Correct the ones that are marked wrong: Prelab Table Ia: Using the solubility rules, write in the predicted results for each pair ofions. Write the formula of the compound that would result for each pair and indicate I forinsoluble, or S for soluble, or SS for slightly soluble. Two examples have been done.Prelab Table Ia : Prediction of Solubility of Salts in water.PO-CHBrSO?-OHCO3² | C2H3O: | S²-CrO,?Na+SK*I.-Fe2+I.I.II.Cu²* CuClCubrI.Ag AC1UI Prelab Table Ib Solubility of Compounds in WaterPrimarySolubility in100mL H20from CRCSolidName ofPredictedspecies inH20Solubility inH20compoundcompoundHandbook1BaSO4BariumBaSO4 (s)Insoluble0.31mgsulfateA(Pude(s) Insolubld D.2 maoluble 50.5 macarbonateoC0z (S) |nsolublel0. maABCHLO: ilveracctatd or ore L.25mgCa3(PO4)2 Calcium2phosplate(NH)»SO4 Ammonium o,3Tonstead4P6CO3Hg2Cl2Mercury(I)chlorideHg2Cl2(s)Insoluble0.4 mg7Cu2OCoppertiDoxide Cu,0(s) | Inolubld 0.2 mia8.C6H12O6Glucore Joluble 0.212 x 10Cattelou and Koorouble 5.834sucrose9C6H5COOHBenzoic acid10BaCl2Barium chlorideBa2+ and 2CSoluble37.0 gions

uld result for each pair and indicate I for Ensoluble, or S for soluble, or SS for slightly soluble. Two examples have been done. Prelab Table la : Prediction of Solubility of Salts in water. SO PO, OH- CF Br CO3²- C2H3O2 S²- CrO,²- Na+ S K* In - Fe²* FeClaFebr|Felk FeS DyFe(MFe(CH) Fe CO3F€CH30)} Fes FelrO I. I I. Cu²* CuClCubr す to

uld result for each pair and indicate I for Ensoluble, or S for soluble, or SS for slightly soluble. Two examples have been done. Prelab Table la : Prediction of Solubility of Salts in water. SO PO, OH- CF Br CO3²- C2H3O2 S²- CrO,²- Na+ S K* In - Fe²* FeClaFebr|Felk FeS DyFe(MFe(CH) Fe CO3F€CH30)} Fes FelrO I. I I. Cu²* CuClCubr す to

