Determine the pH of each of the followingsolutions.(a) 0.549 M hydrogen peroxide (weak acid withКа 3 2.4e-12).(b) 0.615 M acetic acid (weak acid with Ka1.8e-05).(c) 0.866 M pyridine (weak base with Kp = 1.7e-09).

Answered: Image /qna-images/answer/6519f0e7-c8d4-4d17-9203-fe1fee651903.jpg

Determine the pH of each of the following solutions. (a) 0.549 M hydrogen peroxide (weak acid with Ka = 2.4e-12). (b) 0.615 M acetic acid (weak acid with Ka = 1.8e-05). (c) 0.866 M pyridine (weak base with Kb = 1.7e- 09).

Determine the pH of each of the following solutions. (a) 0.549 M hydrogen peroxide (weak acid with Ka = 2.4e-12). (b) 0.615 M acetic acid (weak acid with Ka = 1.8e-05). (c) 0.866 M pyridine (weak base with Kb = 1.7e- 09).

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.71PAE: Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’....

See similar textbooks

Related questions

Q: Calculate the pH of a 0.13 M solution of propanoic acid. K, of propanoic acid is 1.3 x 10-5.

A: pH is defined as negative logarithm of hydrogen ion concentration.

Q: 6) If the hydroxide ion concentration of a solution is 1.0 x 10° M Is it an acidic or basic…

Q: Hldes if heeded for this question. The pH of an aqueous solution of 0.274 M sodium acetate, NaCH3COO…

Q: The pH of a solution containing a [H3O+] = 3.40 x 10 negative 5 M, is:

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: What is the pH of a 0.0810 M solution of HONH;CI (Kb of HONH2 is 1.1 x 108)?

A: Given, HONH3Cl -----> HONH3+ + Cl- Hydrolysis of the weak conjugate acid, HONH3+…

Q: The pH of an aqueous solution of 4.45x102 M ammonium bromide, NH,Br (aq), is This solution is

A: NH4Br is a salt of weak base and strong acid. We have to determine pH of an aqueous solution of…

Q: What is the pH of a 0.0520 M solution of HONH;CI (Kb of HONH2 is 1.1 x 10-8)?

A: HONH3Cl is a salt of weak base HONH2 and strong acid HCl Recall the following expression to…

Q: Calculate the pH of 1.1 M C3H7COOH(aq) given that its Ka = 1.5×10-5. Provide your answer in decimal…

A: First of all, we need to find out the Degree of dissociation (alpha).…

Q: Determine both the pH and the % ionization of a 0.53 M hypochlorous acid, HCIO, solution at 25°C.…

A: The given data is as follows: The concentration of HClO = 0.53 M The value of Ka for HClO = 2.9×10-8…

Q: Determine the pH level of a solution that has 0.05385 M of Pyridine, given that the Kb of pyridine…

A: Given, Concentration of the Pyridine solution (C) = 0.05385 M Kb for pyridine = 1.620 x 10-6 Note:…

Q: Given that the pH of a solution is 6.7, what is the [H3O+]?

A: Since pH = -log[H3O+]

Q: Calculate the pH of the following solutions in which the [H+] is a) 0.01, b) 1.0 x 10 –8 , and c)…

A: Given that - Hydrogen ion concentration , [H+] are - a) 0.01 b)1.0 x 10 –8 c) 4.67 x 10 –4 Then,…

Q: calculate the pH of the solution eith an H+1 concentration of 2.90×10-12 and identify the solution…

A: Given, The concentration of H+ = 2.90 × 10-12 M The pH of the solution is:

Q: A scientist notices an occurrence of acid shock in a body of water that sits close to an in-…

Q: The pH of a solution of 0.63 M pyridine is 9.51, what is the Kb of pyridine? What is the Ka of its…

Q: The pH of 0.01 m Potassium hydrogen phthalate is

Q: In a solution of 0.015 mol L-1 HBr(aq) at 25 °C (a) What are the concentrations of the hydronium,…

A: pH stands for the potential of hydrogen ion concentration or power of hydrogen. The pH of an aqueous…

Q: How do I calculate pH of a salt? for example in 0.10 M NaClO4(aq)?

