Inbox(534)ConveBalanb AnswO Post /CHEM101 CI XC The Fbartlebartlebarlelb My QUnknO SearcE I makapp.101edu.co/#Bryant's GmailCascadia Canvas Lo...T GSBA Scholarship ..HOMEGROWN TRA...Learn Touch Typing...C The Science of Well...Investor360° ® LoginClickUpReading list>>Question 22 of 40SubmitThe conjugate acid of HSO:- isA) SO;2-B) HSO.-C) HSO;?-D) H2SO310:41 PMe Type here to search59°F后W8/26/2021(8)

We have to predict conjugate acid of given species.

Answered: The conjugate acid of HSO, is A) SO;²-…

Science

Chemistry

The conjugate acid of HSO, is A) SO;²- B) HSO.- C) HSO;²- D) H2SO;

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: The molar concentration of OH- in a water solution is 1.0 x 10-9. The pH of the solution is

A: OH — = 1.0 x 10—9

Q: If the molar concentration of H3O* is 1.0 x 104, the pH is Ay and the solution is A (acidic, basic,…

A: pH can be defined as the negative logarithm of hydronium ion (H3O+) concentration. pH = -log[H3O+] •…

Q: In which one of the following reactions does an H2O molecule behave as a Lewis base? O A. Na(s) +…

A: Answer:- This question answered by using the simple concept of Lewis acid and Lewis base. The…

Q: Which of the following would be the acid equilibrium equation for HONH;CI? A) HONH,* (aq) = NH, (aq)…

Q: A solution is prepared by diluting 0.55 mol HNO3 with water to a volume of 1.75L. What is the pH of…

A: Molarity = Number of moles of solute/Volume of solution in L pH = -log[H+]

Q: The pH of a 0.0081 M solution of HNO₃ is

A: Given values-> [HNO3] = 0.0081M HNO3 ---> H^+ + NO3^- [H^+] = 0.0081M pH =-log [H^+] =…

Q: Which is the stronger acid, HF or CH3COOH?

Q: The pH of a 0.225 M weak acid solution, HA, is 4.05, what is the K, of the acid?

A: pH = 4.05 pH = -log[H+] = 4.05 [H+] = 10-4.05 = 8.91 * 10-5 M

Q: 2. Phenol, CH;OH can act as an acid in an aqueous solution. The Ka of phenolis around 2.1 x 10°, and…

A: pH = -log[H+] pOH = -log[OH] Also, pH + pOH = 14 Also Ka and Kb has a relationship Ka × Kb = Kw

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: 5. A 0.050 M solution of the salt sodium acetate (NazH3O2) will be

A: Sodium acetate (NaCH3COO) or (NaC2H3O2) is a salt of weak acid (CH3COOH) and a strong base(NaOH)

Q: 1. The pH of a 0.1 M solution of a monobasic acid P is 1.0 while the pH of a 0.2 M solution of…

A: Introduction : pH can be defined as a measure of the hydrogen ion concentration of a solution.…

Q: The pH of a 0.0030 M solution of Ca(OH), is

Q: In each of the following acid-base reactions, identify the Brønsted acid and base on the left and…

A: According to Bronsted-Lowry theory, Acid is species which donates proton and Base is species which…

Q: Suppose 0.100 mol of NaCH3COO is dissolved in enough water to make 1.00 L of solution. What is the…

A: pH is referred to the potential of hydronium ion and is calculated by taking the negative log value…

Q: HC2H3O2

A: Calculate the concentration of hydrogen ions released from the acetic acid. If the concentration of…

Q: The pH of a 0.0070 M solution of HNO₃ is

Q: The pH of a solution is 4. Which of the following is correct? (A) The solution is basic with an [OH]…

Q: hich of the following is a strong acid in aqueous solution? (a) Mg(OH)2 (b) NH3 (c) H2SO4…

A: When an acid dissociates into its ions, then the ion formed is its conjugate base and when an base…

Q: The pH of 0.65 M aqueous solution of a weak base (monoprotic) is 10.24. Determine the pKb of this…

Q: When a solution is prepared by dissolving one pellet of KOH weighing 128 mg in 500 ml of dH2O…

A: Mass of KOH = 128 mg1mg = 10-3 gMass of KOH = 0.128 gMolar Mass of KOH = 56.1 g/molMoles of KOH =…

Q: Determine the pH of each solution and classify it as acidic, basic, or neutral. (a) pOH = 8.5 (b)…

Q: 6. Identify the acid on the left and its conjugate base on the right in the following equations. d…

A: An acid is defined as a chemical substance that loses protons or hydrogen ions to the solution. A…

Q: Determine the pH of each of the following solutions. (a) 0.762 M hypobromous acid (weak acid…

A: Here, we have to calculate the pH of the given solutions: 0.762 M hypobromous acid (weak acid with…

Q: Which of the following is a conjugate pair of acids and bases involved in the below reaction?…

A: Given reaction HCN + ClO- → HClO + CN-Conjugate pair of acids and bases = To be determined Acid…

Q: 8 Write the formula of the conjugate base of a HSO, b H;PO.