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

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and Employees CH STATE GE 90 ENDULERSE IS FOREVER "ON-Tame Name Jodi Rayal Molarity = wt. x1000 3. Calculate the massof Potassium hydrogen phthalate (KHP) to prepare a 250.0 mL solution of 0.1000 M KHP solution. Mol ut. x Voluse the 2500×1000 204.22250 mass Initial Buret Reading Final Buret Reading Vol NaOH Added Moles of NaOH Moles of HCI Volume of unknown HCI solution Concentration of HCI Average concentration of HCI of KHP = 5.11g 4. Complete the table below for the following neutralization reaction of an unknown concentration of hydrochloric acid with 0.100 M sodium hydroxide: Mu spate solution Trial 1 0 11.15 го data and calculate the concentration 15 Trial 2 11.15 22.15 Trial 3 22.15 33.25 abyh 067 LANDINUKASHU TROWTHCENTISSATE ARAD Ma That par މއކނި REMURNAR MISAMARALISERDRY Tile
Mark and John, two vinegar enthusiasts, are each tasked to determine the acetic acid content of their respective vinegar concoctions by titration. First, a 1 M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol) standard that is 99.4% pure. In the process, 0.540 g KHP was found to require 2.80 mL of the KOH solution to completely react up to the phenolphthalein endpoint. Then, Mark and John both prepared their samples by taking 10.0-mL aliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant and indicator, Mark’s vinegar required 18.60 mL of the standardized titrant to reach the endpoint, while John’s vinegar required 16.50 mL of the same titrant to reach the same endpoint. Question: What is the acetic acid concentration of Mark’s and John’s vinegar in molarity given that the Concentration of KOH is 9386 M?
Mark and John, two vinegar enthusiasts, are each tasked to determine the acetic acid content of their respective vinegar concoctions by titration. First, a 1 M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol) standard that is 99.4% pure. In the process, 0.540 g KHP was found to require 2.80 mL of the KOH solution to completely react up to the phenolphthalein endpoint. Then, Mark and John both prepared their samples by taking 10.0-mL aliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant and indicator, Mark’s vinegar required 18.60 mL of the standardized titrant to reach the endpoint, while John’s vinegar required 16.50 mL of the same titrant to reach the same endpoint. Question: What is the exact concentration of the KOH titrant in molarity? What is the balanced chemical equation between the analyte and the titrant? What is the color transition (color X ? color Y) expected throughout the course of titration?
To determine the percentage of bromide in a mixture containing a soluble bromide salt, the procedure from Experiment 10 is used except the bromide is precipitated with aqueous lead (II) nitrate, Pb(NO3)2, forming PbBr2(s). Initially, a 0.7893 g sample of an unknown bromide salt is dissolved in water. Excess Pb(NO3)2 is added to the solution to quantitatively precipitate the bromide from the solution. The resulting mixture is filtered through a piece of filter paper weighing 1.3587 g. After several days of drying, the filter paper and precipitate weighed 1.8257 g. Calculate the percent bromide in the original sample. Pb(NO3)2 Mw = 331.2 g/mol PbBr2 Mw = 367.0 g/mol
In the standardization of HCl using pure anhydrous sodium carbonate as the primarystandard for methyl orange as an indicator, 1.0 mL HCl was found to be equivalent to 0.05gof sodium carbonate (MW =106). The normality of HCl is:
Choi is fond of carbonated beverages so he crafted his own soda formulation called “Sodalicious.” Ulan, who is a fellow enthusiast, also made her own formulation which she called “Soda Pop!” to challenge his friend Choi. To know which formulation is better, they sought to determine the carbonic acid content of their soda formulations using titration. In the first part of their experiment, a 0.5 Mlabeled NaOH solution was standardized against 0.350 grams of KHP (MW = 204.22 g/mol) primary standard that is 99.6% pure. The titration required 3.16 mL of the NaOH solution to reach the phenolphthalein endpoint. In the second part of their experiment, Choi and Ulan independently prepared their samples by taking 25.0-mL of their soda sample and diluting it to 30.0 mL. Using the same titrant and indicator, Choi’s “Sodalicious” required 1.39 mL of the standardized titrant to reach the endpoint, while Ulan’s “Soda Pop!” required 0.926 mL of the same titrant to reach the endpoint. A. What is the…
Choi is fond of carbonated beverages so he crafted his own soda formulation called “Sodalicious.” Ulan, who is a fellow enthusiast, also made her own formulation which she called “Soda Pop!” to challenge his friend Choi. To know which formulation is better, they sought to determine the carbonic acid content of their soda formulations using titration. In the first part of their experiment, a 0.5 Mlabeled NaOH solution was standardized against 0.350 grams of KHP (MW = 204.22 g/mol) primary standard that is 99.6% pure. The titration required 3.16 mL of the NaOH solution to reach the phenolphthalein endpoint. In the second part of their experiment, Choi and Ulan independently prepared their samples by taking 25.0-mL of their soda sample and diluting it to 30.0 mL. Using the same titrant and indicator, Choi’s “Sodalicious” required 1.39 mL of the standardized titrant to reach the endpoint, while Ulan’s “Soda Pop!” required 0.926 mL of the same titrant to reach the endpoint. D. Calculate…
Rei and Akari, two vinegar enthusiasts, are each tasked to determine the aceticacid content of their respective vinegar concoctions by titration. First, a 1M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol)standard that is 99.4% pure. In the process, 0.540 g KHP was found to require2.80 mL of the KOH solution to completely react up to the phenolphthaleinendpoint. Then, Rei and Akari both prepared their samples by taking 10.0-mLaliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant andindicator, Rei’s vinegar required 18.60 mL of the standardized titrant to reach theendpoint, while Akari’s vinegar required 16.50 mL of the same titrant to reach thesame endpoint. What is the exact concentration of the KOH titrant in molarity? What is the balanced chemical equation between the analyte and the titrant? What is the color transition (color X color Y) expected throughout thecourse of titration? What is the acetic acid concentration of Rei’s and…
The concentration of arsenic in an insecticide can be determined gravimetrically through its precipitation as MgNH4AsO4. After the formation of the precipitate, it must be ignited for total conversion to Mg2As2O7, which is then cooled and weighed. Considering that a sample of 1,627 g of the insecticide produced 106.5 mg of Mg2As2O7, determine the% (m/m) As2O3 in the insecticide. Given the molar masses: Mg2As2O7 = 310.447 g / mol and As2O3 = 197.841 g / mol
25.0mL of a 0.515 M K2S solution is mixed with 30.0 mL of 0.833 M HNO3 acid solution to give the following reaction: K2S(aq) + 2HNO3(aq) → 2KNO3(aq) + H2S(g) H2S is an unwanted by-product in a pulp and paper industry. To capture H2S gas, it is bubbled through a NaOH solution to produce Na2S with a yield of 94%. H2S(g) + 2NaOH (aq) → Na2S (aq) + 2H2O(l) The mass of H2S(g) that was processed (in kg) if 10.76 kg of Na2S was collected is
Calculate the weight of pure sodium carbonate that is necessary to prepare 2.806 L of 0.223 N Na2CO3 (105.99 g/mol) from the primary-standard solid. Assume the solution is to be used for titrations in which the reaction is: CO32- + 2H+ ----> H2O + CO2 Express you answers in 3 decimal places
I need help calculating the solubility. thank you C. Calcium Fluoride, CaF2 (aka, Fluorite), in a solution containing 19 mg/L of LiF (aka, Griceite),with all of the LiF being dissolved into solution. Please assume that LiF dissolves such that [Li] =[F] = 7.33 x 10-4 m. After adding CaF2 to the solution and allowing it to dissolve, what are finalvalues of [Ca], [Li] and [F]?Note: you are given the concentrations of [Li] and [F] that result from dissolving LiF. Nosolubility calculation is required for dissolving LiF; just use the concentration given above.Steps:- First, write the stoichiometric equation for dissolution of CaF2 , with the solidon the left and the two ions in solution on the right, separated by a "two-way" arrow. Hint: whenCaF2 dissolves, you get 2 moles of F for every 1 mole of Ca.- Second, set up a law of mass action equation for dissolution of CaF2. There is a common ioneffect for F, so if [Ca] = x, then [F]= 2x + [FLiF], where [FLiF] is from dissolution of the…