Use the References to access important values if needed for this question.Given the following information:Referenceshypochlorous acid HCIOformic acid+HCOOH(1) Write the net ionic equation for the reaction that occurs whenequal volumes of 0.256 M aqueous hypochlorous acid andsodium formate are mixed. It is not necessary to include statessuch as (aq) or (s). Use HCOO as the formula for theformate ion.Submit Answer(2) At equilibrium the(3) The pH of the resulting solution will beKa =3.5x10-8K₂ =1.8x10-4will be favored.+↑ seven. Use the References to access important values if needed for this question.Given the following information:acetic acidReferencesbenzoic acidCH3COOHSubmit AnswerC6H5COOHKa=1.8x10-5Ka=6.3x10-5(1) Write the net ionic equation for the reaction that occurs whenequal volumes of 0.286 M aqueous acetic acid and sodiumbenzoate are mixed. It is not necessary to include states such as(aq) or (s).CH₂COOH + CHCOONaC,H,COOH +|CH,COONa(2) At equilibrium the reactants will be favored.(3) The pH of the resulting solution will be less than↑seven.

Answered: Image /qna-images/answer/65923f62-58ab-490c-8afc-6bb5245e61f3.jpg

Use the References to access important values if needed for this question. References Given the following information: hypochlorous acid HCIO formic acid + HCOOH (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.256 M aqueous hypochlorous acid and sodium formate are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO™ as the formula for the formate ion. K₂ = 3.5x10-8 Ka = Ка 1.8x10-4 (2) At equilibrium the (3) The pH of the resulting solution will be will be favored. + Ⓒseven.

Use the References to access important values if needed for this question. References Given the following information: hypochlorous acid HCIO formic acid + HCOOH (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.256 M aqueous hypochlorous acid and sodium formate are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO™ as the formula for the formate ion. K₂ = 3.5x10-8 Ka = Ка 1.8x10-4 (2) At equilibrium the (3) The pH of the resulting solution will be will be favored. + Ⓒseven.

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

Acetylsalicylic acid (C₂H8O4) is a monoprotic acid commonly known as aspirin. A typical aspirin tablet, however, contains only a small amount of the acid. In an experiment to determine its composition, an aspirin tablet was crushed and dissolved in water. It took 5.10 mL of 0.1466 M NaOH to neutralize the solution. Calculate the number of grains of aspirin in the tablet. (One grain = 0.0648 g and the molar mass of aspirin = 180.15.) mol Round your answer to 3 significant digits. grains ☐ ☐x10
Write the molecular equation, the total ionic equation (TIE) and the net ionic equation (NIE) for the reaction of aqueous solutions: phosphoric acid and sodium hydroxide.
Given the following information: hypochlorous acid HCIO formic acid НСООН HCOOH is a stronger acid than HCIO (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.078 M aqueous hypochlorous acid and sodium formate are mixed. It is not necessary to include states such as (aq) or (s). Use HC00 as the formula for the formate ion. + + (2) Which is the strongest base, CIO or HCOO ? (3) At equilibrium the will be favored.
Calculate the concentration of S2- in an aqueous solution of 0.239 M hydrosulfuric acid, H2S (aq). [S2*] = M.
An aqueous solution of Ca(OH)2with a concentration of 0.188 M was used to titrate 25.00 mL of aqueous HCl. 18.63 mL of the Ca(OH)2was required to reach the endpoint of the titration. How many moles of base were required to react completely with the acid in this reaction? How many moles of HCl were present in the original 25.00 mL of acid?
Balance the following equations and then write the net ionic equations. (Use the lowest possible whole number coefficients. Include states-of-matter in your answers. Use H+ instead of H3O+ to balance equations. Write weak electrolytes in their undissociated form. Leave any extra answer blanks empty. Omit any coefficients of 1.) (a) (NH4)3PO4 (aq) + Bi(NO3)3(aq) → BiPO4(s) + NH4NO3(aq) balanced equation + net ionic equation (b) AgOH(s) + H₂SO4 (aq) → Ag₂SO4(s) + H₂O(1) balanced equation net ionic equation net ionic equation (c) HCN (aq) + Co(OH)3 (s) → Co(CN)3(aq) + H₂O(1) balanced equation + + + + + ↑ + + + +
An aqueous solution of a strong monoprotic acid (HA) contains 0.550 g of acid and is completely neutralized by 25.0 mL 0f 0.100 M Mg(OH)2 solution. Calculate the molecular mass of acid.
The antacid found in Tums™ has the active ingredient calcium carbonate, which undergoes a reaction when mixed with hydrochloric acid to produce water, calcium chloride and carbon dioxide. A tablet of this antacid had a mass of 1.774g and was dissolved completely in an excess of 30.0mL of 0.794M HCl. The resulting solution was then titrated with 0.995M NaOH. The initial buret reading was 11.05mL and the final buret reading was 28.52mL. The listed mass of active ingredient on the bottle is 325mg. a. What is the calculated mass of active ingredient in this tablet? b. What is the percent error from the listed mass? c. What percent of the tablet is inert (non-active) ingredients? explain in detail
Calculate the number of H+(aq)H+(aq) ions in 1.6 mLmL of pure water at 25 ∘C∘C. Express your answer using two significant figures. N=
Na2CO3 (aq) + HCI (aq) -> Complete ionic equation : Net ionic equation :
What is the concentration of a solution of a diprotic acid (i.e., H2A) which required 19.25 mL of 0.0965 M KOH to titrate 15.00 mL of the acid solution? Report the answer with the correct number of significant figures.
Complete and balance the following formula equation for the reaction below. Write the complete ionic equation and the net ionic equation. All equations must be balanced and include phases (s, I, g, or aq). Formula Eq: КОН (aq) MnBr3 (aq) --- Total lonic: Net lonic: