Answered: Construct the expression for Kb for the…

Construct the expression for Kb for the weak base, CN-. CN-(aq) + H:O(1I) = OH-(aq) + HCN(aq) Based on the definition of Kb, drag the tiles to construct the expression for the given base. Kp =

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 35Q: Consider the following mathematical expressions. a. [H+] = [HA]0 b. [H+] = (Ka [HA]0)1/2 c. [OH] =...

See similar textbooks

Related questions

Q: The acid dissociation constant K of boric acid (H,BO,) is 5.8 x 10. - 10 Calculate the pH of a 6.0 M…

Q: The acid dissociation constant K, of hypobromous acid (HBrO) is 2.3 × 10". Calculate the pH of a 1.2…

A: Given data set: Acid dissociation constant (Ka) for hypobromous acid (HBrO) = 2.3*10-9…

Q: In the laboratory, a general chemistry student measured the pH of a 0.548 M aqueous solution of…

Q: Write the acid dissociation constant expression for nitrous acid, HNO2.

A: Acid dissociation constant is the ratio of concentration of products to the concentration of…

Q: compute the degree of dissociation for a 0.1 M solution of acid HA, whose ionization constant 1x…

Q: Construct the expression for Kb for the weak base, CSHSN. C.H:N(aq) + H:O(() = OH-(aq) + CsH.NH"(aq)…

A: Kb is known as the base dissociation constant. It also tells us about the measure of how completely…

Q: What is the pH of a solution which is 0.021 M in weak base and 0.039 M in the conjugate weak acid…

A: We have a buffer system of weak base (0.021M) and conjugate weak acid (0 .039M) . We also have the…

Q: The weak acid, HA, has a Ka of 1.60 x 10-10. What is the Kb of its conjugate base, A™?

A: Given :- Ka for weak acid (HA) = 1.60 × 10-10 To determine : Kb of its conjugate base (A-)

Q: The ionization constant of methylamine, CH3NH2, (Kb) is 4.2 x 10–4. Write the dissociation equation…

A: Please find your solution below : Ionic Equilibrium is the equilibrium in which the ionic substance…

Q: If the pOH of a solution is 7.7, calculate [H*]. 50118723.362727247 1995262.314968879 0.000000501…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Pure sulfuric acid also autoionizes. Write the ion-product constant expression, Ksulf, and find the…

A: Autoionization or a self ionization is a process in which an atom or molecule in its excited state…

Q: 8. Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: Н. РО, + Н,О…

A: Equilibrium constant is defined as ratio of concentration of products to concentration of reactant.

Q: Consider the following data on some weak acids and weak bases: acid base K, formula formula name…

A: The word pH stands for the potency of hydrogen and it is used to measure the concentration of…

Q: Determine the pOH of a 0.461 M C6H5CO2HM solution if the Ka of C6H5CO2H is 6.5 x 10-5. C6H5CO2H +…

A: The acidity of an acid is determined by its pH. Lower is the pH, more acidic is the acid. The…

Q: Q_/ The acid-dissociation constant for chlorous acid, HCIO2, at 25C° is 1.0x10^-2 . Calculate the…

Q: The compound dimethylamine, (CH3),NH, is a weak base when dissolved in water. Write the K,…

Q: Calculate the pH and the pOH of these solutions: (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH = pOH…

Q: Which of the following bases is the weakest? The base is followed by its K. value. O CC,H,N, 1.7 x…

Q: Q3- The acid-dissociation constant for chlorous acid, HCIO,, at 25C is 1.0x10. Calculate the…

A: Concentration of HClO2 = 0.100 M Ka = 1E-2 Concentration of H+ ions = ?

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 x 10. Calculate the pH of a 4.8M…

Q: In the laboratory, a general chemistry student measured the pH of a 0.564 M aqueous solution of…

A: Quinoline is a heterocyclic aromatic compound and a colorless liquid with a strong odor. Quinolines…

Q: In the laboratory, a general chemistry student measured the pH of a 0.354 M aqueous solution of…

A: Given that: pH = 0.354 [C8H10N4O2] = 12.063 To find: Kb

Q: To what volume should 100 mL of any weak 0.30 molar monobasic acid (HA) or mono-acidic base (BOH) be…

A: According to the Le Chatelier principle, adding water to equilibrium would cause equilibrium left to…

