Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species CH3CH(OH)COOH CH,COO CH,CH(OH)COO H₂O relative pH of 0.1 M aqueous solution 4 3 2 7 ✗ G H₂O + CH3COOH HIO 5 10 6 1 (lowest) 4

Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species CH3CH(OH)COOH CH,COO CH,CH(OH)COO H₂O relative pH of 0.1 M aqueous solution 4 3 2 7 ✗ G H₂O + CH3COOH HIO 5 10 6 1 (lowest) 4

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.40EP: Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the...

See similar textbooks

Related questions

Q: Fill in the left side of this equilibrium constant equation for the reaction of 4-bromoaniline…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: find PH for part C and D Part C 0.085M in HF(K = 6.8 × 104) and 0.225M in HC H₂O (K = 1.3 × 1010)…

A: The objective of the question is to calculate the .

Q: If we used H2C4H4O5 as the weak diprotic acid, which of the four species, H2C4H4O5, HC4H4O5^-,…

A: Given that, H2C4H4O5 is a weak diprotic acid & the four species are H2C4H4O5, HC4H4O5-,…

Q: You can obtain the pH of a 0.100 M HCl solution by assuming that all of the H3O+ ion comes from the…

A: HCl dissociates completely to its constituent ions as: Auto-ionization of Water: Self ionization of…

Q: A stock solution is made by dissolving X grams of KOH in water and making it up to the mark in a…

A: The solution which resists change in pH of the solution is called a buffer solution. The resistance…

Q: Consider the following ions: Cl-, HS-, NO2-, F-, and HS04-. (a) Which of these ions in water gives…

A: Given ions Cl- HS- NO2- F- HSO4-

Q: 1) A conjugate acid is defined as 2) In the general ionization reaction: HX(aq) + H,0(1) H,0* +…

Q: Give the conditions for a neutral aqueous solution at 25 Celcius, in terms of [H+], pH, and the…

A: For a neutral solution at 25oC,The ionic product, Kw is 10-14

Q: Calculate the pH at 25 °C of a 0.12M solution of pyridinium chloride (C,H, NHCL). Note that pyridine…

A: We can calculate the POH of weak base using the relation. POH = 1/2( PKb -logC) From POH we can…

Q: Consider the following data on some weak acids and weak bases: name acid solution 0.1 M KCN 0.1 M…

A: pH of a solution is defined as the negative logarithm of Hydrogen ion concentration. pH = -log(H+)

Q: CLEARLY identify the acid, base, conjugate acid and conjugate base

A: In an acid-base reaction an acid (A) when loses proton and base (B) accepts that proton. Now the…

Q: Part D In the simulation, open the Custom mode. The beaker will be filled to the 0.50 L mark with a…

A: The alkalinity or acidity of a solution is determined by the pH scale. It has a range from 0 to 14,…

Q: An acid has the generic formula H2X, where X is an anion. What is the charge on X? What is the…

A: The acid given is H2X. Since the charge on H will be +1 because it has only 1 valence electrons.…

Q: Monoprotic acids are capable of donating one proton, however SO,2- PO, and CO3? are known as…

A: The species given are SO42-, PO43- and CO32-.

Q: 1--The solution of substance (X) is completely ionized in water, its pH value is (10), so its…

A: Dear student , since you have posted multiple questions we are allowed to solve only first question…

Q: When red wine is fermented with bacteria, the result is red wine vinegar! Fermentation converts the…

A: pH is equal to the negative logarithm of hydronium ion. pH=-log(H3O+) Henderson Hasselbalch…

Q: o simplify the measurement of the acidity or basicity of a solution, the pH (hydrogen potential)…

A: Given[H+] = 0.0000375 pH = To be determined

Q: Rainwater is found to be slightly acidic compared to pure water. It has a hydrogen concentration of…

A: Given: H+ of rainwater = 10-5.6

Q: The pH of saliva is normally in the range of 6.4 to 7.0. However, when a person is ill, the person's…

A: pH is defined as negative logarithm of hydrogen ion concentration pH= -log[H+] If pH<7 then the…

Q: A chemist dissolves 428. mg of pure sodium hydroxide in enough water to make up 100. mL of solution.…

Q: A chemist dissolves 305.mg of pure barium hydroxide in enough water to make up 140.mL of solution.…

A: The amount of Ba(OH)2 taken to prepare the solution is 305 mg = 0.305 g. The volume of the solution…

Q: A chemist dissolves 818. mg of pure potassium hydroxide in enough water to make up 150. mL of…

Q: A chemist dissolves 172. mg of pure barium hydroxide in enough water to make up 120. mL of solution.…

A: Molarity(M) of a solution is defined as the number of moles of solute present in the 1 liter of the…

Q: Find the concentration of hydroxide, OH-, ions in a 0.100 M solution of HOAc, acetic acid

Q: Human blood is slightly basic. Calculate the hydroxide ion concentration in a sample of blood with…

A: Given, (a). pOH = 6.49, then find hydroxide ion concentration that is [OH-] = ? (b). pH value of…

Q: Consider the following data on some weak acids and weak bases: name hydrofluoric acid acid acetic…

Q: On a shelf in the lab storeroom marked “Solutions of Acids”, a bottle has a torn label. All that can…

A: Acid dissociates in water to form hydrogen ion and it's conjugate base.

