Answered: NH,+ + H,O- NH; + H,O* pK, 9.24 pK-1.74…

Science

Chemistry

NH,+ + H,O- NH; + H,O* pK, 9.24 pK-1.74 NH, + OH-–→ NH, + H,0 pK_ 9.24 pK, 15.7 Explain why this rule works.

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter16: Amines

Section: Chapter Questions

Problem 16.27P: 16-27 Guanidine, p/Ca 13.6, is a very strong base, almost as basic as hydroxide ion. NH NH2+ II II...

See similar textbooks

Related questions

Q: the dissociation constant of formic acid, HCOOH, with concentration 0.1M and pH 2.38 is: a) 1.8 ×…

Q: Calculate the pH of the following acid solutions at 25 °C: (a) 1.0 x 10-4 M H3BO3(aq) (boric acid…

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

Q: If the pKa of the indicator is approximately 6, to which of the following equivalence point will it…

A: A suitable indicator should have pH of color transition is given by the equation of pH.…

Q: Hydroxychloroquine is a weak Bronsted base.

Q: Which acid would you choose to combine with its sodium salt to make a solution buffered at pH 4.25?…

Q: Calculate the basic dissociation constant for pyridine, C5H5N, if the acid dissociation constant for…

A: Given that, Ka =5.9×10-6 Kb= ?

Q: The three pKa’s for phosphoric acid (H3PO4) are 2.1, 6.9, and 12.4. At what pH does [H3PO4]…

Q: Lysine (K) is a triprotic amino acid whose most protonated form has a charge of 2+. Its acid…

A: Lysine is a basic amino acid symbolized by K. It has amino group in its side chain.

Q: Assuming that base (B:) and acid (AH) are mixed in equal concentrations and using pKa values of acid…

A: Let the initial concentrations of base and AH be 1 M each. The pKa of AH is 3.5 and the pKa of BH+…

Q: “A typical vitamin C tablet contains H2C6H6O6. If two tablets are dissolved in about a cup of water,…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: Phosphoric acid (H3PO4) is tribasic, with pKa's of 2.14, 6.86, and 12.4. The charge of the ionic…

A: Given: pKa's of phosphoric acids are 2.14, 6.86 and 12.4. And the pH of the solution = 8

Q: A weak base has Kp 6.5x10-6. Calculate the pKa of the conjugate acid. Express your answer to two…

A: The dissociation constant of an aqueous solution of weak acid is known as the acid ionization…

Q: At 25°C, what is the hydronium ion concentration in the following with discussing your result:- )…

A: The hydronium ion concentration can be found from the pH by the reverse of the mathematical…

Q: Aqueous acids may be placed in order of acid strength according to their pka values. In the…

A: Titration methods can be used to determine the Ka of the acid thereby the strength can be known.…

Q: OUL UI 3 points. The boxes below contain a series of 0.1 M aqueous solutions of increasing pH where…

Q: 5. At 25°C, calculate the molar H3O+ and OH-1 concentrations of the following: a. 0.0300 M C6H5COOH

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

Q: Define pKa for a weak acid. What is the relationship between the value of the pKa and the strength…

Q: One way to determine the predominant species at equilibrium for an acid-base reaction is to say that…

A: The pKa value of species in an equilibrium is a useful factor to determine the predominant species…

Q: Calculate the percent dissociation of crotonic acid (C, H,CO,H) in a 0.53 mM aqueous solution of the…

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

Q: 1. Write the reaction for H₂S dissolving into water + 2. Write the expression for the Ka Ka = [ b.…

A: Both the questions have been solved in the following step.

Q: Q2 : At 25°C, K = 3.40 x 10-3 S m-1 for 0.00100 M NH4OH. Values of Lo are: NH4C1 = 0.01497, NaOH…

Q: What is the weight NaCH3COO of that must be added to 750.0 mL of 0.180 M acetic acid to form a pH =…

Q: A student prepared a 0.10 M solution of formic acid, HCHO, and allowed it to be dissociated. The…

A: The equation for acid dissociation of formic acid is; HCHO ↔ H3O++…

Q: Cation: Mg2+ Fe3 PН-раper: pH-рарer: pH-рарer: | pH-раper: |PH-раper: Fe2+ Deionised water 5 3 1 3 5…

A: pH of a substance is its measure of the H+ concentration in the solution . A solution with high pH…

Q: Write the values of Y and X. H2SO4 CH;CH=CH2 + H2O CH3CH-CH2 H HỌ 2-propanol an alcohol The pKa of a…

A: The acid dissociation constant Ka is the representation of acidic strength of a solution and pKa is…

Q: The pKa of a weak acid (increases, decreases, is unaffected) if the equivalence point is increased…

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

Q: Formic acid, HCOOH, is the simplest of the carboxylic acids and occurs naturally, most notably in…

Q: What is the correct relationship between Ka and Kb for a weak acid and its conjugate base…

A: We know, Ka × Kb = Kw Kw is the ionisation constant of water.

