropy Practice 89 Ch 10 questions .92 Chapter 11 Practice 92 Kinetics part I 94 Kinetics part II .97 Accessing Prior Knowledge Acids and Bases .100 pH PRACTICE 101 Ka and Kb practice 102 Titration Curve Practice .103 Chapter 14 and 15 practice: 110 Ksp practice Keep me but put all answers in your notes 112 Electrochem practice 114 10/19/2022 Page of 115 10/19/2022 Page of 115 Lab Notebook Guidelines You must have a composition notebook or the notebook from Chem I as a lab notebook A lab notebook should be used to explain lab procedures, record all lab data, and show how calculations are made You may also use the notebook to discuss the results of an experiment and to explain the theories involved A record of lab work is an important document which will show the quality of the lab work that you have done You may need to show your notebook and your lab reports to the Chemistry Department at a college or university in order to obtain credit for the lab part of an AP Chemistry class As you record information in your notebook, keep in mind that someone who is unfamiliar with your work may be using this notebook to evaluate your lab experience in chemistry When you explain your work, list your data, calculate values and answer questions, be sure that the meaning will be obvious to anyone who reads your notebook Guidelines for the notebook: Write your name and class on the front cover In black or blue ink, number all the right hand pages on the lower right corner if they are not already numbered Save the first pages for a Table of Contents This should be kept current as you proceed Each time you write up a lab, place the title and page numbers where the lab report begins in the Table of Contents Write in ink Use only the right hand pages If you make a mistake, DO NOT ERASE OR SCRIBBLE Just draw ONE LINE through your error, and continue It is expected that some errors will occur A lab notebook is a working document, not a perfect, error-free, polished product Errors should be corrected by drawing one line through the mistake, and then proceeding with the new data Do not use the first person or include personal comments Prelab Instructions: On most every lab you will have prelab instructions If it has you read, read carefully as there will often times be a quiz over that content If there are questions you are supposed to answer, them on a separate sheet of paper and hand them in as your ticket into lab If there is a code word in the procedure or weird instructions be prepared to follow them Some labs will be full write-ups and some will be data and calculations only You must always answer questions if they are in the lab manual You must get your data stamped in your lab notebook before you leave the lab Lab Reports (Lab reports will be worth 50 points) Include the following information in your lab reports Label each section Title – The title should be descriptive Experiment is not a descriptive title Date and lab station – This is the date you performed the experiment and lab station Purpose – A brief statement of what you are attempting to Must be a sentence Procedure – A shortened description of the method you are using You may refer to the lab manual for specific instructions, but you should include a brief statement of the method Do not include lengthy, detailed directions A person who understands chemistry should be able to read this section and know what you are doing Reactions: Write a balanced reaction including states of matter for any reactions If there are no reactions omit this section 10/19/2022 Page of 115 Data- Record all your data directly into your lab notebook on the right-hand pages Organize your data in a neat, orderly form Label all data very clearly Use correct sig figs and always include proper units Underline, use capital letters or use any device you choose to help organize this section well