24.) After an acid has given up its proton, it is capable of getting back that proton and acting as a base. A conjugate base is what is left after an acid gives up a proton. The stronger the acid, the weaker the conjugate base. The weaker the acid, the stronger the conjugate base. Complete the table below. Acid H₂SO4 H3PO4 H₂PO4 H₂O HPO4² NH4* Base HSO4 F NO3 SO4² H₂O Equation H₂SO4 →→H + HSO4

24.) After an acid has given up its proton, it is capable of getting back that proton and acting as a base. A conjugate base is what is left after an acid gives up a proton. The stronger the acid, the weaker the conjugate base. The weaker the acid, the stronger the conjugate base. Complete the table below. Acid H₂SO4 H3PO4 H₂PO4 H₂O HPO4² NH4* Base HSO4 F NO3 SO4² H₂O Equation H₂SO4 →→H + HSO4

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 pH of a solution in which [OH−]=7.1×10−3M.

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

Q: In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, or weak…

A: In an aqueous solution, strong acids and strong bases tend dissociate completely by forming H+ ions…

Q: Consider some common drinks. Organize this list of foods with pH from most basic to most acidic.…

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: What is the pH of a 7.5 × 10⁻⁶ M KOH solution?

A: pH is used in various fields to specify the acidity and basic of the solution. pH value ranges from…

Q: The relative acidity of an aqueous solution is measured by the H+ ion concentration. pH = – log(H+)…

A: We know that PH=−log(H3O+)[H3O+]=10−PH[H3O+]=10−3.5=0.00031622776601=3.162×10−4 M hence 1st…

Q: Write the products of the following acid-base reaction. H₂C- OH OH You should include all products.…

A: Bronsted–Lowry acids and bases: According to this theory, an acid is a proton (H⁺) donor, and a base…

Q: An acid does not donate a proton. True O False

A: An acid is a substance that donates proton. The above statement is true or false.

Q: An aqueous solution has a hydrogen ion concentration of 1.0 x 10-8 M. What is the hydroxide ion…

A: If pH of solution is greater than seven than solution will be basic in nature

Q: A) Identify each of the following as an acid or a base. LiOH, HClO4, HI, Ca(OH)2 B) Write a…

A: This question demands the basic concept about acid-base theory. We know that, according to Arrhenius…

Q: From the list of the given compounds, choose the strong acid in an aqueous solution. H, SO, CH;CO,H…

A: To solve this problem we have to know about the strong and weak acids .

Q: Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH…

A: pH of the solution is equal to the negative logarithm of the concentration of hydronium ions H3O+.…

Q: O ACIDS AND BASES Daria Calculating percent dissociation of a weak acid Calculate the percent…

A: The term percent ionization can be defined the fraction of the weak acid or base which ionizes in…

Q: How would you categorize a solution that has a concentration of hyc O acid O a salt O basic O…

A: A solution isAcidic if pH<7Basic if pH>7Neutral if pH=7& pH + pOH = 14pH = -log[H+]pOH =…

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H3O+],[H3⁢O+], of 4.18×10−6…

A: The pH of the solution is = 5.38

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

Q: H₂SO4

A: Acids are the substances which releases proton i.e. H+ in the solution. Acids often are electron…

Q: Strong and weak acids differ greatly in their empirical and theoretical definitions. Identify…

Q: Suppose we have a 1.0M solution of acetic acid, CH,COOH, and a solution of 0.1M hydrochloric acid,…

A: Acidity is defined as the ability of a molecule to release protons. If a compound easily donates…

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

A: The question is based on the concept of salt hydrolysis. We need to arrange given salts in…

Q: What is the pH of a bleach solution that has a [OH−]=5.6×10−6 M?[OH−]=5.6×10−6 M? pH=pH= Is…

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the pOH of the solution. Is the…

Q: All of the following are weak acids except O HNO2 O HCN HBr НCNO HF

A: • we need to predict the strong acid from the given acids - HNO2 (Nitrous acid), HCN (Hydrocyanic…

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

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: The pH of an aqueous solution at 25°C was found to be 6.60. The pOH of this solution is The…

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

A: There are several theories to explain the compound as an acid or a base.Arrhenius theory is one such…

Q: What concentration of sodium hydroxide is needed to give an aqueous solution with a pH of 10.210?…

A: NaOH → Sodium Hydroxide NaOH → It is strong BaseSo it will completely dissociate NaOH ⇌ Na++…

Q: Label the acid, base, conjugate aci choices. HCI + NH3 --> CI" + NH4*

A: An acid can be defined as substance which is capable of donating a proton. A base is a molecule…

Q: An aqueous solution has a hydrogen ion concentration of 1.0 × 10¬4 M. What is the hydroxide ion…

A: if the concentration of hydrogen ion is greater than 10^(-7) the solution is acidic

Q: * pH of a Strong Acid, a Weak Acid The pH of a solution is the negative logarithm of the molar…

A: Ph of given solution= 1.

