Video Solution: Write an equation for the Brønsted–Lowry acidR...

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Organic Chemistry / Acid and Base Conjugates / Problem #15914

Write an equation for the Brønsted–Lowry acid–base reaction that occurs when each of the following bases react with water. Show all unshared electron pairs and formal charges, and use curved arrows to track electron movement.

(a) H3C–C≡N:

Video Transcript

So, now here we've got on how alkane, right? Notice how it doesn't have that hydrogen, so that means this carbon has three bonds and what? a lone pair, right? An a negative charge, so we've got a base right here, right? And we got on water, so what's going to happen, this is going to come in grab this water to take electrons onto that O, so then what do we get? we get H3C, right? O and remember we've got two lone pairs on this oxygen, we've got a H3C, C, triple bond CH now and then we've got just our hydroxide with three lone pairs and a negative charge, right? Alright, so let's move on.

Use curved arrows to show the movement of pair of electrons in the following acid-base reaction and show the structure of the conjugate base and the conjugate acid.

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Identify the acid, base, the conjugate acid and the conjugate base in each of the equations. 

 

1. HCl + NH3 ––> NH4+ + Cl- 

 

2. OH- + HCN ––> H2O + CN-

 

3. PO43- + HNO3 ––> NO3- + HPO42-

 

4. HCO3- + HCl ––> H2CO3 + Cl-

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What is the conjugate base of Phosphoric Acid, H3PO4 ?

a) HPO42–

b)H2PO42–

c)HPO42–

d) H2PO4

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Label the acid, conjugate acid, base and conjugate base in the reaction below. 

 

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Give the conjugate bases of the following molecules.

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The following is a stepwise synthesis by applying Bronsted-Lowry (B-L) and Lewis acid-base (LA and LB) reactions. Please use electron-pushing arrows to show this transformation logically.

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Write the conjugate acid and conjugate base of the following ion: H 2PO4 1-

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Consider molecule A shown below. Remember that for a Lewis structure, you must show all atoms, all bonding valence electrons, all nonbonding valence electrons, and all nonzero formal charges.

Using Lewis structures for reactants and products and using curved arrows to show the flow of electrons in molecule A, give the chemical equation that shows the heterolytic dissociation of one of the three CH bonds in molecule A to give H+ and the corresponding conjugate base. If resonance structures exist for the conjugate base, give all important resonance structures for the conjugate base. Clearly give the numerical value of the HCC bond angle in this conjugate base of molecule A.

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The two substances which are both acids are:

a. HC ≡ CNa and HC ≡ CH
b. CH3NH2 and CH3NHNa
c. CH3NH2 and HC ≡ CH
d. HC ≡ CNa and CH3NH2
e. HC ≡ CNa and CH3NHNa
 

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