Space things out – don’t try to cram everything on one page A data table must have a label and a title e.g – Table 1: Density Values for Sugar Solutions Calculations and Graphs- You should show how calculations are carried out Give the equation used and show how your values are substituted into it Give the calculated values If graphs are included, make the graphs an appropriate size Label all axes and give each graph a title If experiments are not quantitative, this section may be omitted Conclusions – Make a simple statement concerning what you conclude from the experiment This is not a place to give your opinion of the lab and whether or not it was “fun” It is not your job to review the lab like you would if you saw a movie Experimental error – If there is a known value for something you are doing in lab, calculate the experimental error 10 Error Analysis – What are some specific sources of error, and how they influence the data? Do they make the values obtained larger or smaller than they should be? Which measurement was the least precise? Instrumental error and human error exist in all experiments, and should not be mentioned as a source of error unless they cause a significant fault Significant digits and mistakes in calculations are NOT a valid source of error In writing this section it is sometimes helpful to ask yourself what you would differently if you were to repeat the experiment and wanted to obtain better precision 11 Questions – Answer any questions included in the lab directions Answer in such a way that the meaning of the question is obvious from your answer Reporting Lab Data Graphing Data All graphs should have a descriptive title (“Graph” is not a title) and a label e.g – Graph A: Density of Solutions with Varying Sugar Concentrations Both the vertical and horizontal axes should both have labels and units clearly marked Use a ruler to draw the axes The scales chosen should reflect the precision of the measurements For example, if temperature is known to be ±0.1ºC, you should be able to plot the value this closely Don’t have each block of the graph equal to 10ºC There should be a table in which the data values are listed Don’t put data in a graph unless you have first listed it in a table The controlled or independent variable is placed on the horizontal axis The dependent variable is graphed on the vertical axis There should be an obvious small point on the graph for each experimental value It is not necessary to include the coordinates of each point since they will be in the data table A smooth line should be drawn that lies as close as possible to most of the points Do NOT draw a line connecting one point to the next as in a dot-to-dot drawing If the line is a straight line, use a ruler to draw it If a computer program is used to draw the graph, the rules still apply Accuracy Accuracy is a measure of how close an experimental value is to a value which is accepted as correct The measure of the accuracy of an experimental value is reported as Percent Error 10/19/2022 Page of 115 Experimental  Accepted Accepted Data Tables All data tables must be neatly organized Numbers should be aligned by decimal point Appropriate units must always be used Data should be appropriately spaced out so that there is room for corrections or annotations about the data All data must be in your lab notebook and initialed by the teacher before you leave the lab %error  10/19/2022 Page of 115 QRS lab Reactions and explanations only, no full writeup In this lab, there are three flasks labeled Q, R, and S Each flask contains one of the following solutions: 0.1 M Pb(NO3)2, 0.1 M NaCl, or 0.10 M K2CO3 Two other flasks are labeled X and Y One of these flasks contains 0.1 M AgNO3 and the other contains 0.1 M BaCl2 Mix each of the solutions with each of the other and record all observations For all precipitates which