Use[HOJAre value of ki to calculate the final concertadeсанаTCalculate [H3O+] that would resultsolution of HXWhenof solution[04] = 2x10fromki for HX= 3.3 × 10-4[H3O+] and [OH-] and % iomization3.4 moles ofit is-10Calculateof HXisdissolvedfound at equilibrium thatki for HX14a[1₂0*31043=1×10.41min I Liker

We know for an acid HX HX + H2O↔H3O+ + X-Ki=[H3O-][X-][HX]

the value of ki to calculate Use [H₂OJ Calculate [M30+ that would result from [H3O+] Ki for HX= 3.3 × 10 -4 [H₂O*] and [OH-] and % ionization solution of HX When of solution it is [04²] = 2x10] 3.4 moles of HX Found to calculate the finment concertade -10 Calculate ki for Hox C13₂031043=1*10* a .41m is dissolved at equilibrium that in I Liker

the value of ki to calculate Use [H₂OJ Calculate [M30+ that would result from [H3O+] Ki for HX= 3.3 × 10 -4 [H₂O] and [OH-] and % ionization solution of HX When of solution it is [04²] = 2x10] 3.4 moles of HX Found to calculate the finment concertade -10 Calculate ki for Hox C13₂031043=110* a .41m is dissolved at equilibrium that in I Liker

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.26QAP

See similar textbooks

Similar questions

calkulate Hhemolar Solubiliky of pbl (kse s.o X167) in Awater the
The equilibrium for the vorious proportions of the dissociation of the liquid solutions of amyl ester of dichloroacetic ccid (CHCI,.COOC,H,} into the acid (CHCLCOOH) and amylene (C,H was investigated. The inltial amount tor the CHCI,COOC.H used Is 1 mole. Completethe table below Let b the inltial moles of omylene, V the totdl volume cof mixtures in iters, x. be the number of moles of V. 1.05 0.215 0.455 3.12 .af equibrium ond Kc ester outionum constont n.moles per iter. 2.61 0.401 4.45 0.628 3.54 0.794 0.658 3.44
Which of the following statements are true and which arefalse? (a) For the reaction 2 A1g2 + B1g2 ∆ A2B1g2 Kcand Kp are numerically the same. (b) It is possible todistinguish Kc from Kp by comparing the units used toexpress the equilibrium constant. (c) For the equilibriumin (a), the value of Kc increases with increasing pressure.
In the standardi zation of HCl using pure anhydrou s sodium carbonate as primarystandard for methy l orange as indica tor , 1.0 mL HCl was found to be equiva lent to 0.05gof sodium carbonate (MW =106). The no rmality of HCl is
Non-Commercial Substances Hypothesis: Soluble in Test Bond Molecular Structure ΔΕΝ H2O? Result: H20 Solubility Result: Hexane Substance Classification Solubility Hexane? H2O: pS Sodium Na--Br lonic Bromide 1.9 Hexane: I |--| lodine NP C 0.0 Ammonium N/A lonic Carbonate NH4* O O NH4* Sodium N/A lonic Acetate C--H NP C 0.4 H-C-OH C--O PC H-C-OH Glycerol 1.0 H-C-OH O--H PC 1.4 HI
Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.
Five drops of dichlorofluorescein have been added to a solution containing 0.800 g sample which required 25.30 mL of 0.100 M AgNO3. (c) Calculate the weight percent NaCl in the original sample.
What is the molar fraction of glycine in an aqueous solution whose concentration is 0.140 molkg-1. Data: Mass H2O = 1 kg; M.M. H2O = 18.01 gmol-1.
One of the possible consequences of climate change is anincrease in the temperature of ocean water. The oceansserve as a “sink” for CO2 by dissolving large amounts of it.(a) The figure below shows the solubility of CO2 in water as a function of temperature. Does CO2 behave more or lesssimilarly to other gases in this respect?(b) What are the implications of this figure for the problemof climate change?
Calculate Ksp = () A2BO3 ->2A*+ BO32- Molar concentration of At = Molar concentration of BO32- = 2 M %3D (*Answer in whole number only. No unit)
The Ksn for AgCl is 1.77 x 10-10 while Ksn for PbSO4 is 1.82 x 10-8. Considering both the compounds have the same dissociation stoichiometry, which one would be more soluble in water? Both are equally soluble. O PbSO4 AgCI O The answer cannot be determined with the given information.
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: