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- Write these reactions as proton-transfer reactions. Label which reactant is the acid and which is the base, which product is the conjugate base of the original acid, and which is the conjugate acid of the original base. In addition, write Lewis structures for each reactant and product and use curved arrows to show the flow of electrons in reaction. Q.) H2O + NH4+ -----> H3O1 + NH3I Normal 1 No Spac.. Heading 1 Heading 2 Title Styles Paragraph 5. Fill in the following table: [H3O"] РОН [OH'] ACID or BASE pH 7.21 9.84 x 10° M 3.25 2.64 x 102 M 2.49Drive-Google X Logout Successhil X O- Mail- Mariin, And X e Kegistration-Lifer X Sign pw.com/iln/takeAssignment/takeCovalentActivity.do?locator=assignment-take Clear All (C,H3),NH, Stronger Bronsted-Lowry acid Weaker Bronsted-Lowry acid NO, (C;H3)½NH Stronger Bronsted-Lowry base HNO2 Weaker Bronsted-Lowry base Cengage Learning | Cengage Technical Support a W
- C6H5NH2 + H2O <-> C6H5NH3+ + OH-. Aniline, a weak base, reacts with water according to the reaction. (a) a sample of aniline is dissolved in water to produce 25.0 mL of 0.10 m solution. The pH of the solution 8.82. Calculate the equilibrium constant, Kb, for this reaction (b) What is the percent disassociation for the solution in part (a) (c) 25.0 mL of 0.10 HCI was then added in a titration experiment. What is the pH at the equivalence point?I'm asked to "assume that ozempic is in a solution at pH = 7. Draw the functional groups at their correct protonation form". For this, would I make all of the carboxyl groupsgo from COOH to COO-? and then the amide groups go from CONH to CONH3 + ? What about ether groups (COC) ?Consider the molecules R-CH2OH and R-CH2CO2H where R is rest of the hydrocarbon molecule. a) Which has the stronger conjugate base? b) Explain why it is the stronger base. What about the structure helps us to understand why one is stronger than the other? You may use drawings to help explain your answer.
- 1) Complete the following reactions and identify the acid, base, conjugate acid and conjugate base. CH;CH,NH2 (aq) + H2O (1) a) CH;COOH (aq) + H,O (I) b) c) Identify the conjugate base and conjugate acid of each of the following. Conjugate Base Molecule Conjugate Acid HCO3 H20 HSO4- H2PO4Consider the reaction below. Then select all that are true about this reaction. CH,CH₂ÖH H CH,CH,OH + Cr This reaction is a Bronsted-Lowry acid base reaction This reaction is a Lewis acid base reaction The curved arrows are correct for this reaction The curved arrows are incorrect for this reaction CH3CH2OH is a base CH3CH2OH is an acid Give detailed Solution...don't give Handwritten answer3. For the following acid - base reaction, (a) predict the products; (b) identify the Bronsted acid, Bronsted base, conjugate acid, and conjugate base; (c) use curved arrows to show the flow of electron pairs in the reaction. CH3 CH2C-OH + NaNHa
- Question 2 Consider the following Bronsted-Lowry acid/base reaction. (Note that not all hydrogens or lone pair electrons are drawn in) [1] Draw the products of the reaction [2] Use curved arrows to show the movement of electrons to form the products. Be sure to draw in lone pairs of electrons if they are directly involved in a step. [3] Label the acid, base, conjugate acid, and conjugate base [4] Indicate which side equilibrium will favor and explain why. H H 3 E 80 Na NH₂ $ 4 a F4 R % 5 F5 T 6 F6 Y F7 UCH;COOH so,?- CH;COO HSO; Brønsted-Lowr Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry acid base In this reaction: The formula for the conjugate O of CH3COOH is The formula for the conjugate of SO,- is Submit Answer Retry Entire Group 9 more group attempts remaining Use the References to access important values if needed for this question. Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. HCIO co,²- CIO HCO; Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugat v e of HCIO is acid base The formula for the conjugate 8 of CO,2 is Use tne Keierences to access important values iI neeaea ior this question. Identify whether each species functions as a Brønsted-Lowry acid a Brønsted-Lowry base in this net ionic equation. HCIO H,S (aq) + HS CIO Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugate 8 of HCIO is The formula…Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline Pyridine NH3 CH;NH2 CH5NH2 C,H;NH, C;H;N NH,+ CH;NH3+ CH;NH3* CH;NH3+ C;H;NH+ 1.8 × 10-5 4.38 x 10- 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 2. Compute for pKb. (round off final answer to 2 decimal places)