form, you must write a balanced equation and net ionic equation and identify the precipitate You will need to wait until you have identified the solutions to write the equations As you carry out the reactions you must use as little solution as possible Part of your grade is the way in which you are observed performing the reactions Frugality is key You must explain how you reasoned out the solution’s identity 10/19/2022 Page of 115 Qualitative Analysis of the Group III Cations No writeup Only data sheet Discussion A known solution of the Group III cations (Cr3+, Al3+, Fe3+, Mn2+) and an unknown solution containing some combination of ions will be analyzed Group III contains those cations whose hydroxides not precipitate under highly acidic conditions Under basic conditions, however, the Group III cations will precipitate as the hydroxides Cr3+ (aq) + 3OH-(aq) Cr(OH)3(s) Al3+(aq) + 3OH-(aq)  Al(OH)3(s) Fe3+(aq) + 3OH-(aq)  Fe(OH)3(s) Mn2+(aq) + 2OH-(aq)  Mn(OH)2(s) The pH is then raised with NaOH and hydrogen peroxide is added to further oxidize the precipitates The Fe(OH)3 (s) remains the same, the Mn(OH)2(s) becomes MnO2(s), the Cr(OH)3(s) oxidizes to the chromate ion CrO42-(aq) and the Al(OH)3(s) complexes with more hydroxide ion to form Al(OH)4-(aq) MSDS 2M NH4Cl solution 6M Ammonia 6M NaOH 3% H2O2 3M H2SO4 6M HNO3 0.5M KSCN PbO2 6M HC2H3O2 0.1 M Pb(C2H3O2)2 Irritating to body tissues Avoid all body tissue contact Liquid and vapor are strongly irritating to skin, eyes, and mucous membranes Vapor extremely irritating to eyes May cause blindness Toxic by ingestion or inhalation When heated to decomposition, emits toxic fumes of NH3 and NOx Moderately toxic by ingestion and skin absorption Corrosive to body tissues Causes severe eye burns Avoid all body tissue contact Slightly toxic by ingestion or inhalation Irritant to skin, eyes and respiratory tract Avoid prolong body contact Hydrogen peroxide will decompose rapidly when exposed to almost any substance Moderately toxic by ingestion Corrosive to eye, skin, and all other body tissues Avoid all body tissue contact Very considerable heat generated when diluted with water Corrosive; will cause severe damage to eyes, skin and mucous membranes Moderately toxic by ingestion and inhalation Strong oxidizer Avoid contact with acetic acid and readily oxidized substances Slightly toxic by ingestion Irritating to body tissues Avoid all body tissue contact Contact with acids or heat may liberate poisonous hydrogen cyanide gas Moderately toxic by ingestion or inhalation Irritating to body tissues Avoid all body contact Oxidizer Lead and lead compounds are possible carcinogens Substance not considered hazardous However, not all health aspects of this substance have been thoroughly investigated Moderately toxic by ingestion and skin absorption Eye and skin irritant Possible carcinogen Avoid ingestion, inhalation and skin absorption 10/19/2022 Page of 115 Chronic exposure to inorganic lead via inhalation or ingestion can result in accumulation in and damage to the soft tissues and bones Procedure Obtain a Group III known sample which contains all of the ions You will get a Group III unknown solution (which may contain any or all of these cations) after you have completed the known All glassware should be cleaned, rinsed and rinsed with distilled water before starting the lab Step Notes Place 1-2 mL of solution to be tested in a small test tube Add mL of M ammonium chloride solution to the sample in the test tube and stir Add M aqueous ammonia to the sample dropwise until the solution is just barely basic (remove a drop of the solution with a stirring rod and touch the drop to a strip of pH test paper) Add about mL of distilled water to wash the precipitate Mix thoroughly, centrifuge, decant and discard water Add ~ 2mL 6M NaOH to the residue and mix Add 10 drops 3% H2O2 and mix