A solution of a weak acid, HA, has [HA] = [A¹] = 0.333 M. If the acid dissociation constant for the equilibrium reaction shown below is 1.9 x 10-4, find the pH of the solution. HA + H₂0 H30++ A¯ Your Answer: Answer

A solution of a weak acid, HA, has [HA] = [A¹] = 0.333 M. If the acid dissociation constant for the equilibrium reaction shown below is 1.9 x 10-4, find the pH of the solution. HA + H₂0 H30++ A¯ Your Answer: Answer

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 66QRT: Complete each of these reactions by filling in the blanks. Predict whether each reaction is...

See similar textbooks

Related questions

Q: The acid-dissociation constant, Ka, for a particular acid is 4.57 x 10. What is the…

A: We know that, Ka × Kb =10(-14) Given that, Ka = 4.57 × 10(-3) So,

Q: For the diprotic weak acid H2A, Kal = 3.8 × 10-6 and K2 = 7.8 x 10-9. What is the pH of a 0.0750 M…

Q: In ammonia stripping, hitrogen is removed from wastewater by volatilization of NH3. Would ammonia…

Q: For the diprotic weak acid H₂A, Kal What is the pH of a 0.0750 M solution of H₂ A? pH = = = 3.7 ×…

A: Given, The concentration of H2A = 0.0750 M. Ka1 = 3.7 × 10-6 and Ka2 = 5.4 × 10-9 The pH of the…

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

Q: The weak base methylamine, CH3NH2, has Kb= 4.2 x 10-4 . It reacts with water according to the…

A: Given: Kb= 4.2 x 10-4 Equation reaction: CH3NH2(aq) + H2O(ℓ) ⇌ CH3NH3+(aq) + OH-(aq) Concentration…

Q: What is the [H3O+] in a solution with a pH of 8.66? Group of answer choices 2.2 × 10-9 M 1.5 × 10-5…

Q: What is the pH of a 0.00138 M hypochlorous acid (HClO) solution? Ka = 3.5 * 10-8 Report your answer…

Q: H₂SO3 is a diprotic acid with Kal = 1.6 × 10°² and K₁2 = 6.4 × 10-8 What is the equilibrium constant…

A: When we subtract two equations; value of equilibrium constant gets divided.Equilibrium constant is…

Q: If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.210 M, determine the carbonic…

A: Carbonate buffers are important in regulating the pH of blood.Given,the carbonate concentration in a…

Q: A 0.60 M solution of a weak acid, HA, has a pH of 3.41. What is the percentage ionization of the…

A: ★ Answer : percentage of ionization of the acid is 0.064%

Q: HCN

A: When we add NaCN in HCN then pH will change .

Q: Which of the following is the weakest acid? HCN ( Ka = 4.9 × 10-¹⁰) HF (Ka = 6.8 × 10−4) OHCIO (Ka =…

A: pKa value: pKa value negative logarithm of the acid dissociation constant (Ka). pKa = -logKa Low pKa…

Q: Four solutions of an acid dissolved in water are sketched below, as if under a microscope so…

A: The strength of different acids can be compared on the basis of the degree of dissociation of these…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: pH + pOH =14

Q: Which of the following K values would indicate the weakest base of the group? O 1.2 x 109 O 6.3 x…

A: Ans:- (1.2×10-9 is the weakest base of the group).

Q: Sodium bisulfate, NaHSO4, is used in some household cleansers as a source of HSO4- ion, a weak acid.…

A: The objective of the question is to find the pH of fully dissociated acid and undissociated acid .

Q: Calculate pH and pOH for each of the following solutions and determine whether thesolution is…

A: The objective of the question is to calculate the pH and pOH of the given solutions and determine…

Q: A weak acid, HA, has a K₁ = 7.76x10-3. What is the pH of a solution with [HA] = 0.236 M and [NaA] =…

A: The pH of a mixture of a weak acid (HA) with its conjugate base (A-) is calculated using the…

Q: A weak acid has K a = 1.00 × 10 -3. If [HA] = 1.00 M what must be [A -] for the pH to be 2.7?