Q: The acid dissociation constant K, of acetic acid (HCH3CO,) is 1.8 x 10. Calculate the pH of a 0.52M…

A: Given that : The acid dissociation Ka of acetic acid = 1.8 x 10-5 We have to calculate the pH of a…

Q: BiF5 is a strong Lewis Acid, forming adducts with simple Lewis bases such as ammonia and pyridine…

A: BiF5, being a strong Lewis acid, accepts electron pairs from Lewis bases such as NH3 and…

Q: Calculate the ph of 0.350 M acetic acid whose ionization constant is Ka= 1.8x10-5

A: Given :- concentration of acetic acid solution = 0.350 M Ka = 1.8 × 10-5 To be calculated :- pH…

Q: The base-dissociation constant (Kb) for this base is 1.7x109, If the pH of the solution is 9.15,…

Q: In the laboratory, a general chemistry student measured the pH of a 0.400 M aqueous solution of…

A: To find Kb for base, first write reaction of base with water and according to that, find [OH-] or…

Q: In the laboratory, a general chemistry student measured the pH of a 0.552 M aqueous solution of…

Q: The compound trimethylamine, (CH3)3N, is a weak base when dissolved in water. Write the K,…

A: Equilibrium constant : It is the ratio of the concentration of the product to that of the…

Q: Construct the expression for Ka for the weak acid, HPO,2". HPO, (aq) + H20(1) = H;O*(aq) + PO, (aq)…

Q: Hydrocyanic acid (HCN) is a weak acid. Write the mass action expression for its acid-ionization…

A: liquid water is not written in the mass law expression

Q: The acid-dissociation constant for chlorous acid, HCIO,, at 25C' is 1.0x10. Calculate the…

A: According to guidelines i can answer only first question. please repost with the second one given…

Q: 5. For the following acids: i. Name the following acids. ii. Identify if it is strong or weak acid.…

A: Since you have posted multiple sub-parts, the answer for first three sub-parts are given below.…

Q: Calculate the pH of a weak base which dissociates as BOH ⇌ B+ + OH- ( like NH3 (g) + H2O(l) →…

A: The dissociation reaction taking place is BOH ⇌ B+ + OH-

Q: In the laboratory, a general chemistry student measured the pH of a 0.522 M aqueous solution of…

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

Q: 8. K/U Write the base-dissociation constant expressions for the conjugate base of each of the…

Q: -9 The acid dissociation constant K, of hypobromous acid (HBRO) is 2.3 x 10 Calculate the pH of a…

Q: 3' 4. 6. 7. 6. 10 12 13 14 The acid dissociation constant K of alloxanic acid (HC,H,N,0,) is 2.24 x…

Q: 8. Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H,PO, + H̟O…

A: Given equations are :

Q: The base protonation constant K, of lidocaine (C4H2 NONH) is 1.15 x 10 . Calculate the pH of a 1.0 M…

Q: In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of…

Q: Construct the expression for Ka for the weak acid, NH,*. NH,*(aq) + H,0(I0) = H,0*(aq) + NH;(aq) 1…

A: The hydrolysis or ionisation reaction of weak acid is given as, => NH4+ (aq) + H2O (l) ------>…

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 x 10 '. а Calculate the pH of a…

Q: In the laboratory, a general chemistry student measured the pH of a 0.470 M aqueous solution of…

Q: Construct the expression for Ka for the weak acid, CH,COOH. CH,COOH(aq) + H,O(1) = H,0*(aq) +…

A: Expression of Ka The equilibrium constant expression is the ratio of the concentrations of a…

Q: In the laboratory, a general chemistry student measured the pH of a 0.591 M aqueous solution of…

Q: Calculate the PH of a solution that is 0.175 M benzoic acid and 0.110M sodium benzoate, a salt whose…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

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

100%

Construct the expression for Kb for the weak base, CN-.
CN-(aq) + H:O(1) = OH-(aq) + HCN(aq)
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]
[H.CN]
[HCN]
[CN]
2[H:O]
2[H:O*]
2[OH]
2[H.CN]
2[HCN]
2[CN]
[H:O]?
[OH]
[HCNJ?
[HCNJ?
[CNF