immediately Boil several minutes to remove excess H2O2 If solution is green, add more H2O2 (yellow is okay) Look for separation of precipitate and supernatant Centrifuge, decant and obtain residue for step 6, and decantate for step 12 Do not discard If necessary, recentrifuge decantate until absolutely clear or filter into another test tube Add 1-2 mL 3M H2SO4 to residue Mix Add 5-6 drops 3%H2O2 to hasten the process Mix thoroughly If it doesn’t dissolve, heat for a few minutes until all the solid dissolves Dilute solution to a total of mL with distilled water and divide the solution into parts to be tested for Fe3+ ions in step and Mn2+ ions in step 10 Add 1-2 drops 0.5M KSCN to one test tube from part A blood red solution indicates the presence of Fe3+ ions 10 To the other half of the solution from step 6, add ~ 1mL 6M HNO3 and mix 11 Add solid PbO2 equivalent to 1/10 the volume of the liquid Mix well and Boil for 2-3 minutes and let stand for minutes If Mn2+ ions are present, the solution will turn a pink to dark purple color If test is negative, add another small portion of acid, mix and Boil solution Centrifuge 12 Dilute decantate from step to ~ 4mL with distilled water and divide into two parts to be tested for Al3+ in step 13 and CrO42- in step 14 13 Add ~ 2mL 2M NH4Cl to the first half of decantate from step 12 DO NOT MIX Place in Boiling water for minutes Look closely for a fluffy, translucent solid in the top layer which indicates the presence of Al3+ ions If uncertain 10/19/2022 about the aluminum test, centrifuge If other ions are present, the decantate may not be clear and a halo effect may be seen around the precipitate The iron and manganese hydroxides will spin down first because of the greater densities and the aluminum hydroxide will be on top 14 Add 6M HC2H3O2 to second half of decantate from step until acidic to litmus paper Add 1-2 drops 0.1 M Pb(C2H3O2)2 Let stand for minutes A white or yellow precipitate is a positive test for CrO42- ions Page of 115 10/19/2022 Page 10 of 115 Unknown # Station # Name(s) Presence of Aluminum ion Yes No Presence of Chromium ion Yes No Presence of Iron ion Yes No Presence of Manganese ion Yes No Group III Cation Analysis Al3+, Cr3+, Fe3+, Mn2+ NH4Cl NH4OH Residue Decantate discard Fe(OH)3, Mn(OH)2, Cr(OH)3, Al(OH)3 NaOH(aq) H2O2 Residue Decantate CrO42-, Al(OH)4- H2SO4(aq) H2O2 3+ Fe KSCN Fe(SCN)2+ blood red Mn 2+ HNO3(aq) PbO2 MnO4Pink/purple HC2H3O2 Pb(C2H3O2)2 PbCrO4 yellow or white NH4Cl Al(OH)3 Translucent flecks 10/19/2022 Page 101 of 115 Accessing Prior Knowledge Acids and Bases Define acids and bases from three viewpoints, Arrhenius, Bronsted Lowry and Lewis What the [H+] and [OH-] always multiply together to equal? What pH and pOH always add up to? Write the formulas/names for the follwing: Nitric acid Hydrocyanic acid Chloric acid Acetic acid Hydrobromic acid 10 Sulfurous acid 11 Chlorous acid 12 Boric acid 13 Hydrochloric acid 14 Phosphoric acid 15 Nitrous acid 16 Hydrofluoric acid 17 Perchloric acid 18 Hydroiodic acid 19 Phosphorous acid 20 Carbonic acid 21 Sulfuric acid 22 Formic acid (the formate ion is COOH-) 23 Thiocyanic acid 24 HClO4 25 HCOOH 26 H3PO4 27 HCl 28 H3BO3 29 H2SO4 30 HNO2 31 HI 32 CH3COOH 33 HF 34 H3PO3 35 HCN 36 HClO3 37 H2CO3 38 H2SO3 39 HClO2 40 HNO3 41 HBr 42 H2S2O3 10/19/2022 Page 102 of 115 pH PRACTICE Write the pH of each solution above the [H+]’s pH = -log[H+] Label the “Z” diagram as “Acidic”, “Basic” and “Neutral.” Knowing that the [H+] x [OH-] always equals x 10-14, fill in the [OH-] for each of the five solutions in the “Z” Diagram (1 x 10-14 is called the Dissociation Constant for water, Kw) (1 x 10-14 = 10 x 10-15) Write the “pOH” of each solution below the [OH-]’s pH + pOH always equals _ A solution of acid has [H+] = 3.0 x 10-3 M a Calculate the [OH-] b Calculate the pH _ the pOH _ A solution of base has an [OH-] = 4.25 x 10-5 M a Calculate the [H+] _ b Calculate the pH _ the pOH _ Calculate the pH’s of the following solutions: 2.53 x 10-2M HCl pH = 2.53 x 10-4M HCl pH = 2.53 x 10-5M HCl pH = A pH with significant figures is written with numbers after the decimal place 10/19/2022 Page 103 of 115 Ka and Kb practice Benzoic acid, HC6H5CO2, is an organic acid whose sodium salt, NaC6H5CO2, has long been used as a safe food additive to protect beverages and many foods against harmful yeasts and bacteria The acid is monoprotic Write the equation for its Ka The [H+] of a 0.10 M solution of cyanic acid (HCNO) is found to be 0.0010 M Calculate the Ka for cyanic acid HCNO↔H+ + CNO3 If 1.22 grams of benzoic acid, HC6H5CO2, is dissolved in 1.0 L of water, the [H+] is found to be 8.0 x 10-4M Calculate the Ka for benzoic acid HC6H5CO2↔H+ + C6H5CO24 A 0.0050 M solution of butyric acid, HC4H7, has a pH =4.0, calculate Ka HC4H7O ↔ H+ + C4H7O25 Determine the [OH-] and the [H+] of a 0.20 M solution of formic acid The Ka = 1.8 x 10-4 HCOOH ↔ H+ + HCOO6 HCN has an initial molarity of 0.50 M, with a Ka value of 3.7 x 10-8 Calculate its pH at equilibrium Ethylamine (C2H5NH3) is a weak Bronsted-Lowry base If it has an initial molarity of 0.24M and a Kb of 5.6 x 10-4, calculate its pH at equilibrium A chemist adds 0.75 moles of NH3 to enough water to make 0.50 liters of solution -5 Kb of ammonia is 1.8 x 10 Determine the pH of this solution at equilibrium Hydrazine, N2H4, has been used as a rocket fuel Like ammonia, it is a Bronsted base A 0.15 M solution has a pH of 10.70 What is the Kb for hydrazine? 10 Nicotinic acid, HC2H4NO2 is a B vitamin It is also a weak acid with Ka=1.4 x 10-5 What is the [H+] and the pH of a 0.010 M solution? 10/19/2022 Page 104 of 115 Titration Curve Practice 1) First, identify the type of titration simply by looking at the titration curve a is it a strong acid being titrated with a strong base? b is it a strong base being titrated with a strong acid? c is it a weak acid being titrated with a strong base? d is it a weak base being titrated with a strong acid? e is it a weak base being titrated with a weak acid f If an acid is being titrated, is it a mono-, di-, or tri-protic acid 2) You need to fill in the blanks at the top of each titration curve in the following manner: a fill in the first blank with the type of solution being titrated (what is in the beaker/flask being analyzed) b fill in the second blank with the titrant (the solution being delivered from the buret Example: if a weak acid was in the beaker and it was being titrated with a strong base from the buret, you would write: Weak acid/Strong Base Then… 1) Analyze each curve to find the equivalence point(s) 2) Using the equivalence point(s); a Determine the Ka(’s) or Kb(‘s), when applicable b Use your text to identify an effective indicator that could be used to show the endpoint in a titration c Determine the concentration of the sample being titrated, assuming the titrant is 0.100 M and that 10.0 mL of sample was titrated each time 10/19/2022 - _ titration Page 105 of 115 10/19/2022 - _ titration Page 106 of 115 10/19/2022 - _ titration Page 107 of 115 10/19/2022 _ - _ _ Titration Page 108 of 115 10/19/2022 - _ titration Page 109 of 115 10/19/2022 - _ titration Page 110 of 115 10/19/2022 Page 111 of 115 Chapter 14 and 15 practice: In your group be sure to show all work associated with the problem If you would like to see the answer, you must first show me the work to the problem 2NH3  NH4+ + NH2In liquid ammonia, the reaction represented above occurs In the reaction NH4+ acts as At 25C, aqueous solutions with a pH of have a hydroxide ion concentration, [OH-], of What part of the curve corresponds to the optimum buffer action for the acetic acid/acetate ion pair? How can 100 mL of sodium hydroxide solution with a pH of 13.00 be converted to a sodium