A: Henderson Hassel Balch equation is given below.

Q: What is the pH of a 0.0100 M solution of acetic acid? Ka=1.8x10-5

A: Dissociation of acetic acid can be written as; CH3COOH → CH3COO- + H+ Given that concentration of…

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

A solution of a weak acid, HA, has [HA] = [A¹] = 0.333 M. If the acid dissociation
constant for the equilibrium reaction shown below is 1.9 x 10-4, find the pH of the
solution.
HA + H₂0 H30++ A¯
Your Answer:
Answer

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step by step

Solved in 4 steps

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

The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107
Find the concentration of A − for the generic acid dissociation reaction:HA(aq) + H2O(l) A(aq) − + H3O(aq)+ With [HA] = 0.150 M, [H2O] = 0.100 M, [A −] = 0.000 M and [H3O +] = 0.0000 M
A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) + H₂O(1) ⇒ H₂O*(aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] [A-] = 2.00 × 10-4 M. Calculate the Ką value for the acid HA. Ka = = 0.260 M, [H3O+] = 2.00 × 10-4 M, and
Part A At 25 °C phosphoric acid, H3PO4, has the following equilibrium constants: What is the pH of a solution of 0.25 mol L K3PO4, potassium phosphate? 7.5 x 10-3 6.2 x 10 8 Ka К Express your answer numerically to the hundredths place. Km 4.2 x 10 13 • View Available Hint(s) ? pH = Submit Part B What is the pH of a solution of 0.300 mol L-1 K,HPO,, potassium hydrogen phosphate? Express your answer numerically to the hundredths place. • View Available Hint(s) pH = Submit Part C What is the pH of a solution of 0.500 mol L-1 KH,PO4, potassium dihydrogen phosphate? Express your answer numerically to the hundredths place. • View Available Hint(s) pH = Submit
What is the equilibrium constant for the following reaction equal to? H+(aq) + OH−(aq) ⇌ H2O(l) Group of answer choices Kw 1 / Kw Ka Kb Kp
If AG° < 0, then at equilibrium there will be more products than reactants. false true
-10 The acid dissociation constant K of boric acid (H,BO, is 5.8 x 10 . Calculate the pH of a 6.0 M solution of boric acid. Round your answer to 1 decimal place. PH pH = ?
Activity 3: pH and pOH Calculation Fill in the missing information in the table below. On a separate paper, show your complete solution. pH [H'] pOH [OH] 5.39 х 10-12 М Acid or Base? 12.24 9.22 x 10-8 M 11.68 9.87 x 10-3 M 1.33 4.73 x 10-10 М 7.05 8.53 x 10-7 M 3.82
The ionization constant, Ka, for weak acid, HA, is 3.96 × 10-10, What is the pH of a 0.5213 M solution of this acid? The equation for the ionization of weak acid HA as follows. HA (aq) + H2O(1) =H3O+(aq) + A (aq) Report your answer with two places past the decimal point. (Hint: Use an ICE table.) Tyne vour answer.
QUESTION 7 Determine the acid dissociation constant, Ka, for a 0.10 Ma weak acid solution that has a pH of 2.87. HA, is a weak.monoproticacid and the equilibrium equation of interest is HA(ag) + H20()= H30*(aq) + A (ag) Enter your answer in exponential format using a capital "E" (example 1.23E-4) and no units (value + 2%).
Calculate the pH at 25 °C of a 0.81M solution of potassium acetate (KCH3CO2). Note that acetic acid (HCH 2 CO2) is a weak acid with a pк pK of 4.76. Round your answer to 1 decimal place. pH = ☐
Calculate the pH of a 0.50 M solution of oxalic acid (H2C2O4) given the equilibrium constants below. Ka1 = 5.9 × 10–2 Ka2 = 6.4 × 10–5 Enter your response in pH units to the nearest 0.01.