Q 6.5You have been given thefollowing equilibrium:HCN (aq) + HCO₂ (aq) = (N¯ (aq) +if K<1, what issystem?a) CN-what is theb) H ₂ CO 3H₂ (O3(aq)strongest base in thec) HCO 3d) H ( N

A strong acid or base has a weak conjugate base or acid. A weak acid or base has a strong conjugate…

Q 6.5 You have been given the following equilibrium: HCN (aq) + HCO₂ (aq) НСО = (N¯ (aq) + H₂CO3(aq) if K<1, what is the strongest base in the system a) CN- b) H ₂ CO ₂ c) HCO ₂ d) H (N 3

Q 6.5 You have been given the following equilibrium: HCN (aq) + HCO₂ (aq) НСО = (N¯ (aq) + H₂CO3(aq) if K<1, what is the strongest base in the system a) CN- b) H ₂ CO ₂ c) HCO ₂ d) H (N 3

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: Consider the following acidic equilibrium: H₂CO3(aq) + H₂O(1) HCO3(aq) + H3O*(aq). If you add NaHCO3…

A: According to Le-Chatelier's principle, if the equilibrium reaction is disturbed by changing…

Q: F(aq) is a weak base. Which equilibrium corresponds to the equilibrium constant K for F(aq)? Oa.…

A: According to Bronsted-Lowry concept base is a substance that always attracts protons from other…

Q: Calculate [OH-] for each solution and determine whether the solution is acidic, basic, or…

A: We have hydronium Ion Concentration as 7.5 * 10-5 M, 1.5 * 10-9 M, 1.0 * 10-7 M . We have to…

Q: 1. All are examples of Lewis acid-base reactions except (A) Cu²+ (aq) + 4NH3(aq) [Cu(NH3)4]²+ (aq)…

A: According to Lewis acid-base concept acid is electron pair acceptor and base is electron pair donor.…

Q: 5. Consider a weak acid HX. If a 0.10 M solution of HX has a pH of 4.27 at 25 degrees C, what is AG…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Which of the following would be the acid equilibrium equation for HONH₃Cl? A) HONH₃⁺ (aq) ⇌ NH₃ (aq)…

A: Given reactions A) HONH₃⁺ (aq) ⇌ NH₃ (aq) + OH⁻(aq) B) HONH₃Cl (aq) ⇌ HONH₃⁺ (aq) +…

Q: stion 26 Which of the following is an example of a covalent bond? A) K - CI B) AI - CI c)A- CI D) Al…

A: Note: According to our guidelines we are supposed to answer only one question. Kindly repost other…

Q: group of students are trying to determine whether a base is an Arrhenius base or a Bronsted-Lowry…

A: An Arrhenius acid is a substance which can donate protons while an Arrhenius base can donate…

Q: 4. Rank the following in INCREASING acidity: (a) A>B>C (b) C> B>A (c) B>A>C (d) C> A>B (e) A > C> B…

Q: Identify which of the following compounds CANNOT be classified as a Bronsted-Lowry base: H3C Na IV…

A: Bronsted–Lowry base is a proton acceptor. Bronsted-Lowry Acid is a proton donor.

Q: What type of ion is Na+?

Q: Consider the reaction below. Which species are the Brønsted-Lowry acids? HNO₂(aq) + NH3(aq) =…

A: Brønsted-Lowry concept: Brønsted-Lowry acid: a substance that can donate or looses a proton (H+). HA…

Q: Questio Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: The salt given is C3H7NH3Br Since there is a proton on N in the salt ( cation C3H7NH3+ and anion Br-…

Q: In the following reaction, what is the function of the bolded substance? H2CO3(aq) + H2O(l) ⇌…

A: We know that Acid : Acid is substance that gives H+ ion. Base : Base is substance that Accept H+…

Q: Identify acid, conjugate acid, base and conjugate base in the reactions below: →NH4* (aq) ◆ +H₂O (1)…

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: Which is a polar covalent bond? O CEC OC-F OH-H O C-C O C=C

Q: An aqueous solution of which of the following salts are basic? A) NANO3 B) K:SO: C) NH:CI D) NaBr E)…

A: A solution of any salt will be basic if it is formed by strong base and weak acid.