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

Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
12.63 For each of the following reactions, indicate the Bronsted-Lowrv acids and bases. What are the conjugate acid-base pairs? CN’(aq) + H2O(€) «=* HCN(aq) + OH’(aq) HCO}-(aq) + H,o+(aq) +* H2CO,(aq) + H,O(€) (C) CH,CtX)H(aq) + HS~(aq)i=i CH}COO"(aq) + H2S(aq)
Consider the following mathematical expressions. a. [H+] = [HA]0 b. [H+] = (Ka [HA]0)1/2 c. [OH] = 2[B]0 d. [OH] = (Kb [B]0)1/2 For each expression, give three solutions where the mathematical expression would give a good approximation for the [H+] or [OH]. [HA]0 and [B]0 represent initial concentrations of an acid or a base.
Composition diagrams, commonly known as alpha plots, are often used to visualize the species in a solution of an acid or base as the pH is varied. The diagram for 0.100 M acetic acid is shown here. The plot shows how the fraction [alpha ()] of acetic acid in solution, =[CH3CO2H][CH3CO2H]+[CH3CO2] changes as the pH increases (blue curve). (The red curve shows how the fraction of acetate ion, CH3CO2, changes as the pH increases.) Alpha plots are another way of viewing the relative concentrations of acetic acid and acetate ion as a strong base is added to a solution of acetic acid in the course of a titration. (a) Explain why the fraction of acetic acid declines and that of acetate ion increases as the pH increases. (b) Which species predominates at a pH of 4, acetic acid or acetate ion? What is the situation at a pH of 6? (c) Consider the point where the two lines cross. The fraction of acetic acid in the solution is 0.5, and so is that of acetate ion. That is, the solution is half acid and half conjugate base; their concentrations are equal. At this point, the graph shows the pH is 4.74. Explain why the pH at this point is 4 74.
Construct the expression for Kb for the weak base, ClO⁻. ClO⁻(aq) + H₂O(l) ⇌ OH⁻(aq) + HClO(aq)
The generic equation for a weak base in water is: ?+?2?⟷??++??−B+H2O⟷BH++OH− A 0.0500 M solution of a base is 7.5% ionized. Calculate the base ionization constant Kb Input the numerical answer. Remember significant figures. Do NOT round until the final answer. There are two fields in which to input the number. The exponent will go after the 10^ Kb = x 10^
Acid Formula Ka Acetic acid HCH3CO2 1.8*10^-5 hypochlorous acid HClO 3.0*10^-8 Base formula Kb ammonia NH3 1.8*10^-5 aniline C6H5NH2 4.3*10^-10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. Solution pH .1 M KCH3CO2 .1 M C6H5NH3Br .1 M NH4Cl .1 M KI
Ka for formic acid , HCOOH , is 1.80×10-4 . Ka for nitrous acid , HNO2 , is 4.00×10-4 .Ka for phenol (a weak acid) , C6H5OH , is1.60×10-10 .What is the formula for the weakest conjugate base? Ka for acetic acid , CH3COOH , is 1.80×10-5 Ka for nitrous acid , HNO2 , is 4.00×10-4 Ka for hypochlorous acid , HClO , is 3.50×10-8 What is the formula for the strongest acid?
Consider the following list when answering the questions that follow: C6H5CO2H , Ka = 6.3 x 10-5 C6H5CO2 - , Kb = 1.6 x 10-10 CN- , Kb = 2.5 x 10-5 HCN , Ka = 4.0 x 10-10 For the reaction between benzoic acid (C6H5CO2H ) and a solution containing cyanide ions (CN- ): (a) The name of the conjugate base produced is --- (b) The name of the conjugate acid produced is --- (c) The reaction is ----- favoured (type 'reactant' or 'product'), because the reactants are the ----- (type 'weaker' or 'stronger') set of acid and base.
The acid ionization constant, Ka, of a certain weak acid HA equals 1.4 x 10-11. What does Kb for the conjugate base, A- equal? Assume that the temperature equals 25 ˚C.
1. The hydroxide ion concentration, [OH-], of an aqueous solution of 0.429 M methylamine (a weak base with the formula CH3NH2) , Kb = 4.2×10-4, is: [OH-] = _________ M 2. The pH of an aqueous solution of 0.429 M aniline (a weak base with the formula C6H5NH2) is _______ 3.The hydronium ion concentration of an aqueous solution of 0.429 M diethylamine (a weak base with the formula (C2H5)2NH) is [H3O+] = __________ M.