Q: Determine the [OH−] , pH, and pOH of a solution with a [H+] of 6.0×10−5 M at 25 °C. Determine the…

A: pH, pOH are related through the below formulas: pH + pOH = 14 (or) pH = 14 - pOH (or) pOH = 14 - pH…

Q: Determine the [OH−] , pH, and pOH of a solution with a [H+] of 1.5×10−8 M at 25 °C. Determine the…

A: To solve these problems, we can use the equations relating pH, pOH, [H+], and [OH-] in water For a…

Q: Enter your answer in the provided box. A solution of formic acid (HCOOH) has a pH of 2.88. How many…

A: Given information,Concentration of the phosphoric acid solution =0.25 M

Q: The concentration [H*] of a substance is 3.7×10 10. Calculate the pH value of the substance and…

Q: Nitric Acid is used in cleaning glassware during very precise analytical chemistry. You obtain a…

A: Given, Concentration of HNO3 = 0.15 M PH =?

Q: the pH of a mysterious solution has an H+ concentration of: 1.704 x 10-2 is. After finding the pH,…

Q: Calculate the value of [OH] from the given [H3O+] in Note: The ion product of water = 1.0 × 10¯¯ 14…

A: Part 1) .Given , [H3O+] = 10-6 M [OH-] = ? We know that, [H3O+] [OH-] = kw = 1.0×10-14 So, [OH-] =…

Q: Calculate the [H+] in each of the following solutions, and indicate whether the solution is acidic…

Q: What is the pH of a bleach solution that has a [OH−]=7.1×10−4 M?[OH−]=7.1×10−4 M? pH=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

24.) After an acid has given up its proton, it is capable of getting back that proton and acting as a base. A
conjugate base is what is left after an acid gives up a proton. The stronger the acid, the weaker the
conjugate base. The weaker the acid, the stronger the conjugate base. Complete the table below.
Acid
H₂SO4
H3PO4
H₂PO4
H₂O
HPO4
NH4*
Base
HSO4
F
NO3
SO
H₂O
Equation
H₂SO4 → H*+ HSO4

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

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

Strong acids and strong bases ionize 100% in aqueous solution.- HCl is a strong acid. In solution we write it as H+(aq) + Cl -(aq).- HF is a weak acid. In solution we write it as HF(aq).- KOH is a strong base. In solution we write it as K+(aq) + OH -(aq).- NH3 is a weak base. In solution we write it as NH3(aq).Exception: Since Ca(OH)2 is only slightly soluble we write it as Ca(OH)2(s).Below is a list of the 6 strong acids and 6 strong bases you should know. All other acids and bases are considered weak. Strong Acids Strong Bases HCl, HBr, HI LiOH, NaOH, KOH HNO3 Ca(OH)2 (slightly soluble) HClO4 Ba(OH)2 H2SO4 Sr(OH)2 What is the pOH of an aqueous solution of 1.78E-2 M perchloric acid?pOH =
Please don't provide handwriting solution
Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– + H3O+ Can you identify the acid, base, conjugate acid, and conjugate base in this reaction? Use patterns in the periodic table to explain why the substances you identified acted as the acid and the base in this reaction.
pH РОН [H*] [OH"] 11.34 M M 13.41 M -- - 3.30 x 10-10 _M 3.60 х 10-5 м Complete the following table by calculating the missing entries. In each case indicate whether the solution is acidic or basic. Σ
Is HNO3 an acid, base, or neither?
match the terms to the correct definition. (A choice that describes a property of an acid, but is NOT the definition as requested, will be counted as wrong). Brønsted acid Brønsted base Arrhenius acid Arrhenius base A. Substance that donates a proton B. Substance that accepts a proton C. Substance that causes an increase of [H+] in solution D. Substance that causes an increase of [OH–] in solution E. Substance that causes a decrease in [H+] in solution F. Substance that causes a decrease in [OH–] in solution
Give detailed Solution with explanation needed (don't give Handwritten answer
An aqueous solution at 25 °C has a pH of 5.8. Calculate the pOH. Be sure your answer has the correct number of significant digits. 0 Ś ? X
A solution with [H+]= 1 x 10-3 M has pH . Is this solution an acid, base, or neutral? A solution with [H+] = 1 x 10-7 M has pH . Is this solution an acid, base, or neutral?
16. For the following reactions, label each species as an acid or a base. Indicate the species that are conjugates of one another. HSO4_+ H2O +→ SO2²- + H3O+ HS- + CN- E→ S²- + HCN
Calculate the pH of a 9.8 x 10^-4M aqueous solution of hydrobromic acid . Round your answer to 2 decimal places.
Finding pH An unknown substance has a hydrogen ion concentration of 3H 4  3.1  108M. Find the pH and classify the substance as acidic or basic