A: Salt are produced by the reaction of an acid and a base. For example, The pH of salt is given as :

Q: Determine the pH of a solution that is 0.00372 M HCl and 0.0240 M HCIO,. The K, of HCIO, is 1.1 x…

A: pH is the negative logarithm of hydronium ion concentration. It is used to measure the acidic or…

Q: A weak base is dissolved in water with a concentration of 0.200 mol/L. The Kb value of the base is…

A: Given :- initial concentration of base = 0.200 mol/L Kb of base = 9.75 × 10-4 To…

Q: 0.1 M NH4CI solution, using the given pH data, write expression for equilibrium constant (Ka or Kb):

A: Net ionic reaction for the hydrolysis reaction in NH4Cl is given below NH4+(aq) +…

Q: Determine the pH of each of the following solutions. (a) 0.684 M hypochlorous acid (weak acid…

Q: What is the pH of a 0.0760 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: Given salt is a mixture of W.B + SA HONH3Cl it undergo salt hydrolysis It's pH = 7 - 1/2(pkb +…

Q: The compound ethylamine is a weak base like ammonia. A solution contains 0.111 M C,H5NH3* and 0.406…

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: Place the following acids in order of increasing strength: -H3PO4, H3PO2 and H3PO3.…

A: We have to explain the acidity order: -H3PO4, H3PO2 and H3PO3.

Q: If the molar concentration of OH- is 1.0 x 10-7, the pH is what?

A: Applying formula of pH POH= -log[OH-]

Q: Suppose 1.00 mol of HCOOH and 0.500 mol of NaHCOO are added to water and diluted to 1.00 L.…

A: Given moles of HCOOH = 1.00 mol moles of NaHCOO = 0.500 mol Ka = 1.77…

Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?

A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…

Q: The pH of an aqueous solution of 0.508 M phenol (a weak acid) , C6H5OH, is _______.

A: Since pKa for phenol is 9.98 and concentration of phenol is 0.508 M (given)

Q: A study of the acid shows that the pH of an acid HA O.12 MIK2.62. What is the K, of this acid?

A: Acid Dissocaition constant, Ka has to be determined for the Acid HA of 0.12 M with pH 2.26.

Q: In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of…

A: The dissociation of formic acid. Given data: Initial concentration of formic acid is 0.558M. pH of…

Q: Provided that a chemist prepared a 1.00 M acetic acid solution (HC2H3O2) wherein he found out that…

A: The weak acids are those that partially dissociate in aqueous solution to give protons. The pH is…

Q: Determine the pH of a 0.13 M acetic acid solution. The K, of acetic acid is 1.8 X 10 5.

Q: The Kb of pyridine, C5H5N, is 1.7 x 10−9. Calculate the pH of a 0.124 M solution of pyridinium…

A: Given: The Kb of pyridine (C5H5N) = 1.7 x 10−9 The molarity of the solution of pyridinium bromide…

Q: Calculate the pH of a 0.300 M solution of the dibasic compound piperazine, which we will designate…

A: pH is used to determine the concentration of hydronium ion.

Q: 3b.) The Ka of acetic acid is 1.8 x 105. Calculate the pH of the following solutions: b. A solution…

Q: The pH of an aqueous solution of 0.223 M ammonium bromide, NH,Br (aq), is This solution is

A: In this question, we want to determine first the pH of the aqueous solution of NH4Br(aq) and then…

Q: Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D) 0.100…

Q: The pH and Kh of O.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 will be respectively equal…

A: Value of pH is used to measure extent of acidity or basicity of a solution. At room temperature,…

Q: 6. Calculate the pH of the following solutions: a. 2.0 M morphine hydrochloride, C,H„NO, HCI (pK, =…

A: The given are salts, thus the pH will be calculated considering the salt hydrolysis.

Q: Explain how a set of weak bases, all with approximately the same 0.1 molarity, can have different pH…

A: Answer

Q: Construct the expression for Ka for the weak acid, CH,COOH. CH,COOH(aq) + H,O(1) = H,0*(aq) +…

A: Expression of Ka The equilibrium constant expression is the ratio of the concentrations of a…

Q: In the laboratory, a general chemistry student measured the pH of a 0.591 M aqueous solution of…

Q: The [H3O+] of Coca-Cola Classic ® is 3.2 x 10-3. What is its pH? Is it acidic or basic?

A: The pH of the given solution can be defined as the measure of its basicity or the acidity. It is…

Q: Determine the pH of the solution

A: According to question Ka = 1.82 x 10-⁵ Mass of acetic acid = 20.0 g Molar mass = 60.05g/mol No. Of…

Q: Determine the pH of a 0.085 M solution of boric acid. Ka of boric acid = 5.4 x 10 10

A: Ka= acid strength measured relative to water For Acid dissociation constant, the strength of acid is…

Q: If the KbKb of a weak base is 1.6×10−6,1.6×10−6, what is the pH of a 0.18 M0.18 M solution of this…

A: Concentration of the solution is 0.18 M. Kb = 1.6 x 10-6 The Ka value is calculated by following…

Q: The pH of an aqueous solution of 0.176 M ammonium bromide, NH Br (aq), is This solution is

A: 1. Solution - According to the question - pH = pH stand for potential of hydrogen, since pH is…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Determine the pH of each of the following
solutions.
(a) 0.549 M hydrogen peroxide (weak acid with
Ка 3 2.4e-12).
(b) 0.615 M acetic acid (weak acid with Ka
1.8e-05).
(c) 0.866 M pyridine (weak base with Kp = 1.7e-
09).

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 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

Determine the pH of each of the following solutions.(a) 0.246 M hydrocyanic acid (HCN) (weak acid with Ka = 4.9e-10).(b) 0.228 M propionic acid (weak acid with Ka = 1.3e-05).(c) 0.850 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions. (a) 0.296 M arsenous acid (weak acid with Ka = 5.1e-10). (b) 0.315 M boric acid (weak acid with Ka = 5.8e-10). (c) 0.571 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions.(a) 0.112 M acetic acid (weak acid with Ka = 1.8e-05).(b) 0.855 M hydrazoic acid (weak acid with Ka = 1.9e-05).(c) 0.867 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of (a) A 0.10 M CH3COOH solution (ICE) (b) A solution that is 0.10 M CH3COOH and 0.10 M CH3COONa. Ka for CH3COOH = 1.8 X 10-5.
Determine the pH of each of the following solutions. (a) 0.826 M hydrocyanic acid (HCN) (weak acid with K₂ = 4.9e-10). 5.81 (b) 0.656 M hypobromous acid (weak acid with K₂ = 2.5e-09). (c) 0.673 M pyridine (weak base with Kb = 1.7e-09).
(7) Calculate the pH of each of the following solutions: (a) 0.1000M Propanoic acid( HC H O,,K=1.3x105) (b) 0.1000M sodium propanoate (Na C HỎ) (c) 0.1000M HC₂H₂O, and 0.1000M Nа С¸¸0₂ 3 5 52 (d) After 0.020 mol of HCl is added to 1.00 L solution of (a) and (b) above. (e) After 0.020 mol of NaOH is added to 1.00 L solution of (a) and (b) above.
You prepared 500 mL buffer solution that contains 0.50 moles monoprotic weak acid (HA) and 0.30 moles conjugate base (NaA). The solution has a pH of 4.20. (a) What is the Kp of the conjugate base, NaA? (b) What is the pH of the buffer solution after adding 400 mL of 0.30 M H,SO4? pH = pKa – log(THA), [A*]
A buffer is made with sodium acetate (CH3COONa) andacetic acid (CH3COOH); the Ka for acetic acid is 1.80 x 10-5.The pH of the buffer is 3.98. What is the ratio of the equilibriumconcentration of sodium acetate to that of acetic acid?(a) -0.760 (b) 0.174 (c) 0.840 (d) 5.75 (e) Not enough informationis given to answer this question.
COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…
650.0 mL of HBr gas at 21.0 °C and 1025 mm Hg is absorbed completely into a solution that was created by mixing 7.147 g of Na2CO3 and 250.0 g of water. (a) What is the pH of the solution? (b) What is the freezing point of the solution?
The thermodynamic solubility product of AGCN is 6.0x10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.7e-9 X mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.8e-15 X mol·L-1
(ii) Calculate the pH of a 0.250 M solution of a weak acid with Ka = 2.5 x 107 [HA] [H'] (A'] initial change equilibrium