Q: 4. What is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.26 at…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: What are some possible sources of error in determining the Ka value of an unknown acid except for…

Q: Which of the following is true about acids and bases? A. When bases ionize, they donate protons.…

Q: Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer…

A: Given: pH of buffer solution = 10.1

Q: Ethanoic acid is a weak acid pka value 4.74 at 298K. Calculate the pH value at 298K of: a 0.1M…

Q: The pKb for the propanoate ion, CH3CH2CO3 , is 9.126. What is the value of Ka (NOT the pKa) for…

A: Given-> pKb of CH3CH2COO- = 9.126

Q: B: At 25°C, what is the hydronium ion concentration in the following with discussing your result-…

Q: Calculate the pH of a 0.105 M solution of ethylenediamine (H,NCH,CH,NH,). The pKa values for the…

A: The pH of 0.105 M ethylene diamine solution is needed to calculated given that the pKa values of…

Q: f the Kb of a weak base is 8.7E-9, what is the Ka of its conjugate acid?

A: Conjugate acid is defined as a chemical compound formed when an acid donates a proton (H+) to a…

Q: How do I use the numbers given to find the masses in grams?

A: Preparation of a buffer solutionBuffer is a solution that can resist any change in its pH by the…

Q: In the laboratory, a general chemistry student measured the pH of a 0.590 M aqueous solution of…

A: Given: The concentration of ethylamine in the aqueous solution is 0.590 M. The pH of the solution is…

Q: The conjugate base that is produced after the first ionization step of carbonic acid when it has…

A: NOTE : Since you've asked multiple questions,we'll solve first question for you. If you want any…

Q: If you mix equal molar quantities of NH3 (Kb = 1.8 x 10-5) and CH3CO2H (Ka= 1.8 x 10-5), the…

A: Given that the solution contains equal molar concentrations of NH3 and CH3COOH. Also given Kb of NH3…

Q: Q1 :- What is the pK, of acetic acid, if K, for acetic acid is 1.58 x 10-6?

A: In multiple questions we solve only first question according to the Bartleby guidelines.

Q: Suppose a biochemist has 10 mL of a 1.0 M solution of a compound with two ionizable groups at a pH…

A: PH is a measure of how acidic or basic the solution is and it stands for potential of hydrogen and…

Q: 100.0 mL at pH= 12.000, [conj.base] = 0.500 M conjugate acid: HPO4 ^2- conjugate base: PO4 ^3-…

A: Buffer is a solution that resists the change in pH when small amount of acid or base is added to it.…

Q: The acid-dissociation constant, Ka, for gallic acid is 7.71 × 10-10. What is the base-dissociation…

A: Calculate the Kw (water dissociation constant) using the following equation: Kw = [H+] x [OH−] and…

Q: If the Kb value for a weak base is 2.6*10^-4, what is the value of its conjugate acid?

Q: When a 0.028M aqueous solution of a certain acid is prepared, the acid is 1.7% dissociated.…

A: The acid can be represented as HA. Acid dissociation constant of the reaction is given.

Q: Base: Sodium Acetate pka: 4.76 *pH value for conjugate acid (Acetic Acid) Soln. #1 Weak Base Strong…

A: As per Henderson equation- pH = pKa + log [B-]/[HB] [HB] = Concentration of acid [B-] =…

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

One way to determine the predominant species at equilibrium for an acid-base reaction is to say that the reaction arrow points to the acid with the higher value of pK_a. For example,

NH,+ + H,O- NH; + H,O*
pK, 9.24
pK-1.74
NH, + OH-–→ NH, + H,0
pK_ 9.24
pK, 15.7
Explain why this rule works.

