### Weak Acids and Weak Bases Data OverviewConsider the following data on some weak acids and weak bases:#### Weak Acids:| **Name** | **Formula** | **Ka** ||-------------------|--------------|-----------------|| Acetic Acid | HCH₃CO₂ | 1.8 × 10⁻⁵ || Hydrocyanic Acid | HCN | 4.9 × 10⁻¹⁰ |#### Weak Bases:| **Name** | **Formula** | **Kb** ||------------|------------------|-----------------|| Aniline | C₆H₅NH₂ | 4.3 × 10⁻¹⁰ || Ammonia | NH₃ | 1.8 × 10⁻⁵ |### pH Ranking Task:Using this data, rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on.| **Solution** | **pH** ||--------------------------|-----------------------------|| 0.1 M NH₄Cl | [ Dropdown: 1 (lowest), 2, 3, 4 (highest) ] || 0.1 M NaCN | [ Dropdown: 1 (lowest), 2, 3, 4 (highest) ] || 0.1 M KCl | [ Dropdown: 1 (lowest), 2, 3, 4 (highest) ] || 0.1 M C₆H₅NH₃Br | [ Dropdown: 1 (lowest), 2, 3, 4 (highest) ] |### Explanation of Data Tables:- **Ka (Acidity constant)**: A measure of the strength of a weak acid in solution. The smaller the Ka value, the weaker the acid.- **Kb (Basicity constant)**: A measure of the strength of a weak base in solution. The smaller the Kb value, the weaker the base.### Solution Ranking Logic:- Solutions with species that do not hydrolyze (e.g., KCl) typically have neutral pH

Answered: Image /qna-images/answer/010c91bc-9a74-468a-ac97-02218f9eaa7d.jpg

Answered: solution 0.1 M NHACI 0.1 M NaCN 0.1 M…

Science

Chemistry

solution 0.1 M NHACI 0.1 M NaCN 0.1 M KCI 0.1 M C6H5NH3Br PH choose one 1 (lowest) 2 4 (highest) choose one 234

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: You use a pH meter to measure the pH of a solution that has a pH of 5.0. Determine the concentration…

A: The measure of the acidic and basic strength of any solution is given by its pH value. A strong acid…

Q: Calculate the pH of a 0.5000M NaCN solution. K. of HCN=4.9x10-10

Q: 5. Rank the following solutions from highest pH to the lowest pH: 0.10 M HF, 0.10 M KCI, 0.10 M KOH,…

A: The question asked to rank the given solutions from highest to lowest pH, which required an…

Q: What is the pH of a 0.075 M LiF solution? (Round answer to nearest decimal place. Example, 75.877…

Q: Find the percent ionization of a 0.337 M HX solution. The Ka for HX is 3.5 x 104. Select one: O 3.2…

Q: Which of the following solutions of monoprotic acids has the HIGHEST concentration of its conjugate?…

A: Acid and conjugate base For an acid HA, HA(aq)+H2O(l)→A-(aq)+H3O+(aq) The equilibrium constant is :…

Q: Hydrogen fluoride (HF) behaves as a weak acid in aqueous solution. Two equilibria influence which…

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

Q: What is the pH of a 0.570 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?

A: NaCN dissociates in an aqueous medium as follows: NaCN→Na++CN- Na+ ions don't contribute to the pH…

Q: At 40oC a solution has a Kw of 1.6 x10 - 14. What is the pOH of this neutral solution? Group of…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: A 2.0 M solution of a weak acid is found to have a pH of 5.5. What is the K₂ value of the weak acid?…

Q: Which of the following solutions would be expected to have a pH less than 7.00? A) C.H:COOK B) HONH…

A: hydrolysis salt of strong acid and weak base. HBr +HONH2→ HONH3Br HONH3Br + H2O → HONH2 + H3+O +…

Q: Assume the following substances form solutions at the same concentration, whicch one would provide…

A: According to Arrhenius concept, an acid is a substance i.e. when dissolved in water gives H+ ions.…

Q: Each of the systems below has a total volume of 100 mL. Which of the systems would be able to…

A: A buffer is a solution that cannot change the even after the addition of an acid or a base.To find…

Q: What is the pH of a solution of 100 mL of 0.025 M HBr and 100 mL of 0.10 M NaF? (HF Ka= 7.2 x 10-4)

A: Given Volume of HBr solution = 100 mLConcentration of HBr solution = 0.025 MVolume of NaF solution =…

Q: 5. If the pH of the methyl red solution is changed to 4, answer with T (increase), v (decrease), +…

A: Given information:

Q: Find the pH and percent ionization of each HF solution (Ka = 6.8 ́ 10-4). In which cases can you not…

Q: At 50°C the value of K w is 5.5 x 1014. A basic solution at 50°C has

Q: For the diprotic weak acid H₂A, K₁1 = 3.5 x 10-6 and K₁2 = 8.3 × 10-⁹. What is the pH of a 0.0500 M…

Q: What is the factor difference between a solution with a pH of 9 and 9.3?