A: We know that, if we have an acid HA, it undergoes dissociation as - HA → H+ + A- So, we call A to be…

Q: [References) Choose the reaction for each of the following species in which it acts as a Brønsted…

A: Bronsted base is the species which accepts H+ from the reaction. EXAMPLE – Here , HSO3- accepts the…

Q: Give the formula for the conjugate acid of each species: (a) H₂O; (b) I; (c) HCO3. (a) (b) (c)

A: Acid and Base:• Acid: acids are proton (H+) donor.• Base: bases are proton (H+) acceptor.2)…

Q: 7. What are the conjugate base and conjugate acid for HSO, ? What is the term used to describe…

A: Conjugate acid is formed when we add protons to a base and conjugate base is formed when proton is…

Q: Which of the following equations represents the acid equilibrium associated with Kaz for H3PO3? A)…

A: Given : To write the acid equilibrium associated with Ka3 for H3PO3.

Q: Let's assume that there is 400 μatm of pCO2 in our atmosphere. Assuming there is nothing else in the…

Q: In the following reaction, HCO; (aq) + H20(E)=co;²(aq) + H;0*(aq) Select one: O a. H3O* is an acid…

Q: Determine the pH of each of the following solutions. (a) 0.112 M acetic acid (weak acid with Ka…

A: pH : It is scale which measures the acidity or basicity of the solution under observation. If pH…

Q: The pH of a 0.0041 M solution of HNO₃ is

Q: (i) (ii) لال حمدم Ph OEt ?

A: An arrow always depicts from a region of high electron density to low electron density ; that is…

Q: Define Lewis acid/base versus Bronsted acid/base and describe the other two effects that influence…

Q: The pH and pOH of 0.05 M of NaOH is ..

Q: 5. Identify the conjugate base of НРО,- О но O H;PO, O H;PO, О РО 3- O OH

A: 5. Given that : We have to identify the conjugate base of HPO42- out of the following :…

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 0.0720M solution of a weak acid is 2.670. What is the Ka of the acid

Q: 11. Identify the acid and the base that are reactants in each equation; identify the conjugate base…

Q: Determine the pH of each of the following solutions. (a) 0.134 M hypochlorous acid (weak acid with…

A: The objective of the question is to calculate the pH of three different solutions, each containing a…

Q: pH of unboiled H2O: 5.90 [H+] for unboiled H2O [OH−] for unboiled H2O

A: In our daily life, importance of pH is there. The Importance of pH is everywhere in food and…

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

Inbox
(534)
Conve
Balan
b Answ
O Post /
CHEM
101 CI X
C The F
bartle
bartle
barlel
b My Q
Unkn
O Searc
E I mak
app.101edu.co/#
Bryant's Gmail
Cascadia Canvas Lo...
T GSBA Scholarship ..
HOMEGROWN TRA...
Learn Touch Typing...
C The Science of Well...
Investor360° ® Login
ClickUp
Reading list
>>
Question 22 of 40
Submit
The conjugate acid of HSO:- is
A) SO;2-
B) HSO.-
C) HSO;?-
D) H2SO3
10:41 PM
e Type here to search
59°F
后
W
8/26/2021
(8)

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 Given

VIEW

Step 2 Solution

VIEW

Step by step

Solved in 2 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

Explain and calculate the pH of a solution that is 0.0400 M in H3PO4
Which of the following is not a conjugate acid-base pair? O H2SO4, SO, O HPO4, HPo O HNO;, NO; O HBr, Br OHC H;O. CH;O
5. a. Write an equation to show that HPo, (aq) can act as a Brønsted base in water. b. Label the species in (a) as acid, base, conjugate a cid and conjugate base respectively c. For the following equilibrium at 298 K, the equilibrium constant К- 2.84 х 10 2 М. Ag PO45) + H,O() = 3Agʻ(aq) + HPO, (aq) + OH (aq) Calculate the concentration of Ag in 0.10 M HPO. solution at pH 10.
Write balanced net ionic equations for the following reac-tions, and label the conjugate acid-base pairs:
G.140.
The base protonation constant K, of allantoin (C,H¸N,O,NH,) is 9.12 x 10 °. 4 3 Calculate the pH of a 0.46 M solution of allantoin at 25 °C. Round your answer to 1 decimal place. pH = || %D
The pH for a solution with a [H3O]+ of 1.0 x 10^-6 is
a. A study of the acid shows that the pH of an acid HA 0.12 MIK 2.62. What is the K, of this acid?
6. Draw two graphs for weak acid HA: (a) percent dissociation for HA versus the initial concentration of HA ([HA]o) (hint: assume [HA], as x and [H*]/[HA], as y). (b) the equilibrium concentration of H+ versus [HA]o. Explain both.
83. Determine the pH of each solution and classify it as acidic, basic, or neutral. (a) pOH = 8.5 = 4.2 (b) pOH (c) POH = 1.7 (d) pOH = 7.0
8:35 : Question 22 of 23 Submit Which one of the following correctly shows the weak acid equilibrium for trichloroacetic acid, CCl,COOH? A) CCl,COOH (aq) = CCl;CO* (aq) + OH- (aq) В) Cli,COOH (аq) + H,0 (I) — СCl,COOH, (aд) + ОН- (аф) C) CCl,COOH (aq) + H20 (1) = CCI,COO- (aq) + H30* (aq) D) CCl;COOH (aq) + H2O (I) CCl,CO(OH), (aq) + H* (aq) Tap here or pull up for additional resources
The pH of a 0.0060 M solution of HNO₃ is