Answered: Lewis Acid-Base Reactions 2.69 Label…

Lewis Acid-Base Reactions 2.69 Label the Lewis acid and Lewis base in each reaction. Use curved arrows to show the movement of electron pairs. О он a. CI- BCI3 + CI-B-CI CI CI b.

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: Find the p H of a 0.439 M N a A solution. The salt completely dissociates intoNaus and Anus, N a is…

A: Pka= -logka Use formula of PH of salt which is mixture of strong base and weak acid. PH=9.32

Q: 5. Which hydrogen is most acidic? На На 15/3 Ha Hb OMP Hb SP Hc -Hс Hd

Q: Name Period Directions: read each section and answer the questions accordingly. Show all…

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

Q: Which of the following acids has the strongest conjugate base? O A. succinic acid, Ka = 6.2 x 10-5…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: In the following reaction, identify the Bronsted-Lowry base and its conjugate acid. S(s) + 2 HBr(aq)…

A: Given Chemical Reaction : S (s) + 2 HBr(aq) --> H2S (g) + Br2 (l) Identify a pair of Base and…

Q: Given the reaction: HI + CN- ↔ I- + HCN What is the Bronsted-Lowry base in the forward reaction?…

A: The Bronsted acid are those which lose proton whereas Bronsted base are proton accepter.

Q: Which student is right??

A: According to Arrhenius theory base are those species which donates OH- ions in aqueous solution.…

Q: Rank the bold-faced hydrogens for the following compounds from most acidic to least acidic.

A: These are the compounds given, we need to find the most acidic protons.

Q: 6. Calculate the percent dissociation of 0.10 M hydrazoic acid (HN3, Ka= 1.9 x 10-5). Recalculate…

A: Answer: Hydrazoic acid is a weak acid and we have to study the common ion effect on its dissociation…

Q: What is the [H+] of a 0.075 M solution of the acid HA? The Ka for this acid is Ka = 4.8*10-8

A: The objective of the question is to find the concentration of hydrogen ions, [H+], in a 0.075 M…

Q: 2) Find the pH, the pOH, [H*] and [OH-] for the following strong acids or bases. a. A solution of…

A: pH is equal to negative logarithmic value of hydrogen ions concentration. pOH is…

Q: For the following reaction: Part: 0/2 Part 1 of 2 Ï + Identify the Lewis acid and the Lewis base. O…

A: A Lewis acid is a substance that accepts a pair of electrons. On the other hand, a Lewis base is a…

Q: 2. Answer the questions for the acid below: a) Write the acid dissociation constant, Ka, expression…

A: Given reaction: HA(aq) + H2O(l) ⇔H3O+(aq) + A-(aq) Acidic strength is…

Q: 4. Calculate the value of [H3O*]and [OH] in each solution: a. 0.0001 M NaOH b. 0.0001 M HCI

A: 4. Given,a. 0.0001 M NaOHb. 0.0001 M HClRequired, The value of H3O+ and OH- .

Q: A weak acid, HX, has a Ka of 1.00 x 10. If 0.0500 mole of HX is dissolved in 500 mL of water, what…

Q: For a weak acid HA solution of 0.50 M (Ka = 4.0 x 10-10) a. [H+] at equilibrium (to 3 significant…

A: Given: Concentration of weak acid HA= 0.5 M Ka for HA = 4.0×10-10

Q: 5. Answer whether the following questions are True or False. If false, fix the statement to make it…

A: PH =7 Neutral PH > 7 Basic PH< 7 Acidic PH = -log[H+]

Q: 3)CH3NH2 is a weak base (?b = 5.0×10-4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH…

A: Given, Kb of weak base CH3NH2 = 5.0×10–4 And , concentration of CH3NH3NO3 = 0.0450 M .

