The ionization constant of a very weak acid, HA, is 6.6x10-⁹. Calculate the equilibrium concentrations of H3O+, A, and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O+] [A] = [HA] pH = = = mol/L mol/L mol/L

The ionization constant of a very weak acid, HA, is 6.6x10-⁹. Calculate the equilibrium concentrations of H3O+, A, and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O+] [A] = [HA] pH = = = mol/L mol/L mol/L

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

Related questions

Q: Calculate the concentrations of all species in a 0.940 M Na, SO, (sodium sulfite) solution. The…

Q: Write the equilibrium constant expression for this reaction: 2 H+ (aq) +SO² (aq) → H₂SO4(aq) 4

A: Equilibrium constant is the ratio of the equilibrium concentrations of product over equilibrium…

Q: calculate the equilibrium constant for the reaction

A: We are given concentrations of H+ and Al(H2O)5OH2+ are found to be (2.74x10^-3) M (1.3x10^-1) M in…

Q: 101. The pH indicator phenol red turns pink or magenta when the pH of the medium becomes more (basic…

A: Note: Since you have posted a question with multiple subparts, we will solve the first three…

Q: For the diprotic weak acid H₂A, K₁1 = 2.1 x 106 and K₁2 = 7.6 x 10-⁹. What is the pH of a 0.0400 M…

A: pH is a measure of how acidic/basic water is. The range goes from 0 - 14, with 7 being neutral. pH…

Q: Write the concentration equilibrium constant expression for this reaction. + 3+ Cr,0, (aq)+61…

A: Given equation: Cr2O72- (aq) + 6I-(aq) + 14H+ (aq) → 3I2 (s) + 2Cr3+ (aq) + 7H2O (l) We have to…

Q: In a neutral solution, the [H3O+(aq)] is greater than/equal to/less than 1 x 10-7 mol/L. A sample of…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: Write the equilibrium constant expression for this reaction: NH(aq) → NH3(aq) + H+ (aq) - x Ś

A: The objective of the question is to write the equilibrium constant expression for the given chemical…

Q: A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) + H₂O(1) ⇒…

Q: Reaction: HCl + NaOH → NaCl + H2O End point pH: 8.00PH Equivalence point (using your graphs) pH:…

A: To determine the molarity of NaOH at both the end point and the equivalence point, we need to use…

Q: Muscles produce lactic acid, CH, CH(OH)COOH(aq), during exercise. Calculate the percent ionization…

Q: The hydronium ion concentration of an aqueous solution of 0.43 M formic acid, HCOOH is [H3O+] =…

Q: Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution…

Q: Calculate the concentrations of all species in a 0.450 M Na, SO, (sodium sulfite) solution. The…

A: Na2SO3 ---- 2Na+ + SO32-

Q: Weak Acids dissociate according to the following equation: HA(aq) + H2O(L) ⇌ H3O+ (aq) + A-(aq) In…

Q: Calculate the concentrations of all species in a 0.940 M Na, SO, (sodium sulfite) solution. The…

Q: In the laboratory, a general chemistry student measured the pH of a 0.429 M aqueous solution of…

Q: consider the following equilibrium. CrO4(aq) + 2H(aq) Cr2O7(aq) + H2O(l) (yellow)…

A: Le Chatelier's principle: According to the Le Chatelier's principle when a change in concentration…

Q: There is a buffer solution containing 0.50 M acetic acid (CH3COOH, Ka= 1.8 X 10-5) and 0.50 M sodium…

A: A buffer is used to maintain the pH of the solution when the addition of acid or base is done. pH of…

Q: Write the equilibrium constant expression for this reaction: NH(aq) → NH3(aq) +H* (aq) X 믐 5

A: The objective of the question is to write the equilibrium constant expression for the given chemical…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

Q: Write the concentration equilibrium constant expression for this reaction. CN (aq) +H₂O(1)→HCN(aq)…

Q: Percent ionization for a weak acid (HA) is determined by the following formula: [HA] ionized [HA]…