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 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

Consider the following equilibrium between pentanoic acid and its conjugate base: | CH3CH,CH,CH2C0- H20 + H30+ CH;CH2CH,CH,C-OH Will lowering the pH shift the equilibrium to the right or to the left?
Between these two compounds, Be or CH,O, draw the Lewis structure of the stronger base. pk, values of organic and inorganic acids PK, Acid CH₂CH₂ NH₁ 1₂ 51 38 Ⓡ Acid 35 CHÍCHO 159 CHCOOH H₂O 15.7 H₂O CHÍNH "NH₂ H₂S 7,04 H200, 6.36 CH₂COOH 4.76 10.64 ₂50, 9.24 Hie 9985 pk, -1.74 52 Explicitly draw all Hatoms. . Include all valence lone pairs in your answer. -B d AIP [Ref
9:33 Time's Up! Submit Construct the expression for Kb for the weak base, N2H4. N2H4(aq) + H20(1) = OH (aq) + N2H;*(aq) 1 Based on the definition of Kb, drag the tiles to construct the expression for the given base. Kp = 5 RESET [H,O] [H;O*] [OH] [N2Hs] [N;H4] [N;H;] 2[H,O] 2[H,O*] 2[OH] 2[N2H5°] 2[N¿H«] 2[N2H3] [H,O]? [H,O*]? [OH]? [N;Hs']? [N;Ha]? [N2H3 ]? Tap here or pull up for additional resources
Given that K₂ for HF is 6.3 × 10-4 at 25 °C, what is the value of Kb for F¯ at 25 °C? Kb = Given that K for CH₂NH₂ is 5.0 × 10−4 at 25 °C, what is the value of K₂ for CH₂NH² at 25 °C? Ka || =
Pd(PPH3)4 PhBr (CH;CH2);N `NO2 Determine the produc of the rxn Ph Ph Ph `NO2 `NO2 `NO2 b. c. а. Ph Ph Ph Ph NO2 `NO2 `NO2 `NO2 d. е.
2 Using the table of pKa values in the inside cover of your textbook, find the pKa values for the acid and write it below the acid. The for each equilibrium tell which side does each equilibrium favors? HBr + s + OH H3C-C=CH + NHⒸ sé H3C- + Br OH NH₂
4. Predict the repeat unit for the following polymerizations: а. H2O2 CH3 b. NCO OCN
18). The formulas and the structures of two acids are shown below. Which acid is a stronger acid? If the acid strength of the two acids is equal, say so. Cl2CHCOOH CH3COOH но но CI-C-C-OH н-с-с-он ČI Ką = 0.0324 Ką = 1.82 x 10-5 %3D a. Cl¿CHCOOH is a stronger acid than CH;COOH. b. CH;COOH is a stronger acid than CI½CHCOOH c. The two have equal acid strength. d. none of the above
Consider the following reaction: CH, ÇH, + :çi-A-Ci: H,C- A-: H,C- 50 CH3 Based on the reaction above, the reactant which acts as a Lewis base is CAICL CAICIs o(CH);CCI O(CH),C* The product which is a Lewis acid is OAICI O(CH,),cCI CAICI o(CH)C" The following salts can replace AICla in the reaction, except OBeCl OMgCl OFeCl ocrCls
16-27 Guanidine, p/Ca 13.6, is a very strong base, almost as basic as hydroxide ion. NH NH2+ II II H2N—C—NH2 + H2O H2N—C—NH2 + OH" Guanidine Guanidinium ion pKb = 13.6 Complete the Lewis structure for guanidine, showing all valence electrons. The remarkable basicity of guanidine is attributed to the fact that the positive charge on the guanidinium ion is delocalized by resonance over the three nitrogen atoms. This delocalization increases the stability of the guanidinium ion relative to the ammonium ion or substituted ammonium ions. Draw three equivalent contributing structures for the guanidinium ion and show by the use of curved arrows how these three contributors are related. Propose an explanation for the fact that protonation occurs on the C=NH nitrogen rather than on one of the —NH., nitrogens. (Hint: Consider the resonance stabilization of the structure formed by protonation on a —NH., nitrogen compared with the resonance stabilization of the structure formed by protonation on the =NH nitrogen.) Predict the N—C—N bond angles in the hybrid. Which is the stronger acid, the ammonium ion or the guanidinium ion?
10:11 PM Sun Feb 5 < 5 T B 100% + : 0 DH₂07 2) Na₂Cr₂O₂, H₂SO4, H₂0 7 3). Ph Mg Br 4) +₂0 1 1 < N.
H 11602003) NaOH H₂O -S Br