hydroxide solution with a pH of 12.00? Mixtures that would be considered buffers include which of the following? I 0.10 M HCl + 0.10M NaCl II 0.10MHF + 0.10M NaF III 0.10M HBr + 0.10M NaBr A) I only B) II only C) III only D) I and II E) II and III Ascorbic acid, H2C6H6O6(s) is a diprotic acid with Ka1=7.9x10-5 and Ka2=1.6 x10-12 In a 0.005M aqueous solution of ascorbic acid, which of the following species is present in the lowest concentration? A) H2O(l) B) H3O+(aq) C) H2C6H6O6(aq) D) HC6H6O6-(aq) E) C6H6O6-2(aq) In a saturated solution of Zn(OH)2 at 25°C, the value of [OH-] is 2.0 x 10-6 M What is the value of the solubility product constant, Ksp, for Zn(OH)2 at 25°C? For the stepwise dissociation of aqueous H3PO4, which of the following is not a conjugate acid–base pair? A) H2PO4 and PO43 B) HPO42 and PO43 C) H3PO4 and H2PO4 D) H3O+ and H2O 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 10/19/2022 Page 112 of 115  2 E) H2PO4 and HPO4 What is the Ka expression for HOCl? Calculate the [H+] in a solution that has a pH of 2.30 Consider the reaction HNO2(aq) + H2O(l) H3O+(aq) + NO(aq) Which species is the conjugate base? Calculate the pH of 0.250 M HNO3(aq) For weak acid, HX, Ka = 1.0  106 Calculate the pH of a 0.10 M solution of HX Determine the molarity of a solution of the weak acid HClO2 (Ka = 1.10  102) if it has a pH of 1.25 Calculate the pOH of a 0.10 M solution of Ba(OH)2 What is the pH of a 0.45 M KCl solution? solid sodium carbonate (Na2CO3) Use the following choices to describe an aqueous solution made from this substance Acidic, neutral, basic or cannot tell solid ammonium perchlorate (NH4ClO4) For NH4+, Ka = 5.6  1010; for ClO4, Kb 1021 Use the following choices to describe an aqueous solution made from this substance Acidic, neutral, basic or cannot tell The pH of a 1.0 M sodium acetate solution is: A) 7.0 B) less than 7.0 C) not enough information is given D) greater than 7.0 A 1.0-liter solution contains 0.25 M HF and 0.60 M NaF (Ka for HF is 7.2  104) What is the pH of this solution? Calculate the pH of a solution that is 0.5 M in HF (Ka = 7.2  104) and 0.6 M in NaF For a solution equimolar in HCN and NaCN, which statement is false? A) This is an example of the common ion effect B) The [H+] is equal to the Ka C) Addition of NaOH will increase [CN and decrease HCN D) Addition of more NaCN will shift the acid dissociation equilibrium of HCN to the left E) The [H+]is larger than it would be if only the HCN was in solution How many moles of solid NaF would have to be added to 1.0 L of 1.90 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change (Ka for HF = 7.2  104) What is the molarity of a sodium hydroxide solution if 25.0 mL of this solution reacts exactly with 22.30 mL of 0.253 M sulfuric acid? A 10-mL sample of tartaric acid is titrated to a phenolphthalein endpoint with 20 mL of 1.0 M NaOH Assuming tartaric acid is diprotic, what is the molarity of the acid? If 25 mL of 0.75 M HCl are added to 100 mL of 0.25 NaOH, what is the final pH? 10/19/2022 Page 113 of 115 Ksp practice Keep me but put all answers in your notes How many moles of solid NaF would have to be added to 1.0 L of 1.90 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change (Ka for HF = 7.2  104) Calculate the pH of a solution made by mixing 100.0 mL of 0.300 M NH3 with 100.0 mL of 0.100 M HCl (Kb for NH3 is 1.8  105) Find the solubility (in mol/L) of lead chloride (PbCl2) at 25C Ksp = 1.6  105 Solubility Products (Ksp) BaSO 1.5 10 CoS 5.0 10 22 PbSO 1.3 10 AgBr 5.0 10 13 Which of the compounds is the most soluble (in moles/liter)? You have a solution consisting of 0.10 M Cl and 0.10 M CrO42 You add 0.10 M silver nitrate dropwise to this solution Given that the Ksp for Ag2CrO4 is 9.0  1012, and that for AgCl is 1.6  1010, which of the following will precipitate first? silver chromate cannot be determined by the