Q: A chemist dissolves 505. mg of pure barium hydroxide in enough water to make up 180. mL of solution.…

Q: A chemist dissolves 208. mg of pure barium hydroxide in enough water to make up 50. mL of solution.…

A: The mass of barium hydroxide = 208 mg = 0.208 gVolume of the solution = 50 mLThe pH of the solution…

Q: The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per…

A: pH of solution is defined as negative logarithm of hydrogen ions present in solution.

Q: NaCN HC Ba(OH), HONH Na SO HOI

A: The question is based on the concept of acid and bases. we have to determine which compound is…

Q: A chemist dissolves 87. mg of pure barium hydroxide in enough water to make up 90. mL of solution.…

Q: The pH of a nitric acid (HNO:) solution is 3.85 Determine the [H*] in the HNO3 solution. Calculate…

Q: pH is a logarithmic scale used to indicate the hydrogen lon concentration, [H], of a solution: pH =…

A: Given : For part A : Mass of HCl = 0.55 g Volume of solution = 5.5 L For part B : Mass of NaOH…

Q: The pH of a 0.67 M solution of butanoic acid (HC4H₂O₂) is measured to be 2.50. Calculate the acid…

Q: The dissociation of pure water into H3O+ and OH‐ ions depends on temperature. Calculate the pH at…

A: The dissociation of pure water, 2H2O(l)---> H3O+(aq)+ OH-(aq) Given that concentration of ions…

Q: In industrial environments, benzoic acid, C6H5COOH, is widely used to produce a range of products…

A: Given ,

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

Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure
water to the pH of the other solutions.
Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases.
species
CH3CH (OH) COOH
CH3COO
CH2CH(OH) COO
H20
H₂O+
CH3COOH
relative pH of
0.1 M aqueous solution
4
3
5
2
7
1 (lowest)
☑
HIO
IO
6
4

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: Concept required to solve the problem!

VIEW

Step 2: Finding out the relative order of acidic and basic strength!

VIEW

Step 3: Finding out the relative order of pH!

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 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

For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. CaO b. SO2 c. Cl2O
Aqueous Solutions of Acids, Bases, and Salts a For each of the following salts, write the reaction that occurs when it dissociates in water: NaCl(s), NaCN(s), KClO2(s), NH4NO3(s), KBr(aq), and NaF(s). b Consider each of the reactions that you wrote above, and identify the aqueous ions that could be proton donors (acids) or proton acceptors (bases). Briefly explain how you decided which ions to choose. c For each of the acids and bases that you identified in pan b, write the chemical reaction it can undergo in aqueous solution (its reaction with water). d Are there any reactions that you have written above that you anticipate will occur to such an extent that the pH of the solution will be affected? As pan of your answer, be sure to explain how you decided. e Assume that in each case above, 0.01 mol of the salt was dissolved in enough water at 25C to make 1.0 L of solution. In each case what additional information would you need in order to calculate the pH? If there are cases where no additional information is required, be sure to state that as well. f Say you take 0.01 mol of NH4CN and dissolve it in enough water at 25C to make 1.0 L of solution. Using chemical reactions and words, explain how you would go about determining what effect this salt will have on the pH of the solution. Be sure to list any additional information you would need to arrive at an answer.
Pure liquid ammonia ionizes in a manner similar to that of water. (a) Write the equilibrium for the autoionization of liquid ammonia. (b) Identify the conjugate acid form and the base form of the solvent. (c) Is NaNH2 an acid or a base in this solvent? (d) Is ammonium bromide an acid or a base in this solvent?
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
You are asked to determine whether an unknown white solid is acidic or basic. You also need to say whether the acid or base is weak or strong. You are given the molar mass of the solid and told that it is soluble in water. Describe an experiment that you can perform to obtain the desired characteristics of the white solid.
A base is a substance that dissociates in water into one or more ______ ions and one or more ________. a.hydrogen . . . anions b.hydrogen . . . cations c.hydroxide . . . anions d.hydroxide . . . cations
Find [OH+], [OH-] and the pH of the following solutions. (a) 30.0 mL of a 0.216 M solution of HCI diluted with enough water to make 125 mL of solution. (b) A solution made by dissolving 275 mL of HBr gas at 25C and 1.00 atm in enough water to make 475 mL of solution. Assume that all the HBr dissolves in water.
Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic. The relevant Ka and Kb values are found in Tables 13-2 and 13-3. a. NaNO3 b. NaNO2 c. C5H5NHClO4 d. NH4NO2 e. KOCl f. NH4OCl
Consider the following four solutions: (1) apple juice, pH 3.8, (2) pickle juice, pH 3.5, (3) carbonated beverage, pH 3.0, and (4) drinking water, pH 7.2. a. Which solution has the highest [H3O+]? b. Which solution has the highest [OH]? c. List the solutions in order of increasing acidity. d. List the solutions in order of decreasing basicity.
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. HC3H3O3 b. HCN c. H2SO4 d. H2SO3