Q: Which are acid-base reactions according to Lewis theory but not according to the Bransted-Lowry…

A: Bronsted Lowry acid is a component which donate Proton while bronsted lowry base is a species which…

Q: 4 A solution is made by dissolving 24.7 g of LIC3H5O2 in 500.0 mL of water. a Does Li have any…

A: We are authorised to solve first three subparts of a question. Please post rest of the subparts…

Q: Given the following acids and K, values: HCIO, HOAC HCN HF Ix 10 1.76 x 105 4.93 x 10-10 3.53 x 10…

A: Given HClO4 = 1×107 HOAc = 1.76×10-5 HCN = 4.93×10-10 HF = 3.53×10-4

Q: 8. Given the following, what will be the approximate equilibrium pH of an aqueom of ammonium…

A: The problem is based on ionic equilibrium. Here we will be using pH for salt hydrolysis. The…

Q: Pyridine, C5H5N, is a pesticide and deer repellent, Its conjugate acid, the pyridinium ion C5H5NH+,…

Q: Find the pH of a a A solution. The salt completely dissociate and AminusNa is the cation of a strong…

A: NaA is salt so mixture of strong base and weak acid. So use formula of PH of salt. PH=9.32

Q: Predict the acid that has the smallest pKa+ O HBRO2 O HBRO3 O HBRO O They have the same relative…

A: the smaller the pKa value, the stronger the acid

Q: na 0.735 M solution, a weak acid is 12.5% dissociated. a. Calculate the [H;0* ], pH, IOH¯ ], and pOH…

Q: What is the calculated pH of the initial 0.100M Acetic Acid solution? Ka = 1.8 x 10-5 . Give your…

A: The dissociation reaction of acetic acid is given below: CH3COOH(aq) + H2O(aq) ⇌ CH3COO-(aq) +…

Q: b) conjugate acid pairs. i. ii. HCOOH + NH3 For the following reactions identify the acid-conjugate…

Q: Decide which molecule is the Lewis acid and which molecule is the Lewis base in the following…

Q: 10) Always a diligent chemist, you spend your free time thinking about the strengths of acids. How…

A: The dissociation of acid is given by: HA → H+ + A-Ka = H+ A-HA If the strength of the acid…

Q: 7. The ka for acetic acid is 1.0 x 10.5. Is acetic acid a weak or a strong acid?

A: Strong acids completely dissociate in aqueous solution (Ka > 1, pKa < 1).

Q: dentify the Lewis acid in the following reaction of acetone (CH.C(O)CH,) and boron trifluoride (BFs)…

A: A Lewis acid is a species that accepts electrons. It is positively charged or has vacant orbitals to…

Q: Identify the weaker base and the correct relative value of the equilibrium constant, K, for this…

A: Basicity of a compound depends on the electron density present on the donor atom like lone pair or…

Q: For the following reaction at equilibrium HCIO4 + H₂O →→ CIO4¹ +H30+1 HCIO4 is the H₂O is the CIO4¹…

A: According to Bronsted and Lowry concept an Acid is a substance that has the tendency to donate a…

Q: 6. If a buffer solution is 0.290 M in a weak acid (Ka = 3.3x10-) and 0.510 M in its conjugate base,…

Q: What is the base in the following reaction: HCI (aq) + H2O (1) --> Cl* (aq) + H3O* (aq)? a. Cl- b.…

Q: Calculate the molar concentration of [OH-] for a 0.5 M acetic acid solution. Ka = 1.8 × 10-5 a.…

A: Given molarity of acetic acid solution = 0.5 M Dissociation constant , Ka = 1.8 × 10-5

Q: 1. What is the pH of a 0.72M formic acid solution. Formic acid has a Ka = 1.8 * 10-4.

A: The problem is asking for the pH of a 0.72M formic acid solution. Formic acid is a weak acid, and…

Question

100%

Lewis Acid-Base Reactions
2.69 / Label the Lewis acid and Lewis base in each reaction. Use curved arrows to show the movement of electron pairs.
CI
O OH
a. CI-
+
BCI3
CI-B-CI
b.
+
CI
CI

Expert Solution

Step 1 lewis acid-base

Lewis acid accepts pairs of electrons whereas lewis base donates pair of electron.

