5. Complete the table:Chemical System1. 1 М КСI2. 1 M H2SO43.1 М КОН4. 1 M HE5. 1 M AI(OH)36. 1 М НСI7.1 M table sugarType of Substance| Intensity of LightClassificationTypeofsubstance- ionic, strongacid, strong base, weak acid, weak base, organic which is neither an acid norbase

Answered: Image /qna-images/answer/1328ce80-2f19-4ae2-8346-78311caebf44.jpg

Answered: trongacid, strong base, weak acid, weak…

Science

Chemistry

trongacid, strong base, weak acid, weak base, organicwhich is neither

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.54QE: Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+,...

See similar textbooks

Related questions

Q: Among the different pairs given below, one is not an acid-base pair, which one? NaHCO3 / HCO3-…

Q: Brønsted-Lowry base

Q: In this equation H2O +HF- H3O+ +F-1 H20 is a base and HF is its conjugated acid HF is an acid and F-…

Q: The less electronegative the anionic atom in the conjugate base, the better it is at accepting the…

Q: Br2 CH3CO,H (solvent and Lewis acid combined)

Q: When hydroxylamine acts as a base, which atom accepts the proton?

A: Acid base theory- Acids and bases have their own importance in chemistry. Acids and bases are…

Q: @ complete the reaction between the ions HCO₂ and HG₂₂OF HCO₂ + HC₂0₂ = He + List the conjugate acid…

A: The species which accept proton is known as base and the substance formed after accepting proton is…

Q: Hypothetically, what would be the conjugate acid of H3O+

A: Since, In addition of H+ we got conjugate acid. Thus,

Q: Identify the acid-base conjugate pairs for pyridine. O base: CSHNH2 conjugate acid: CSH3NH, base:…

Q: CHCI,COOH CH,CH,COOH CH;CICOOH CH3COOH Strongest acid Weakest acid

Q: Fluorosulfuric acid (HSO3F) is considered a superacid because it is stronger than sulfuric acid…

A: Super acids are a category of acids that are stronger acids than 100% pure sulphuric…

Q: Write the hydrolysis reaction for ethylamine, CH3CH2NH2 (aq). Below the reaction, label the Bronsted…

Q: In each row of the table, select the stronger acid or stronger base, as instructed.

A: By definition, 1) Basic strength is the tendency of an electron rich group/atom to donate its…

Q: Type one definition, description, property and example of an acid and a base using the format below.…

Q: Arrhenius defined bases or acids as ionic hydroxide compounds that dissociate into individual…

Q: A в thylammonium ethoxide ethylamine ethanol cronger base is njugate acid is

A: Stronger base = CH3CH2O- It's conjugate = CH3CH2OH

Q: C2H6 is C neither an an acid a base acid nor a base co03 - 2021 Acellus Corporation. All Rights…

A: This question is related to acid base chemistry.

Q: In any acid base reaction, equilibrium will always favor the side of the reaction with the a)…

A: A chemical equilibrium is the state in which rate of forward reaction and rate of backward reaction…

Q: This molecule can act as a base. H. н H-N-C HIU-I

A: it has the tendency to accept the H+ ions (or proton acceptor) called the bronsted-lowry base. also…

Q: Which of the following is a strong acid? O acetic acid Ohydrochloric acid Ohydrofluoric acid…

A: Acidity order

Q: label the acid,base, conjugate acid, and conjucate base pairs please answer number 2

A: A pair of substances which differ by H+ ion are called conjugate-acid base pairs HClO4 +H2SO4-…

Q: Consider the following three compounds: BF3, hydrazine, and cyclohexane. Identify each as a lewis…

A: According to scientist Lewis, electron deficient species are known as acids. Species which are rich…

Q: Which is the strongest base that can exist in liquid water? а. ОН- b. NH2 С. СНз- d. NH3

A: The strongest base that can exist in liquid water is OH-

Q: Rank the following solutions according to their acidity:

A: pH = - log[H3O+] pH + pOH = 14 pH = 14 - pOH

Q: Write a completed equation for the acid base pair shown below HCO2H + -NH2 to

A: These two chemical species HCO2H and NH2- are examples of Bronsted Lowry acid and base,…

Q: Write the conjugate base formulas of the following base: а. HF b. HNO3 c. HSO3

A: Conjugate base is formed after when an acid loses its proton.

Q: What is the correct increasing acidity arrangement? kindly explain

A: The acidity of a molecule is defined as its tendency to release a proton. The more stable the…

Q: conjugate acid of s is

A: In a Bronsted-Lowry acid-base reaction, a conjugate acid is the species formed after the base…

Q: Fill in the blank with the answer choices. v Choose... BrO is the of the pair HBRO / BrO- conjugate…

Q: When water acts as a Bronsted Base, what is its conjugate acid?

Q: Which is a stronger base and why?

A: The two bases given are LDA and KOt-Bu with below shown structures.

Q: How does molecular property of salicylic acid contributes its acidity?

Q: Show how methanol (CH3OH) can serve as both an acid and a base. Write an equation for the reaction…

A: Those compounds that could acid as well as base is known as amphoteric acid.

Q: Create a Diagram of the process of acid - base equilibrium -

A: Acid and bases maintain a chemical equilibrium in the solution by exchanging the protons from the…

Q: Which of the following is acting as an acid? CH3COOH + NH3 → CH3COO- + NH4+

A: According to Bronsted- Lowry Concept: An acid is defined as a substance which has a tendency to…

Q: conjugate acid and which is the conjugate base

Q: Classify Acetic Acid as one of the following Strong Acid, Strong base, Weak Acid, Weak Base, pH…

A: CH3COOH (acetic acid) is a carboxylic acid.

