Just the incorrect parts. Use the Acid-Base table to write net equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed. (Use the lowest possible coefficients. Omit states-of-matter in your answer. Your reactionarrow may be either a right arrow (-->) or an equilibrium arrow (<=>), depending upon the value of Keq for the reaction.(a) acetic acid (CH3COOH) and ammoniachemPadX₁X(b) hydrochloric acid and sodium hydroxide(c) nitrous acid and sodium fluoride(Please write the conjugate acid and base separately.)(d) KHSO4 and ammoniaCH3COOH + NH3 CH3COO+NH✔✔CH_3COOH + NH_3 <=> CH_3COO^-+NHCorrect.chemPadX₁X² →→chemPadX.XºHNO₂+ F→ NO₂ + HFHNO_2 + F^---> NO_2^-+ HFCorrect.Greek→ HelpGreek→ HelpH+ + OH → H₂OH^+ + OH^---> H_20Your answer contains an ambiguous or incomplete reaction equation. Check all the components on the product-side of the equation.GreekGreekK = 4.04.03.2e456chemPadXoXº2KH¹+ + 250+ 2N³ + 2H¹+→ 2K¹+ +502 + 2NH ¹ So 22KH^1+ + 2SO_4^2- + 2N^3 + 2H^+1 --> 2K^1+ + SO_4^2- + 2NH_4^1+ SO_4^2-Your answer differs too much from the expected answer to provide useful feedback.→ HelpK= 4.0 1.2e2→ HelpxXK= 4.0 1.0e14 Acid Nameperchloric acidhydrohalic acidsulfuric acidnitric acidhydronium ioniodic acidoxalic acidsulfurous acidhydrogen sulfate ionphosphoric acidhydrofluoric acidnitrous acidlactic acidformic acidhydrogen oxalate ionhydrazoic acidConjugateAcidHCIO4HX (X= I, Br, CI) >>1H₂SO4HNO3H30¹+HIO3H₂C₂O4H₂SO3HSO4¹-H3PO4HFHNO2HC3H5O3HCHO2HC₂04¹-HN3HC₂H3O2H₂CO3HSO3¹-H₂Sacetic acidcarbonic acidhydrogen sulfite ionhydrosulfuric aciddihydrogen phosphate ion H₂PO4¹-hypochlorous acidammonium ionhydrocyanic acidhydrogen carbonate ionHCIO1+| NHAHCN1-HCO3¹->>1>>1>>11.0KapKa Conjugate Base<01-CIO4¹-<0x¹-<01.9 x 10-51.8 x 10-54.3 x 10-71-HSO4¹-1-<0 NO3¹0.00 H₂O0.170.77 103¹-5.9 x 10-21.23 HC₂04¹-1-1.5 x 10-21.82 HSO3¹-1.2 x 10-21.92SO4²-7.5 x 10-32.12 H₂PO4¹-7.2 x 10-43.14 F1-4.0 x 10-43.40 NO₂¹-6.4 x 10-53.85| 1.8 × 10-4| 3.746.4 x 10-5 4.194.724.746.37 HCO3¹-C3H503¹-| CHO2-C₂04²-N3¹-1-C₂H30₂¹-1.0 x 10-77.00 SO3²-1.0 x 10-77.00 HS¹-6.2 x 10-87.21 HPO4²-3.5 x 10-8 7.46 CIO¹-5.6 x 10-10 9.25 NH34.0 x 10-10 9.40 CN¹-4.7 x 10-11 10.33 CO3²-Base Nameperchlorate ionhalide ionhydrogen sulfate ionnitrate ionwateriodate ionhydrogen oxalate ionhydrogen sulfite ionsulfate iondihydrogen phosphate ionfluoride ionnitrite ionlactate ionformate ionoxalate ionazide ionacetate ionhydrogen carbonate ionsulfite ionhydrogen sulfide ionhydrogen phosphate ionhypochlorite ionammoniacyanide ioncarbonate ion

To write the net Equations using the Acid- Base Table and then determine the equilibrium constant…

Use the Acid-Base table to write net equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed. (Use the lowest possible coefficients. Omit states-of-matter in your answer. Your reaction arrow may be either a right arrow (-->) or equilibrium arrow (<=>), depending upon the value of Keq for the reaction.

Use the Acid-Base table to write net equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed. (Use the lowest possible coefficients. Omit states-of-matter in your answer. Your reaction arrow may be either a right arrow (-->) or equilibrium arrow (<=>), depending upon the value of Keq for the reaction.

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...

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Use the Acid-Base table to write net equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed. (Use the lowest possible coefficients. Omit states-of-matter in your answer. Your reaction arrow may be either a right arrow (-->) or an equilibrium arrow (<=>), depending upon the value of Keq for the reaction.
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