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

What is the dissociation equation in water and equilibrium constant expression for the dissociation of the following weak acid. a. Hypochlorous acid, HOCl Ka = 3.0 x 10-8 b. propionic acid, CH3CH2COOH Ka = 1.35 x 10-5
Circle the solution in each pair with the Higher pH. Lactic acid Ka = 1.4 x 10-4 Hydrocyanic acid Ka= 6.2 x 10-10 a) 0.1 mol L-' hydrobromic acid or 0.2 mol L-' hydrobromic acid b) 0.1 mol L-1 sulfuric acid 0.1 mol L-' hydrobromic acid or c) 0.1 mol L-1 lactic acid 0.1 mol L-' hydrobromic acid or d) 0.1 mol L-l hydrocyanic acid 0.1 mol L-' lactic acid or e) 0.1 mol L-1 lactic acid or 0.1 mol L-1 sodium lactate
Acid Molarity pH HX 0.010 M 2.0 HY 0.10 M 3.0 HZ 1.0 M 3.0 Based on data in this table, place these 3 acids in order, from weakest (lowest Ka) to strongest (highest Ka): HZ HY HX HX HY HZ
Hi can someone please help with these?
Consider the following two equilibrium constant expressions when HSO3^- dissolve in water. Which of the expressions in the photo is corresponding to HSO3^- acting as an acid? (Choose one option) 1. a only 2. b only 3. a and b 4. neither a nor b
3. What is the pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid? (K, for acetic acid is 1.8x10-5.)
Question 8 of 20 Sub Complete the balanced molecular reaction for the following weak base with a strong acid: NaCIO2(aq) + H2SO«(aq) – 3- 2. 2+ 3+ 4+ 04- 1 6 7 8. 9. 01 D 07 9. 2 3 4. 6. (s) (1) (g) (aq) -> Na H2O H3O* OHT H. CI • x H2O Delete Reset W ? Questions prep ok étv A 山 T。 OCT 4. MacBook Pro 8. 11
Using the data in the table below, which is the weakest acid? Base Kp NH3 1.7 x 10-5 C2H5COO- 7.4 × 10-10 C6H5CO0- 1.6 x 10-10 C4H5O5 2.5 x 10-11 F- 1.5 x 10-11 a. NH4+ Ob. C2H5COOH Oc. C6H5COOH d. C4H6O5 Се. HF
MED PH +POH 1 = -log₁ PH+ Por pk 55. Of the following salts, which one forms a solution with the highest pH? A) KCI B) NH4Cl C) NaBr D) KCN ад, Гонт = 1/ A) HA (aq) + H₂O (1) B) A (aq) + H3O+ (aq) C) HA (aq) + OH- (aq) D) A (aq) + OH- (aq) (E)) A (aq) + H₂O (1) 56. HA is a weak acid. Which equilibrium corresponds to the equilibrium constant K for A? E) Ca(NO3)2 H₂A+ (aq) + OH(aq) HA (aq) + H₂O (1) H₂O (1) + H+ (aq) HOA²- (aq) HA (aq) + OH (aq) A) 3870 B) 9.88 C) 12.28 D) 6.16 E) 7.21 57. Why does the rate of a gas-phase reaction increase when the temperature of the system is increased? A) Increasing the temperature makes the molecules move faster, which results in more molecular collisions. B) Increasing the temperature gives the molecules more energy, so more reactant molecules have enough energy to react together. C) Increasing the temperature makes the volume increase, which provides more space for the product molecules to occupy. (D) Statements A and B are correct. 58. What is the…
• Answer each of the following for the following reaction HCl + H₂O → CI-¹ + H₂O+¹ is the acid is the base is the conjugate acid is the conjugate base HCI is a a. HCI b. H* c. H30+1 acid so we use the one-directional arrow d. CI-1 e. H₂O f. strong g. weak •Answer each of the following for the following reaction H₂SO3 + H₂O → HSO3-¹ + H₂O+¹ For polyprotic acids only one acidic hydrogen is removed by a very weak base such as water is the acid is the base is the conjugate acid is the conjugate base H₂SO3 is not on the list of seven strong acid so is treated like a a. H₂SO3 b. H* c. H30+1 d. HSO3-¹ e. SO3-² g. strong h. weak f. H₂O acid and we use a double-sided arrow
Which of the following statement best explain why the acidity of carboxylic acids is greater than those of the alcohols? a. Alcohols behave as neutral compounds in aqueous solution. b. Alcohol has the ability to donate proton to becomes a negative ion called an alkoxide ion, RO– c. When a carboxylic acid donates its proton, it becomes a negatively charged ion, RCOO−, called a carboxylate ion which is more stabilized by resonance. d. The OH group in alcohol is less charged and often more difficult to release electron for chemical reactions.
Show your work please, thank you!