How to do net ionic equation step by step on the qualitative analysis scheme? [mustredo final draft for in report]Qualitative Analysis Scheme* Comprehensive testing of all ims lconsectutive testing)* After adition of te sting agent, ions go to the RIĞHT, precipitates go to the LEEFT* be Sure to write states of matter, vse steps #s as this scheme does* number all Separation steps!* You will write NIES for all Steps (1-9), yov will Show only the Net lonic, and theymust be typed! Do not show NIE'S if they produced no reaction!* DO NOT LOSE THIS PAPER You WILL NEED TO INCLUDE IT IN YOUR LAB REPORTNOTES/ROUGH DRAFT9.Ag*, Hg,", Pb“, Ca*, Mg**, Ba", NHa"NH 31g)Speciallit. Red-bleeO Add HCItestSolidDe cantDecanNHy CompletePptyou haveAgd (s)HgzCl cs)Ba Laa)cazt Lag)PBC/2a) Add WaterSolid6) Heat decant6 AddAg Cles)Pbzt caqo)SolidDecantCompletePpt.(3) Add usm)NH3Ba SO4 (s)white pptCa?t ca%)PH mustPbCr O415)you haveBaztbebasica) PHZ8yellow ppt(€)SolidDecantSolidYou haepb ?4DecantHg Nih Cl cs)Caczo41s)Black optwhite PPtMgLAg(NHS), ClideM9 Test "a) ada SM NAgyou haveCaztYou havePmer Hab)add o.1 M NazHPOc) Cent & decont8.d) Add HCl 2Mg reagane) Add eM NAOH O(4Add HNO.PH must be < 7]!PH mustAg Clis)MglOH)2 ()bivelselly PPTbe|ЬasicSAVE YOURDECANTYou haveYou haeAgtMghtyou need to test it!tesp pH(audic) 6. For each numbered step in the qualitative analysis scheme in number 5 above, typeall net ionic equations associated with the step. Write only the final net ionic equationsfor the general qualitative separation scheme above. Refer to Experiment 7. You wereasked to do this there as well.orimental

When we are constructing net ionic equations, we have to keep few points in our mind: Only salts in…

6. For each numbered step in the qualitative analysis scheme in number 5 above, type all net ionic equations associated with the step. Write only the final net ionic equations for the general qualitative separation scheme above. Refer to Experiment 7. You were asked to do this there as well.

6. For each numbered step in the qualitative analysis scheme in number 5 above, type all net ionic equations associated with the step. Write only the final net ionic equations for the general qualitative separation scheme above. Refer to Experiment 7. You were asked to do this there as well.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.26QAP