A: Given: Initial pH = 9 Final pH = 9.3

Q: 0.25 — X X X x = 5.8 х 10-2 pH = [ ? ]

Q: Each of the systems below has a total volume of 100 mL. Which of the systems would be able to…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: The nydrogen lon ncentrations in cheeses range from 2.51 to 6.31 X ne corresponding rang 6.8 s pH <…

A: Given , [H+] = 2.51 x 10-5 M PH is defined as negative logarithm of concentration of Hydronium ion.

Q: What is the concentration of the hydroxide ion?

A: Given :- concentration of hydronium ion = 0.0017 M To calculate :- concentration of hydroxide ion…

Q: A mixture formed by adding 43.0 mL of 2.5x10-2 M HCl to 140 mL of 1.5x10-2 M HI Express the pH of…

Q: Which salt produces a basic aqueous solution at 25°C? Group of answer choices KBr NH4Br NaF LiI…

A: We will se acid and base part of salt to predict nature of salt.

Q: Predict whether the following aqueous solutions have a pH less than 7, very close to or equal to 7…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: What is the pH of a 0.580 M solution of NaCN (Ka of HCN is 4.9 x 1010)?

Q: The pOH of a solution is 9.38. What is the H* concentration in the solution?

Q: What is the concentration of Cl in the solution 0.25 M AlCl3

A: AlCl3 (aq) ------> Al3+ (aq) + 3Cl3- (aq)

Q: Select the total concentration of all ions in a 0.2 M (NH4)3PO4 solution O 0.9 M 0.8 M O 0.7 O 0.6 M

A: The question is based on the concept of molarity. molarity is a method of expressing concentration…

Q: Patient 1 comes into the ER is found to have a blood pH of 7.2. Is the patient suffering acidosis…

A: The patient is suffered from the acidosis if the body having excess amount of the acid fluid in the…

Q: In a 0.14.M aqueous solution of propionic acid (C,H,CO₂H), what is the percentage of propionic acid…

A: Given,Molarity of propionic acid ( C2H5CO2H ) = 0.14 MFrom the ALEKS data table:pKa of propionic…

Q: The pH after adding 23.0 mL of 1.0 M NaOH to 25.0 mL of 1.0 M HCl is 0.080 1.1 1.4 0.042

A: According to guidelines i can answer only first question, please repost the other question

Q: A solution of 0.1 M HCl has 0.1 M [H30+]. True…

A: Explanation:HCl is a strong acid, so it will dissociate completely in solution.

Q: he [H3O¯] and [OH]]ion conc

Q: %3D What is the pH of a 0.1000 M NACH3COO solution? (Ka CH3COOH = 1.8x10^-5) 4.75 5.13 8.87 7.45…

A: We have find out pH of 0.1000 MNaCH3COO Solution.

Q: An unknown weak acid with a concentration of 0.066 M has a pH of 1.80. What is the Ka of the weak…

Q: What is the pOH of a solution that has a hydroxide ion concentration[OHˉ] of 2.00 x10ˉ 6 M?

A: A solution is made up of solute and solvent. Solvent is present in large amount and solute is…

Q: Part D A mixture formed by adding 60.0 mL of 2.5x10-2 M HCl to 120 mL of 1.0x10-2 M HI. Express the…

Q: An aqueous solution of HNO3 has pH 4. What is the pOH of the solution? Answer…

A: The relation between pH and pOH is given by, pH + pOH =14 pH of the solution is given by,…

Q: Acid Base Neutralization a) What is the pH of a solution of 20 mL of 0.2 M HBr pH =…

Q: In the following identify if the solution would be acidic, basic or neutral: 25 mL of a 0.200 M…

Q: What is the OH concentration of a solution with a H3O+ concentartion of 8.47 x 10-8

Q: Benzoic acid, C6H5COOH, has a Ka = 6.3 x 10-5, What is the percent ionized in a 0.95 M solution of…

A: Final answer is given in explanation please see from there.Explanation:Approach to solving the…

Q: The acid dissociation constants for phosphoric acid (H₂PO4) are Kai = 0.00711, Ka2 = 6.32 x 10-8,…

A: Given data : Ka1 = 0.00711 Ka2 = 6.32×10-8 Ka3 = 7.1×1-13

Question

### Weak Acids and Weak Bases Data Overview

Consider the following data on some weak acids and weak bases:

#### Weak Acids:
| **Name** | **Formula** | **Ka** |
|-------------------|--------------|-----------------|
| Acetic Acid | HCH₃CO₂ | 1.8 × 10⁻⁵ |
| Hydrocyanic Acid | HCN | 4.9 × 10⁻¹⁰ |

