Iodous acid (HIO,) is a weak acid that dissociates in water as follows.HIO,(aq) + H,0(1)=H;0*(aq) + I02 (aq)The acid-dissociation constant (K) for iodous acid is 3.2x10-5. Calculate the percent ionization (percentdissociation) if the initial concentration of iodous acid was 0.35 M.Step 1 of 5Recall the relationship between an acid's dissociation constant (K) and its percent ionization (percentdissociation).[H,0*1eequilibrium x 100%% ionization of an acid =[HA]initialIn this equation, [HA]nitial is the initial concentration of the acid in molarity and [H,0*]equilibrium is theconcentration of H,0+ ions at equilibrium in molarity. Before calculating the percent ionization, the K,ofiodous acid must be used to find the following.O [H,0*]initialO [HAJequilibrium[HA]initial[H,0*]equilibriumStep 2 of 5Write the acid dissociation constant expression for this given reaction.HIO,(aq) + H,0(1) =H,0*(aq) + I0, (aq)The acid dissociation constant expression for the reaction of HIO, with water is the following. (Concentrationequilibrium expressions take the general form: K. = [C]° / [A]ª . [B]°. Subscripts and superscripts thatinclude letters must be enclosed in braces {}.)chemPadHelpGreek -H20H_20Your answer differs too much from the expected answer to provide useful feedback.Note that the concentrations expressed in the acid dissociation constant are equilibrium concentrations, whichmust be determined.Write the expression for the acid-dissociation or base-dissociation constant for a specified weak acid or base.

Given: Concentration of HIO2 = 0.35 M Ka of HIO2 = 3.2x10-5

Iodous acid (HIO,) is a weak acid that dissociates in water as follows. HIO,(aq) + H,0(1) ==H;0*(aq) + 10, (aq) The acid-dissociation constant (K.) for iodous acid is 3.2x10-5. Calculate the percent ionization (percent dissociation) if the initial concentration of iodous acid was 0.35 M. Step 1 of 5 Recall the relationship between an acid's dissociation constant (K) and its percent ionization (percent dissociation). [H,0*lequilibrium x 100% [HA]initial % ionization of an acid = In this equation, [HA]initial is the initial concentration of the acid in molarity and [H,0*]equilibrium is the concentration of H,0+ ions at equilibrium in molarity. Before calculating the percent ionization, the K, of iodous acid must be used to find the following. O [H,0*linitial O [HAJequilibrium O [HAJinitial [H,0*]equilibrium Step 2 of 5 Write the acid dissociation constant expression for this given reaction. HIO (2a) t H O O = H ot(aa) 1 TO -( ag)

Iodous acid (HIO,) is a weak acid that dissociates in water as follows. HIO,(aq) + H,0(1) ==H;0(aq) + 10, (aq) The acid-dissociation constant (K.) for iodous acid is 3.2x10-5. Calculate the percent ionization (percent dissociation) if the initial concentration of iodous acid was 0.35 M. Step 1 of 5 Recall the relationship between an acid's dissociation constant (K) and its percent ionization (percent dissociation). [H,0lequilibrium x 100% [HA]initial % ionization of an acid = In this equation, [HA]initial is the initial concentration of the acid in molarity and [H,0]equilibrium is the concentration of H,0+ ions at equilibrium in molarity. Before calculating the percent ionization, the K, of iodous acid must be used to find the following. O [H,0linitial O [HAJequilibrium O [HAJinitial [H,0*]equilibrium Step 2 of 5 Write the acid dissociation constant expression for this given reaction. HIO (2a) t H O O = H ot(aa) 1 TO -( ag)

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

9//identify each substance Acid Base conjugate acid Conjugate base
101 Chem101 A app.101edu.co 出 Apps M Apps UT Blackboard 22 Calendar E Reading List >> Question 14 of 24 Submit Consider the reaction below. Which species are conjugate acid/base pairs? HSO, (aq) + HCN (aq) = H,SO, (aq) + CN (aq) A) HSO,, CN B) HSO,, H,SO, C) H,SO,, CN D) HCN, H,SO, Prac Q: W A: Se Q: W A: Se MacBook Air esc 888 F1 F2 F3 F4 F5 F6
At 25 °C, how many dissociated OH ions are there in 1221 mL of an aqueous solution whose pH is 1.26? number of OH ions: ion
Fill in the blanks: 1. Zn"(ag) + 4 NH3(aq) = Zn(NH3),²"(aq) 2. SO-(g) + H20()=H;SO3(aq) In equation 1, the Lewis acid is because it electron pairs to/from In equation 2, the Lewis base is because it electron pairs to/from
Acids & Bases: Understanding Connections Between Descriptions of Weak Acid Dissociation In an aqueous solution of a certain acid the acid is 0.054% dissociated and the pH is 4.49. Calculate the acid dissociation constant Ka of the acid. Round your answer to 2 significant digits.
7/identify each substance Acid Base conjugate acid Conjugate base
The pH of a 1.2M solution of hexanoic acid (HC H,,0,) is measured to be 2.39. Calculate the acid dissociation constant K, of hexanoic acid. Be sure your answer has the correct number of significant digits. K a x10
Calculate the pH, pOH, and the fraction of protonated acid for the 0.1 M solution of lactic acid (see Table 4.4 for pk3 values, also attached below).
4
Ką for acetylsalicylic acid (aspirin), HC,H-O4. is 3.0010-4. Ką for hypochlorous acid, HC1O, is 3.50x10-8. Ką for hydrocyanic acid, HCN, is 4.00×10-10. What is the formula for the weakest conjugate base?
For the reaction CH3COOH + NaOH ------> CH3COO- + Na+ , if CH3COOH is a weak acid and NaOH is a strong base, which of the following is a true statement Group of answer choices CH3COO- is a strong base, Na+ is a strong acid CH3COO- is a strong base, Na+ is a weak acid CH3COO- is a weak base, Na+ is a strong acid CH3COO- is a weak base, Na+ is a weak acid
Niacin, one of the B vitamins,has the molecular structureshown at the right. A 0.020 Msolution of niacin has a pH of3.26. What is the acid-dissociationconstant for niacin?