MISSED THIS? Read Section 17.9 (Pages 765-769). Consider a 0.14 M solution of a weak polyprotic acid (H₂A) with the possible values of Kal and K₁2 given here. Calculate the contributions to [H3O+] from each ionization step. At what point can the contribution of the second step be neglected? ▼ Part C Kal = 1.0 x 10-4 and Ka2 = 1.0 x 10-6 Express your answers in molarity to two significant figures separated by a comma. ΑΣΦ [H3O+]1, [H3O+]2= 3.7.10-³,6.03 10-5 ● ? M

MISSED THIS? Read Section 17.9 (Pages 765-769). Consider a 0.14 M solution of a weak polyprotic acid (H₂A) with the possible values of Kal and K₁2 given here. Calculate the contributions to [H3O+] from each ionization step. At what point can the contribution of the second step be neglected? ▼ Part C Kal = 1.0 x 10-4 and Ka2 = 1.0 x 10-6 Express your answers in molarity to two significant figures separated by a comma. ΑΣΦ [H3O+]1, [H3O+]2= 3.7.10-³,6.03 10-5 ● ? M

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter10: Effect Of Electrolytes On Chemical Equilibria

Section: Chapter Questions

Problem 10.4QAP

See similar textbooks

Similar questions

For the diprotic weak acid H₁A, Kal = 3.2 × 10-6 and Ka2 = 6.3 × 10-9. What is the pH of a 0.0800 M solution of H,A? What are the equilibrium concentrations of H2A and A2 in this solution? Step 1: Make an equilibrium table for the molar concentrations at equilibrium after the first dissociation step. Concentration (M) H,A(aq) H+(aq) + HA (aq) initial 0.0800 0 0 change -I +x +x equilibrium Express Kal in terms of the initial concentration of H,A and x, and then show the simplified expression when x is assumed to be negligible compared to to the initial concentration. complete: Kal= = 3.89 Incorrect Determine the numerical value of x. x = 6.3 ×10 9 M simplified: Kal≈ 3.9 Incorrect
Given that log Kso for Zr(OH)4(s) is 10-54.1, at what pH would the maximum concentration of Zr4+(aq) be 10-3 M?
Consider an F M solution of Fe2(SO4)3. Besides H+ and OH−, the known species are Fe3+, Fe(OH)2+, Fe(OH)2+, Fe2(OH)24+, FeSO4+, SO42−, and HSO4−. a) Write the charge balance equation for this solution. b) Which species must be an ion pair, and which comes from acid hydrolysis of Fe3+? Write the balanced acid hydrolysis reaction for the hexa-aquo complex of Fe3+ and report its pKa c) Write two mass balance equations for this solution, one for total iron and one for total sulfate. [How do you think you should handle the species that includes two iron atoms?] Give numerical values for these equations in terms of F.
Calculate the H+ ion concentration in a 0.55M solution of a moderately strong acid HA, where Ka=3.0x10^-2. Show work. 7:34 PM
What is the hydronium ion concentration of a 0.200 M hypochlorous acid solution with Ka=3.5 x 10-8? The equation for the dissociation of hypochlorous acid is: HOCI(aq) + H2O() = H30*(aq) + OCI"(aq). O 3.7 x 10-5 M O 8.4 x 10-4 M 8.4 x 10-5 M 1.9 x 10-4 M
For a solution having 1.00 x 10-3 eq/L total alkalinity (contributions from HCO3-, CO32-, and OH-) at [H+] = 4.69 x 10-11, what is the percentage contribution to alkalinity from CO32-?
What is the pOH of a solution prepared by diluting 208.4 mL of 1.059 M HNO3 (ka>>1) to a total volume of 14.248L? Please report your answer to 3 decimal places.
a. What is the base ionization constant for CH,BrCOO-? Kb: CH -7 -5 ニフ 7.14 x 10 "CH zBV CoOlH Ś CHZBV C00 b. What is the standard free energy of formation of CH2BRCOO ? CHz Br c O0 c. What is the pH of a 0.027 M NACH;B1COO? Note: More space on next page.
Calculate the concentrations of all species present (other then water) in an aqueous solution of 0.25 M H2SO3 Constants: Ka1,H2SO3= 1.5x10^-2 Ka2,H2SO3= 6.3x10^-8 Kw= 1.0x10^-14
Calculate the pH of a 5.3 x 10-M solution of H2SO4 (Ka, = 1.2 × 10-2). -3 pH =
Calculate the acid dissociation constant, Ka, for hydrogen cyanide, HCN, based on the given information. (CN),(g) + 2 H*(aq)+2 e¯= 2 HCN(aq) E° = 0.373 V Eº! = -0.041 V -10 Ka = 1 x10
Which salt below will produce the lowest [H 3O +] in an aqueous solution? 0.1170 M N2H5Br, Kb(N2H4) = 8.900e-7 0.1170 M CH3NH3Br, Kb(CH3NH2) = 0.0003700 0.1170 M CH3CH2CH2NH3Cl, Kb(CH3CH2CH2NH2) = 0.0005100 0.1170 M C6H5NH3Br, Kb(C6H5NH2) = 4.300e-10