A monoprotic weak acid (HA) has a \( pK_a \) value of 4.435. Calculate the fraction of HA in each of its forms (HA, \( A^- \)) at pH 5.659.\[\alpha_{HA} = \quad \quad \alpha_{A^-} =\]What is the quotient \(\frac{[A^-]}{[HA]}\) at pH 5.659?\[\frac{[A^-]}{[HA]} = \] **Exercise: Calculating Ion Concentrations****Task:**Calculate the concentrations of hydronium ions, \( \text{H}_3\text{O}^+ \), and hydroxide ions, \( \text{OH}^- \), for a 0.0285 M HCl solution.**Inputs:**- [\( \text{H}_3\text{O}^+ \)] = **1.545 M** (Incorrect)- [\( \text{OH}^- \)] = **12.45 M** (Incorrect)**Instructions:**Enter the correct numeric values for each ion concentration in the provided fields. The current entries are incorrect; reassess the calculations based on the given HCl concentration.Understanding the dissociation of HCl in water and the resulting impact on ion concentrations is crucial:- Remember that in a solution, \( \text{HCl} \) completely dissociates to produce equal concentrations of \( \text{H}_3\text{O}^+ \).- Utilize the water dissociation constant, \( K_w \), to calculate \( \text{OH}^- \).**Note:** This exercise helps to reinforce the concept of pH and equilibria in aqueous solutions.

Answered: Image /qna-images/answer/0be0f48d-e36a-4c4b-a2b6-1373d352abcc.jpg

Answered: 20 A monoprotic weak acid (HA) has a pK…

20 A monoprotic weak acid (HA) has a pK value of 4.435. Calculate the fraction of HA in each of its forms (HA, A¯) at pH 5.659. αHA = What is the quotient [A-] = [HA] [A-] at pH 5.659? [HA] αA- =

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 a 0.143 M solution of H2C6H6O6, calculate both the pH and the C6H6O62- ion concentration. H2C6H6O6 + H2O H3O+ + HC6H6O6- Ka1 = 7.9×10-5 HC6H6O6- + H2O H3O+ + C6H6O62- Ka2 = 1.6×10-12 pH = [C6H6O62-] = M
Which of the following statements are FALSE? Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation. SHOW MORE V If the pKa for formic acid is 3.75 the ratio of formate (A) to formic acid (HA) at pH 4.15 is 5:1. The pH of 1 liter of water to which is added 10 ml of 5.0 M HCl is 1.3. If an acid has a pka of 4.76 the Ka =0.00001. The pH of 1 liter of water to which is added 10 ml. of 0.50 M NAOH is 11.0. The pH of a 1 liter solution to which has been added 6.0 mL of 1.5 M acetic acid and 5.0 ml of 0.4 M sodium acetate is 6.0. to
5. Use the following reaction to answer each part of this question: NaCN + OH HCN + iona ONa (a) Label the acid, base, conjugate acid, and conjugate base. (b) What is the pKa of the acid and of the conjugate acid? (c) What is the strongest acid in this reaction? (d) Does the equilibrium lie to the left (toward reactants) or to the right (toward products)?
What is the equilibrium-constant expression of the basic dissociation of NaNO2? Kb = ([HNO2] [NO2])/[OH-] %3D Kb = ([NO2] [OH-])/[HNO2] %3D Kb = ([HNO2] [OH-])/[NO2] Kb = [OH-J/([HN02] [NO2])
You make a solution of a weak acid with a pH of 3.75 and the pKa is 5.42 1. Is the solution acidic or basic? 2. Calculate the [H3O+]. 3. Calculate the pOH 4. Calculate the [OH-] HO(sc) OM (0+1) 5. Calculate the pKb DM 6. Calculate the Kb. 041 halched 109
The pKa of acetic acid is 4.75. What is the ratio of the concentration of sodium acetate to the concentration of acetic acid at pH 5.75? equation: ch3cooh (aq)+oh-(aq) = ch3coo-(aq)+h20(l)
Pp
A diprotic acid (H₂A) has pKa values of 4.20 (pKal) and 8.40 (pKa2). Which of the equalities is true when the pH is 4.20? O [HA] = [A²-] O [H₂A] = [A²-] O [H₂A] = [HA¯] What is the predominant species of H₂A at pH 2.52? HA O H₂A O A²- What is the predominant species of H₂A at pH 10.50? HA 2- Which of the equalities is true when the pH is 8.40? O [H₂A] = [HA] O [HA] = [A²-] O [H₂A] = [A²-] What is the predominant species of H₂A at pH 7.01? O A²- O H₂A O HA™
What is Kb of B? What is the pH of a 0.05 M solution of B?
Phenylacetic acid (C₂H₂CH₂COOH) has a K₂ of 4.9 x a 10-5. Calculate for the pH, pOH, [H+] and [OH-] of a solution of phenylacetic acid that is 0.186 M.
The diprotic acid, H2A, has Ka1 i.e. (K1) = 1.00 X 10-4 and K2 = 1.00 X 10-8.
The pH of a 0.62M solution of 4-chlorobutanoic acid (HC4HO₂C1) is measured to be 2.37. Calculate the acid dissociation constant K of 4-chlorobutanoic acid. Round your answer to 2 significant digits. a a 0 x10 X Ś