A: we have to calculate the percent ionization

Q: A weak acid, HA, undergoes only partial ionization in water: HA (aq) + H2O (I) → H3O* (aq) + A (aq)…

A: • The ionisation of weak acid, HA is, HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq) • We need to write…

Q: Which of the following is true of a buffer solution that contains equivalent amounts of acid and…

A: buffer solution that contains equivalent amounts of acid and conjugate base means [Conjugate base ]…

Q: Formic acid, HCOOH, is the simplest of the carboxylic acids and occurs naturally, most notably in…

Q: Write the equilibrium constant expression for this reaction: NH(aq) → NH3(aq) + H+ (aq) - x Ś

A: The objective of the question is to write the equilibrium constant expression for the given chemical…

Q: Muscles produce lactic acid, CH₂ CH(OH)COOH(aq), during exercise. Calculate the percent ionization…

Q: 0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium,…

A: Given: Initial moles of HA = 0.030 moles Volume of container = 2.0 L Equilibrium concentration of HA…

Q: Calculate the concentrations of all species in a 1.01 M Na₂SO3 (sodium sulfite) solution. The…

A: Given that: Concentration of Na2SO3 = 1.01 M Ionization constants of H2SO3, Ka1 = 1.4 x 10-2 M and…

Q: Write the equilibrium constant expression for this reaction: 2 H(aq) +SO (aq) → H₂SO4(aq) 1 0

Q: A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) → H+ (aq) + A¯(aq)…

Q: Acetylsalicylic acid (aspirin), HC9H7O4, is the most widely used pain reliever and fever reducer.…

Q: The ionization constant of a very weak acid, HA, is 1.9×109. Calculate the equilibrium…

Q: Write the concentration equilibrium constant expression for this reaction. F (aq)+H,O*…

Q: You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization…

A: Applying similar concept of kw and pH as like water because it also involves in auto ionisation like…

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

The ionization constant of a very weak acid, HA, is 6.6×10-⁹ . Calculate the equilibrium
concentrations of H3O+, A¯, and HA in a 0.040 M solution of the acid.
Determine the concentrations of all species at equilibrium and the solution pH.
[H3O+]
[A] =
[HA] =
pH
=
=
Submit
mol/L
mol/L
mol/L
Show Approach Show Tutor Steps

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

HA is a weak acid. Select the correct dropdown value to correctly complete the incomplete concentration table below being used to determine the equilibrium concentrations of HA, H3O*, and A¯ of a 0.1300 M HA solution that has a pH of 3.60 at 25°C. HA(aq) + H,0(1) = H,0^(aq) + A-(aq) Initial 0.1300 Change Equilibrium (b) (a] The value for a is [ Select ] The value for b is [ Select ] What is the Ka of this weak acid? [ Select]
Consider two aqueous solutions of equal concentration: chlorous acid (HCNO, K, = 2.0 x 10 4) and acetic acid (CH3COOH, K, = 1.77 x 10-5). Which statement is true when the solutions are at equilibrium? %3! O CNO produces more [OH ] than CH3COO O HCNO produces less [H3O*] than CH3COOH O The pH value of HCNO solution is the same as that of CH3COOH solution. O HCNO produces more [H3O*] than CH;COOH O The pH value of HCNO solution is higher than that of CH3COOH solution.
5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.
Write the equilibrium for the autoionization of sulfuric acids (H 2 SO 4 ) and write the expression for the equilibrium constant for this process.
Write the equilibrium constant expression for this reaction: NH(aq) → NH3(aq) + H+ (aq) - x Ś
HA, a weak acid, also forms the ion HA, in solution. The reaction is HA(aq) + A (aq) = HA, (aq) The weak acid has K, = 8.64 × 10-7 and the reaction has K = 3.80. Calculate the concentrations of A, H*, and HA, in a 1.00 M solution of HA. [A¯] = M [H*] = M [HA,] = M
Calculate the pH of a 3.5 M solution and the equilibrium concentrations of the species H3PO4, H2PO4- , HPO4-2, and PO4-3 (Ka1= 7.5 x 10-3, Ka2= 6.2 x 10-8, Ka3= 4.8 x 10-13)