Q: Directions: Identify the Brønsted acid and base in the following reactions and give the…

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

Q: Which of the following statements is/are TRUE? Choose all that apply. O Select all that apply A H,Se…

Q: grade 12 chemistry: In the following reaction, what is the function of the bolded substance?…

A: The species which can give (donate) H+ in the solution are acids and the base formed by them are…

Q: In the equilibrium, HCO32-(aq)+NH3(aq)⇄CO32-(aq)+NH4+(aq), CO32- is the a acid b base c conjugate…

A: Conjugate base : Substance formed when acid loses H+ ion

Q: 5. In the reaction: Bronsted would identify which of the following species as acids? H₂PO4 (aq) +…

A: According to Bronsted acids are the species which donates proton (H+) while bases are the species…

Q: 5. The dissociation reactions for several acids and their equilibrium constants are given below:…

A: The acid dissociation constant (Ka) of an acid is used to distinguish between strong acid and weak…

Q: 4. H2O + HCl = H3O* + Cl 5. NH3 + HF = NH,* + F

Q: Liquid hexane (CH₂(CH₂) CH₂) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide…

A: The objective of this question is to calculate the percent yield of water from the reaction of…

Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: Given, the chemical reaction is as follows,C6H5NH2(aq) +H2O(l) → C6H5NH3+(aq)+ OH-(aq)we are asked…

Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

A: According to Bronsted-Lowry acid-base theory, a pair of substances which differ by proton (H+) ion…

Q: 2. Calculate the [ H*] of each of the following given the pH and pOH c) pOH = 2.5 d) pOH = 3.4

A: The pH of a solution depends upon the concentration of H+ ions present in it. It is calculated by…

Q: Which of the following is a Lewis acid? A) Fe3* B) CN C) NH3 D) SCN

A: In this question we have to tell that which is act as lewis acid.

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

A: GIVEN :- (a) [OH-]= 0.00045 M; (b) [OH-]= 8.8 X 10-9 M; (c) a solution in which [OH-] is 100 times…

Q: 33. Which set represents a conjugate acid/base pair? (A) H₂PO. and HPO (C) H₂PO. and H₂PO 34. For…

A: The objective of this question is to show the given chemical equations contain species that,…

Q: Which of the following compounds are Lewis acids? Select all that apply OS O AIF, U (CHINH ONH₂ Fe…

A: The electron pair acceptor is a Lewis acid and electron pair donor is a Lewis base.

Q: For each of the weak acids listed below, a) write a balanced equilibrium equation showing the…

A: Using ionisation of acids . We find ka by which we can determine weak acid .

Q: What is the original molarity of a solution of HF whose pH is 1.7 at equilibrium?…

A: The quantity pH, or "power of hydrogen," is a numerical representation of the acidity or basicity…

Q: 16.73 Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This…

Q: Question 2 In which reaction does bicarbonate act as a Bronsted-Lowry base? O HCO (aq) + NaOH (aq) →…

Q: Consider the reaction below. Which species are the Brønsted-Lowry bases? HPO2 (aq) + NO¿(aq) = PO³…

A: A species which accepts H+ is called a Bronsted base

Q: Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its…

A: Acids and bases are defined on the basis of theories, According to Bronsted-Lowry theory, acids are…

Q: of the following is not a property of acids? (a) They release hydrogen ions in solution. (b) They…

A: Equilibrium is a state of a reaction at which rate of forward reaction become equal to rate of…

Q: What is the [H30*] and pH of a 0.350 M HF solution? The Kg of HF is 3.5 X 104.

A: ★ Answer : [ H3O+] = 3.5×10-3 and pH = 2.46 of HF solution. ★ Solution : Weak acids dissociated…

Q: pH and pOH or

Q: Please arrange the following according to increasing acid strength

Q: Will a solution whose [H] = 5.04 x 10 be acidic, basic or neutral?