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La) Provide the balance cauation for this veaction Consider th hydrasne Na He NHs Caq)NA ockag)+ H2 OpN2H rcacko to produce 4- st Na Cl(an) b)if, 136.0.me of 0.375 M amming solution reacts With188L Na OCL at STP Which the immiting reagent and Which is the excess regont. is c)if 250ML hudrazine gas is collected at STP, wheet is eaction. the percend yield of the
B. Molar Solubility of Calcium Hydroxide in the Presence of a Common Ion Trial 1 Trial 2 Trial 3 OM 1. Volume of saturated Ca(OH), with added CaCl, solution (mL) 25.0 25.0 25.0 0.05956 16.80 32.9 2. Concentration of standardized HCI solution (moVL) 3. Buret reading, initial (mL) O.00 33.5 4. Buret reading, final (mL) 10.80 48 5. Volume of HCI added (mL) 6. Moles of HCI added (mol) 7. Moles of OH¯ in saturated solution (mol) 8. (OH), equilibrium (moVL) 9. Molar solubility of Ca(OH), with added CaCl, (mo/L) 10. Average molar solubility of Ca(OH), with added CaCl, (mo/L) Account for the different molar solubilities in Part A.11 and Part B.10 (Report Sheet).
O KINETICS AND EQUILIBRIUM Calculating the solubility of an ionic compound when a commo... oh Data Formula Ksp Calculate the solubility at 25 °C of Zn(OH), in pure water and in a 0.0060M ZnSO , solution. BaCrO4 1.17x10-10 BaSO4 1.08x10-10 Round both of your answers to 2 significant digits. CaCO3 3.36x10-9 CaF2 3.45x10-11 solubility in pure water: Co(OH)2 5.92x10-15 CuBr 6.27x10-9 solubility in 0.0060 M ZNSO4 solution: CuCO3 1.4x10-10 Fe(OH)2 4.87x10-17 PbCO3 7.40x10-14 PbCrO4 2.8x10-13 PBF2 3.3x10-8 Mg(OH)2 5.61x10-12 Ni(OH)2 5.48x10-16 AgBrO3 5.38x10-5 A92CO3 8.46x10-12 AgCI 1.77x10-10 Ag2CrO4 1.12x10-12 SrCO3 5.60x10-10 ZnCO3 1.46x10-10 Zn(OH)2 3.0x10-17 AgBr 5.35x10-13 AuCl 1.77x10-10 Explanation Check Terms of Use Privacy O 2021 McGraw-Hill Education. All Rights Reserved 18 MacBook Air olo
please help. will comment and like when all answerd and correct Use the References to access important values if needed for this question. The Solubility Product Constant for calcium fluoride is 3.9 × 10-11. The maximum amount of calcium fluoride that will dissolve in a 0.102 M potassium fluoride solution is Submit Answer Retry Entire Group 8 more group attempts remaining Fil When 25.0 mL of a 1.78 x 10-4 M barium chloride solution is combined with 15.0 mL of a 3.67 x 10-4 M potassium carbonate solution does a precipitate form? ( Kap (BaCO3) = 8.1 × 10-⁹) OYes, the precipitate forms. ONo, the precipitate doesn't form. For these conditions the Reaction Quotient, Q, is equal to When 25.0 mL of a 9.96 x 10-4 M sodium bromide solution is combined with 15.0 mL of a 1.82 x 10-4 M lead nitrate solution does a precipitate form? ( Ksp (PbBr₂) = 6.3 × 10-8) M. OYes, the precipitate forms. ONO, the precipitate doesn't form. For these conditions the Reaction Quotient, Q, is equal to
o/index.html?deploymentld%=55750828934189288909969212&eiSBN=9781305657571&snapshotld%32199898&id%3... ☆ IDTAP Q Search this cou Use the References to access important values if needed for this question. The concentration of H3ASO3 in a solution is determined by titration with a 0.1945 M Ce+ solution. The balanced net ionic equation for the reaction is: 2Ce*(aq) + H3ASO3(aq) + 5H2O(1) 2Ce*(aq) + H3ASO4(aq) + 2H3O*(aq) (a) If 19.83 mL of the 0.1945 M Ce** solution are needed to react completely with 30.00 mL of the H3ASO3 solution, what is the concentration of the H3ASO3 solution? M (b) Which of the two solutions was in the buret during the titration? (c) Suppose at the end of the titration, the solution containing the Ce³* ion is transferred to a volumetric flask and diluted to 300. mL. What is the concentration of Ce3+In the diluted solution? Submit Answer 5 question attempts remaining
96% [4) Wed 3:41 AM Jarissa Collado Q A cvg.cengagenow.com My Home OWLV2 | Online teaching and learning resource from... [Review Topics] (References] Use the References to access important values if needed for this question. M Solid lead nitrate is slowly added to 75.0 mL of a 0.0486 M sodium iodide solution. The concentration of lead ion required to just initiate precipitation is s 2req M. Es M ts M Submit Answer Retry Entire Group ts 2req 8 more group attempts remaining Previous Next problem set O Focus 92%
Table 1: Qualitative Analysis of Group II Cations Group II Cations Confirmatory Reagent Result/ Observation Substance Formed Inference Write the chemical equations involve in the analysis of group II cations. Guide Question: What are differences of the precipitates of each cation in group II? Reference video : https://www.youtube.com/watch?v=BZGZZx1lHKA
la a laccd sign in - X ||| ctrl shift T tab O CHEMICAL REACTIONS Calculating molarity using solute moles caps lock ILION McGraw-Hill Ec X A ALEKS - Shusha X https://www-awu.aleks.com/alekscgi/x/lsl.exe/10_u-IgNslkr7j8P3jH-IvUrTNdLZh5A8CnG03PBGuXr8iCPa7ZMmym 0 lion x360 fn ALEKS μmol L A chemist prepares a solution of sodium hyposulfate (Na₂S₂O3) by measuring out 200. μmol of sodium hyposulfate into a 400. mL volumetric flask and filling the flask to the mark with water. Explanation esc Calculate the concentration in μmol/L of the chemist's sodium hyposulfate solution. Be sure your answer has the correct number of significant digits. →1 1 Z X Type here to search hp Check 2 x10 Graw # 3 X Xx WIL S alt ** 4 C S O % 40 5 V A- G B f7 4+ & 19 ALEKS 7 H hip 18 X IAA N 8 McGraw-Hill Ex A ALEKS-Shush x+ 95T1680XLLcyeOLT... A © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acce 6:25 PM a 7/22/202 9 K M ho P f12 87°F Qo insert 1/5 [ alt prt sc 1 G 2 backspac pause…
AA Learning Learning prod03-cnow-owl.cengagenow.com Login Learning × Online tea... y dr. marlow... Member L... 1req 1req Use the References to access important values if needed for this question. The Solubility Product Constant for silver bromide is 3.3 x 10-13 Solid ammonium bromide is slowly added to 75.0 mL of a 0.0663 M silver acetate solution. The concentration of bromide ion required to just initiate precipitation is M.
DATE Calculate the thconetical uield of the precipitate formed in the reaction 4ml of O.17M Na OH 2ml of O.I M Fecla
plz do correctly & show all work thnx!!! Solid lead(II) nitrate is slowly added to 150 mL of a 0.106 M potassium carbonate solution until the concentration of lead ion is 0.0358 M. The percent of carbonate ion remaining in solution is [ Submit Answer Retry Entire Group 6 more group attempts remaining Solid copper(II) nitrate is slowly added to 125 mL of a ammonium sulfide solution until the concentration of copper(II) ion is 0.0548 M. The maximum amount of sulfide remaining in solution is M. When 12.0 mL of a 6.35×104 M ammonium sulfide solution is combined with 25.0 mL of a 5.64×104M cobalt(II) nitrate solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to[ When 15.0 mL of a 6.32x104 M nickel(II) iodide solution is combined with 25.0 mL of a 2.32×104M sodium hydroxide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to
In bromine water test Procedure: -Add 3 ml of phenol and ethanol in separate test tube-Add 10 ml of water to each test tubes-Transfer to bigger test tubes-For phenol and ethanol, Add bromine water drop by drop until bromine color persists MUST DO: Observe formation of precipitate P.s I provided photos for better visualization of the overall result procedure, I just need a further and detailed answer based on observation. If answered properly I will upvote, I promise tyyy. Please do focus on the formation of precipitate, thank youuu The first photo is the phenol one (colored one) and the second one is the ethanol (clear one)