Which statement is incorrect for conditional formation constants, Kf ?O Kf = ay4- KịO Kf allows the view of uncomplexed EDTA as being in only one form, Y, inequilibrium calculations.O As pH drops the value of Kf increases.O Kt is pH dependent.O The values of K must be large to guarantee sharp end points during titrations.

The statement which is incorrect about the conditional formation constant Kf is, As pH drops the…

Which statement is incorrect for conditional formation constants, K¢ ? O K = ay4- Kf %3D O K allows the view of uncomplexed EDTA as being in only one form, Yª-, in equilibrium calculations. O As pH drops the value of K increases. O Kt is pH dependent. O The values of K must be large to guarantee sharp end points during titrations.

Which statement is incorrect for conditional formation constants, K¢ ? O K = ay4- Kf %3D O K allows the view of uncomplexed EDTA as being in only one form, Yª-, in equilibrium calculations. O As pH drops the value of K increases. O Kt is pH dependent. O The values of K must be large to guarantee sharp end points during titrations.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A certain solution is 0.010 M in Zn²* and Fe2*. If the hydrogen sulfide solution is saturated, that is [H2S)= 0.30 M, for each pH determine which sulfides will precipitate. Kspa for FeS = 6 x 10*2, Kapa for Zn – 3 x 102 pH - 0.5 1. Neither will precipitate. pH - 1.5 2. Only FeS will precipitate. pH 2.5 3. Only ZnS will precipitate. 4. Both FeS and ZnS will precipitate. pH = 3.5 ->
23
Which of the following does NOT happen with a weak acid's pkKa = pH of the environment? Answers A-D A Log(IA-/[HA]) = 1 В 0.5 equivalents of strong base has been added to weak acid C The weak acid's [HA] = [A-] %3D The midpoint of the titration curve has been reached
Given this series of equilibrium reactions. See Image(a) Which way should the reaction to “tend” at high pH? Why?(b) Which way should the reaction to “tend” at low pH? Why? (c) What Fe(III) species would be least soluble?
Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.02 M KMnO4 solution was used for the titration. gH * + MnO 4 + 5Fe 2+ -> SFe 3+ + Mn 2+ + 4H 20 (MM Fe = 56 a/moll mass of iron compound (g) 0.604 initial buret reading (mL) 0.94 Tinal buret reading (mL 16.21
• An unknown acid (HA) was titrated with NaOH(aq). • The following titration curve was constructed using the laboratory data. You will use this titration curve to answer the questions related to this problem. • Assume that all laboratory work was completed at 298 K. 14 12 10 6. 4. 2. 4 9. 8. 10 12 14 16 18 20 22 24 26 28 30 Volume of Titrant / mL Which of the following net ionic equations explains the pH of the analyte solution before any titrant is added? A (aq) + H20(1) HA(aq) + OH (aq) A (aq) + H3O*(aq) --> HA(aq) + H20(1) O H*(aq) + OH (aq) H20(1) --> O HA(aq) + OH (aq) --> H2O(aq) + A (aq) HA(aq) + H20() H3O*(aq) + A (aq)
175.0 mL of 0.2015 M nitric acid was added to 1.4213 g of impure calcium carbonate sample. The excessacid was back titrated with 72.5mL of 0.1152 M sodium hydroxide to reach the endpoint. Calculate for thepercent calcium carbonate? (MM of CaCO3= 100.0869 g/mol)2HNO3 + CaCO3 → Ca(NO3)2 + H2O + CO2HNO3 + NaOH → NaNO3 + H2O
Aditi titrated 80.00 mL of 0.50 M methylamine, CH3NH2, with 0.40 M HCI. CH3NH₂ Kb = 4.4 x 10-4 What is the pH for the solution at the equivalence point of the titration? pH = [?] pH @ Equiv. Pt Enter
Q1) in titration of the solution containing 0.1 Molar of I and 0.1 Molar of Cro,", with the solution of 0.1 mołar of Ag+, what is the titration error in first step? if the end point of first titration will be taken on the precipitation of Ag.Cro, KSP(Ag,Cro,)=101n KSP(Agi) = 10 Q2) Q2) How much mole of NH, to be added to 500 ml of the solution with pH-8.9 to dissolve 5x10 * of ABSCN? PKSP(AGSCN)=12 , PKa(NH.") =9.2, PKdAg(NH,)*/Ag+=7.2
3. At 48.2°C, 5.00ml of the saturated solution of bo ax was titrated with 0.235M HC1. It took 23.00 mL of the a id to reach the equivalence point. What is the molarity of the tetra-borate anion in t e solution?
A student does not filter his/her saturated solution before titrating. Will the calculated Ksp probably be too high, too low, or unaffected? Why? Solid substances are not part of equilibrium equations, so their presence would leave the value of Ksp unaffected. The remaining solids would absorb excess H30+ ions during the titration, making the calculated value of [OH ], and thus Ksp, too low. O The remaining solids would dissolve during the titration to give more OH¯. The calculated Ksp would therefore be too high.
None