A: Given : Concentration of H+ ions=5.04×10-3 To identify : The nature of solution

Q: In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and…

A: SOLUTION: Step 1: A Bronsted-Lowry acid is a chemical species capable of donating a proton or…

Q: Complete the balanced molecular reaction for the following weak base with a strong acid: NaCIO2(aq)…

A: Given,

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

Q 6.5
You have been given the
following equilibrium:
HCN (aq) + HCO₂ (aq) = (N¯ (aq) +
if K<1, what is
system?
a) CN-
what is the
b) H ₂ CO 3
H₂ (O3(aq)
strongest base in the
c) HCO 3
d) H ( N

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

Step 2

Step 3

Step 4

Step 5

Step by step

Solved in 5 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

10. Which side of the equation does the acid-base equilibrium favor? вхь о: `ОН + a : + b ОН
Which of the following equations represents the acid equilibrium associated with Ка, for H, PO,? A) HPO,2 (aq) + H,O (1) = PO, (aq) + H,O* (aq) B) H,PO, (aq) + H,O (1) = H̟PO, (aq) + H,O* (aq) C) H̟PO, (aq) + H,O (1) = H̟PO, (aq) + OH (aq) D) H,PO, (aq) + H,O (1) = HPO,* (aq) + H,O* (aq) 80 DII DD F2 F3 F4 FS F9 F11 @ $ & ( 2 3 4 6 8 9 W E R S D F G K C V B N M I
Assuming the forward reactions are favored in the chemical equations below, arrange the acids according to INCREASING acid strength. HNO2(aq) + HCOO (aq) = NO2 (aq) + HCOOH(aq) HN3(aq) + Bro¯(aq) - N3¯(aq) + HBrO(aq) N3- + HCOOH(aq) = HN3(aq) + HC00"(aq) Your answer: HN3 HBRO HNO2 НСООН
In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base. C2H;NH,(aq) + H,0(1) — CHNH3" (aq)(аq) + он (аq) В-L В-L The formula of the reactant that acts as a proton donor is The formula of the reactant that acts as a proton acceptor is
4. a) Indicate the Bronsted acid and its bases in the following reactions: H2CO3 + NH3 → HCO3- + NH4 + SO32- + H2O → HSO3- + OH- CH3COO- + HCN → CH3COOH + CN- b) State why the following solutions are acidic, basic or neutral. NaOCl (aq), KCl (aq), NH4NO3 (aq)
12) Based on the acid structures below, which option ranks the acids in order of increasing K.? HO CH H3C HO HO HO, A B a) A< B
6:15 Question 18 of 22 Construct the expression for Ka for the weak acid, HC,H,O4. Ka = HC,H,O,(aq) + H2O(l) = HgO*(aq) + C,H,O, (aq) 1 Based on the definition of Ka, drag the tiles into the numerator or denominator to construct the expression for the given acid. Submit [H₂O] [H3O+] [OH-] [H₂C9H₂O4*] [C₂H₂O4] 2[H₂O] 2[OH-] 2[HC₂H₂O4] 2[H₂C9H₂O4*] [H₂O]² [H3O+]² [OH-]² [H₂C9H₂O4*]² [C₂H₂O₂-]² Tap here or pull up for additional resources RESET [HC₂H₂O4] 2[H3O+] 2[C9H₂O4] [HC,H,O]
What is the pH of 25.0 mL of 0.01M H2SO4 strong acid solution?
14) What is the percent ionization of a 5.3 X 10 M HCN solution? The Ka of HCN is 4.9 X 10". HCN (aq) + H20 (1) H;O* (aq) + CN (aq)
Identify each of the substances in the reaction as acid, base, conjugate acid, or conjugate base. HSO, (aq) H¸O(1) 1, SO,² (aq) H,O*(aq) 31 --
6) Phenol is an organic compound that behaves as a weak acid. In water, it ionizes as shown below. C6H5OH = C6H5O+H* If a 0.71 M aqueous solution of phenol has a pH of 5.02, what is the K, for phenol?
Which of the following bases is the weakest? The base is followed by its K, value. O C,H,N, 1.7 x 109 O CH,CH,NH, 5.6 x 10 O (CH,CH,),N. 5.2 x 10 O NH,, 1.76 x 10 O HOCH,CH,NH, 3.2 x 10