#### Weak Bases:
| **Name** | **Formula** | **Kb** |
|------------|------------------|-----------------|
| Aniline | C₆H₅NH₂ | 4.3 × 10⁻¹⁰ |
| Ammonia | NH₃ | 1.8 × 10⁻⁵ |

### pH Ranking Task:

Using this data, rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on.

| **Solution** | **pH** |
|--------------------------|-----------------------------|
| 0.1 M NH₄Cl | [ Dropdown: 1 (lowest), 2, 3, 4 (highest) ] |
| 0.1 M NaCN | [ Dropdown: 1 (lowest), 2, 3, 4 (highest) ] |
| 0.1 M KCl | [ Dropdown: 1 (lowest), 2, 3, 4 (highest) ] |
| 0.1 M C₆H₅NH₃Br | [ Dropdown: 1 (lowest), 2, 3, 4 (highest) ] |

### Explanation of Data Tables:
- **Ka (Acidity constant)**: A measure of the strength of a weak acid in solution. The smaller the Ka value, the weaker the acid.
- **Kb (Basicity constant)**: A measure of the strength of a weak base in solution. The smaller the Kb value, the weaker the base.

### Solution Ranking Logic:
- Solutions with species that do not hydrolyze (e.g., KCl) typically have neutral pH

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

The OH– concentration in a 1.0 × 10–3 M Ba(OH)2 solution is Group of answer choices 0.50 × 10–3 M. 1.0 × 10–3 M. 2.0 × 10–3 M. 1.0 × 10–2 M. 0.020 M.
What is the pH of a 0.25 M NH3 solution? Kb = 1.8 x 10-5 pH = [?] pH Enter
Normal text Arial 11 BIU A 1 2 I 3 4 I 5 | 6 7 Color after addition of red Is the solution acidic, basic or neutral? Substance pH using cabbage juice indicator pH using pH meter cabbage juice indicator Lemon Juice Pinkish violet 2-4 2.23 Apple Juice Light violet 4-6 4.62 Very light violet 6-7 purple Milk 6.75 Baking Soda Bluish-violet 6-9 9.43 Aspirin Light pink 2-4 3.28 Antacid Light violet 4-6 6.82 Shampoo Purple violet 2-6 5.93 Conditioner Pale purple 4-6 7.37 Mouthwash Pinkish violet 3-6 4.62 Soap Bluish-violet 6-9 8.24 10-11 10.21 Light greenish yellow Bleach Detergent Light green 10-12 9.41 Vinegar Pink 1-3 2.79 Windex Light green 10-12 10.75 W otv
What is the pH of a solution that is 0.80M benzoic acid and 0.20 M sodium benzoate ? Ka HC6H5O2 = 6.3x10^-5 -> 3.1 -> 3.6 -> 4.2 -> 4.8 -> 6.3
Ka for a 0.100 M methanoic acid solution whose pH is 2.37 is 4.2x10-3 8.7x10-3 1.8x10-4 1.8x10-5
4. Which of the following statements is true? A) In an acidic solution, the concentration of OH is less than H₂O In a basic solution, the concentration of OH is less than H,0 C) In a basic solution, the concentration of OH' is equal to H,O D) In an acidic solution, the concentration of H,O' is less than OH
Which of the following 0.5M aqueous salt solutions will have a pH of 7.0 at 25.0oC? LiF LiBr Sr(CIO4)2 NH4NO3
Calculate the [H+] in a solution that is 0.18 M in NaF and 0.25 M in HF. (Ka = 7.2 × 10–4)Group of answer choices 7.2 × 10–4 M 1.4 M 1.0 × 10–3 M 0.20 M 5.2 × 10–4 M
A solution has a pOH of 4.5. What is the concentration of H3O+ in the solution in Molarity? Group of answer choices 0.0000316 M 0.00000316 M 0.00316M 3.16 x 10^-10 M 3.16 x 10^-11 M 3.16 x 10^-13 M
What is the pH of a solution made by adding 0.65 mol of acetic acid (H3CO2H) and 0.30 mol of sodium acetate (H3CO2Na) to enough water to make a 1.0 L solution? (Ka = 1.8 x 10-5) Group of answer choices 8.92 5.08 4.74 4.40
Find the pH of the following: 0.2 M HCIO4 0.2 M HCIO 0.2 M NaOCI 0.5 M CH3COONa 0.5 M C6H5NH3CI 0.1 M C6H5 NH2 (utilize ICE on your solution, find ka or Kb using google)
Calculate the pH of a 0.210M NACN solution. Ką of HCN = 6.2 × 10-10 2.74 11.26 9.06 None of these 4.94 7.00