--chlorous acid hydrocyanic acid lactic acid nitrous acidOrder these acids from weakest to strongest.D <11HCIO,<1.2x10-2HCN4.9×10-10E<HC,H,O,5(weakest)Order the conjugate bases for these acids from weakest to strongest.(weakest)

Given the values of Ka along with the acids: We will determine the answers by the value of Ka as :…

chlorous acid hydrocyanic acid lactic acid nitrous acid < HCIO, Order these acids from weakest to strongest. 1.2×10 ² -- < < HCN -- 4.9×10-10 HC HẠO, (weakest) Order the conjugate bases for these acids from weakest to strongest. (weakest) Order 0.150 M solutions of each acid above from lowest to highest pH. (lowest) (highest) Order 0.150 M solutions of each acid above from lowest to highest percent dissociation. (lowest) #< (highest) 1.4×10-4 HNO₂ 4.6x104 (strongest) (strongest)

chlorous acid hydrocyanic acid lactic acid nitrous acid < HCIO, Order these acids from weakest to strongest. 1.2×10 ² -- < < HCN -- 4.9×10-10 HC HẠO, (weakest) Order the conjugate bases for these acids from weakest to strongest. (weakest) Order 0.150 M solutions of each acid above from lowest to highest pH. (lowest) (highest) Order 0.150 M solutions of each acid above from lowest to highest percent dissociation. (lowest) #< (highest) 1.4×10-4 HNO₂ 4.6x104 (strongest) (strongest)

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

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
Calculate the equilibrium concentration of the nonionized bases and all ions in a solution that is 0.115 M in NH3 and 0.100 M in C6H5NH2.
Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. CH;C00 HCN (aq) CHĄCOOH CN Brønsted-Lowry | Brønsted-Lowry Brønsted-Lowry | Bronsted-Lowry { In this reaction: The formula for the conjugate )of CH3COO¯ is The formula for the conjugate| of HCN is
4. Describe the procedure and show the mathematics required to determine the K. for the conjugate acid of a weak base.
For each of the following strong base solutions, determine OH-| and (H30+] and pH and РОН For 2.2 x 10-4 M KOH, determine [OH ] and (H30+). Express your answers in moles per liter to two significant figures separated by a comma. • View Available Hint(s) [OH-], [H3O*] = 2.2×10-44.5×10-11 M Previous Answers Correct Term 2: Correct answer is shown. Your answer 4.57-10-11 = 4.57x10-11 M was either rounded differently or used a different number of significant figures than required for this part. Important: If you use this answer in later parts, use the full unrounded value in your calculations. KOH is a strong base that completely dissociates into K+ and OH in an aqueous solution: KOH(aq) → K*(aq) + OH- (aq) Therefore, the concentration of OH is the same as the given concentration of KOH and is equal to 2.2 x 10-1 M. Then use the ion product constant, substitute the calculated value for OH, and solve for (H3O*]:
Consider the following reaction. Which are conjugate acid/base pairs? HNO2(aq) + HS-(aq) ----> H2S(g) +NO2-(aq) HNO2 & H2S HNO2 & HS^- HNO2 & NO2^- H2S & NO2^- HS^- & NO2^-
If the ?a of a monoprotic weak acid is 5.7×10^−6 ,what is the pH of a 0.27 M solution of this acid? Remember there are special significant figure rules you need to use when dealing with logs.
If Kb for the dissociation of HSO4- is 1.2 x 10^-2 , what is the pH of a solution containing equal quantities of SO4^2- and HSO4-?
If the pH of a 0.800 M solution of an acid is 3.45, calculate the % ionization of this acid and ka of this acid. PH = 3.45M = 0.800
the pH of a 0.012 M weak acid solution is 3.75. what is the percent ionization for this acid?