information given silver nitrate silver chloride The solubility of CaSO4 in pure water at 0C is gram per liter The value of the solubility product is The molar solubility of PbI2 is 1.5  103 M Calculate the value of Ksp for PbI2 Calculate the concentration of chromate ion, CrO42, in a saturated solution of CaCrO4 (Ksp = 7.1  104) Calculate the concentration of the silver ion in a saturated solution of silver chloride, AgCl (Ksp = 1.6  1010) 10 The molar solubility of BaCO3 (Ksp = 1.6  109) in 0.10 M BaCl2 solution is: 11 It is observed that 7.5 mmol of BaF2 will dissolve in 1.0 L of water Use these data to calculate the values of Ksp for barium fluoride 12 The Ksp of AgI is 1.5  1016 Calculate the solubility in mol/L of AgI in a 0.30 M NaI solution 13 The molar solubility of AgCl (Ksp = 1.6  1010) in 0.0020 M sodium chloride at 25C is: 14 Silver chromate, Ag2CrO4, has a Ksp of 9.0  1012 Calculate the solubility in mol/L of silver chromate 15 The solubility of mol/L of Ag2CrO4 is 1.3  104 M at 25C Calculate the Ksp for this compound 16 Calculate the concentration of Al3+ in a saturated aqueous solution of Al(OH)3 (Ksp =  1032) at 25C 17 The Ksp for PbF2 is 4.0  108 If a 0.050 M NaF solution is saturated with PbF2, what is the Pb2+ in solution? 10/19/2022 Page 114 of 115 18 Chromate ion is added to a saturated solution of Ag2CrO4 to reach 0.10 M CrO42 Calculate the final concentration of silver ion at equilibrium (Ksp for Ag2CrO4 is 9.0  1012) 19 In a solution prepared by adding excess PbI2(s) Ksp = 1.4  108 to water, the I at equilibrium is: 10/19/2022 Page 115 of 115 Electrochem practice Which energy conversion takes place in a galvinic cell? Which of the following reactions is possible at the anode of a galvinic cell A) Zn > Zn2+ + 2eB) Zn2+ + 2e- > Zn C) Zn2+ + Cu >Zn + Cu2+ D) Zn + Cu2+ > Zn2+ + Cu A block of Pt is immersed in a solution which has 0.50 M Br2 and 0.10 M Br- A block of chromium is immersed in a solution of 0.20 M Cr3+ The wires are connected to a voltmeter a What type of cell is this? b What is Eo for this cell c What is E for this cell at 25oC d How many moles of electrons are involved in the reaction? Consider a galvanic cell with a zinc electrode immersed in 1.0 M Zn2+ and a silver electrode immersed in 1.0 M Ag+ a Calculate E0 for this cell b Which of the electrodes in the anode? c Calculate delta G d Calculate K for the cell 11 Consider a galvanic cell with a zinc electrode immersed in 0.050 M Zn 2+ and a silver electrode immersed in 10.00 M Ag+ Calculate Q for the cell E for the cell at these non standard conditions Assume Temp is 25 oC 12 An antique car bumper is to be chrome plated The bumper is dipped into acid dichromate solution and the bumper serves as the cathode of the electrolytic cell The dichromate deposits solid chromium onto the surface of the bumper If the current is 10 amperes, how long does it take to deposit 1.00 x 102 g of Cr(s) 13 What quantity of coulombs is required to reduce 40.0 g of CrCl3 to chromium metal? 14 If a constant current of 5.0 amperes is passed through a cell containing Cr 3+ for 1.0 hour, how many grams of Cr will plate out on the cathode? 15 How many seconds would it take to deposit 21.40 g of silver from a solution of silver nitrate using a current of 10.00 amperes? ... be data and calculations only You must always answer questions if they are in the lab manual You must get your data stamped in your lab notebook before you leave the lab Lab Reports (Lab reports... a link to a video and a paper handout of how to solve for the exponents if you don’t remember how to logs Prelab: Read all the procedures and be ready to hand me a slip of paper cm square with... region of rapid change and then leveled off, the data collected is graphed The end point is determined graphically, and other information may also be read from the shape of the graph MSDS: Vinegar