Q: Write the name of compound which act both as Bronsted acid and Bronsted base?

A: Bronsted acid is a H+ donor whereas base is a H+ acceptor.

Q: The following is a Bronsted acid-base reaction: HClO4 + NH3 ---> ClO4- + NH4+ Which of the following…

Q: Which is a stronger base? Must explain with both, words and structures.

Q: Identify the most acidic compound between the following molecules Draw the resonance structures of…

Q: the weakest base?

A: According to Bronsted-Lowry concept, base is defined as a species which accepts a proton whereas an…

Q: Classify Acetate ion as one of the following -Strong Acid,Strong Base, Weak Acid, Weak Base, pH…

A: Acids are the species which donate its proton (H+) or acts as electron pair acceptor. Bases are the…

Q: Within living cells, water can also act both as an acid and a base, that describes them to

A: ANSWER IS :

Q: Consider cyclohexane and benzene (draw the structures below). Draw the conjugate base of each…

A: Interpretation: We have to draw structure of cyclohexane and benzene.

Q: In a CH3COOH/CH3COO" pair, which among these is the base? A) CH3COO- (в) Both С) снзсоон D Neither

A: CH3COOH/CH3COO-

Q: Why does not an acid show any acidic behavior is the absence of water?

A: According to Arrhenius theory, acids are those compounds which when dissolved in water, dissociates…

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

5. Complete the table:
Chemical System
1. 1 М КСI
2. 1 M H2SO4
3.1 М КОН
4. 1 M HE
5. 1 M AI(OH)3
6. 1 М НСI
7.1 M table sugar
Type of Substance
| Intensity of Light
Classification
Typeofsubstance- ionic, strongacid, strong base, weak acid, weak base, organic which is neither an acid norbase

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

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 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

Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.
Both H2PO3−H2PO3− and HS−HS− are amphoteric. Write an equation to show how H2PO3−H2PO3− can act as a base with HS−HS− acting as an acid. Express your answer as a chemical equation. Identify all of the phases in your answer. then Write an equation to show how H2PO3−H2PO3− can act as an acid with HS−HS− acting as a base. Express your answer as a chemical equation. Identify all of the phases in your answer.
Consider the following five solutions: Solution A: [OH-] = 1.66 x 10-5 MSolution B: pH = 6.81Solution C: [OH-] = 5.62 x 10-12 MSolution D: pOH = 2.49Solution E: [H3O+] = 5.50 x 10-5 M Order each solution from most acidic (1) to least acidic (5).
Give any three examples of soft base ?
Which of the following happens to acid when it reacts with another substance? It receives a hydrogen ion. It receives a hydroxide ion. It donates a hydroxide ion. It donates a hydrogen ion. Define cohesion. Describe how the cohesive property of water is useful for living organisms.
For each conjugate acid-base pair, identify the first species as an acid or a base and the second species as its conjugate acid or base. In addition, draw Lewis structures for each species, showing all valence electrons and any formal charge. (a) CH3S- CH3SH
(THANKS FOR TUTORING ME) Have you ever been swimming in a pool, and your eyes were red when you get out? This means the chemicals in the pool were not adjusted correctly! More specifically, the measurement of the pool's pH was not quite right. pH is a measurement of hydronium ions and can be modeled by the function f(x) = −log10x. The variable x represents the amount of hydronium ions, and f(x) gives the pH level. Different liquids have ideal pH values that are different. Water at 25 degrees Celsius has a pH of 7. Anything that has a pH less than 7 is called acidic, and a pH above 7 is basic, or alkaline. Seawater has a pH just more than 8, whereas lemonade has a pH of approximately 3. Create a graph of the pH function either by hand or using technology. Locate on your graph where the pH value is 0 and where it is 1. You may need to zoom in on your graph. Use your graph to find the ideal pH level if the amount of hydronium ions is raised to 0.50. The pool company developed new…
Determine the pH of each of the following solutions. Ka and Kb values are given in the following table: Hydrazine (H2NNH2 ) Kb=1.3×10−6 Hydroxylamine ( HONH2 ) Ka=1.1×10−8 0.0084 M hydrazine 0.168 M hydroxylamine
Calculate the pH of the solution. Assume 1.0 L of solution. You must identify the type of solution before calculating the pH. Express all pH values to two decimal places. 0.100 moles HCl and 0.100 mole HC2H3O2 Ka (HC2H3O2) = 1.8 x 10-5
If a sample of a certain solution is determined to have a [H3O+] concentration of 8.94×10^−4 moles/liter, what is its pH? Round off your answer to one decimal place.
Use the formula pH=-log[H^+]. The variable pH represents the level of acidity or alkalinity of a liquid on the pH scale, and [H^+] is the concentration of hydrogen ions in the solution. Determine the value of [H^+] (in mol/L) for the following liquids, given their pH values. Express your answers in scientific notation with three significant digits. a.) Tea pH=5.5 b.) Milk pH=6.2 What is the concentration of hydrogen ions in tea? What is the concentration of hydrogen ions in milk?
What is the cation exchange capacity (in meq/100 g) and base saturation (in %) of a 150 g soil sample that contains the following amounts of exchangeable cations: 240 mg Ca2+, 69 mg Na+, 234 mg K+, 192 mg Mg2+, 54 mg Al3+, and 10 mg H+. Use the following molar weights: Ca2+ = 40 g/mol; Na+ = 23 g/mol; K+ = 39 g/mol; Mg2+ = 24 g/mol; Al3+ = 27 g/mol and H+ is 1 g/mol.