The more acidic compound has to be predicted among the given pair of compound. Concept Introduction: Acids donate protons, base accepts protons. The strength of the acid can be said by finding the willingness of the acid to give proton. An acid giving away the proton can be represented in the form of equation as shown below, H − A ⇌ − H + A − If the acid “HA” is very much willing to give the proton it holds means then it is known as a strong acid. If it is not very much willing means it is a weak acid. The strength of the acid can be figured out by looking into the conjugate base that is formed on removal of proton. After loss of proton, a negative charge will be created. If the formed negative charge is more stabilized means then the acid is a strong acid and if it is not stabilized means then it is a weak acid. There are few factors which determine the strength of the acid and they are, What atom the charge is present Resonance Induction Orbitals If the charge is on a more electronegative atom, then it is stabilized more. Hence, the compound will be more acidic. If the negative charge is made to participate in resonance, then the negative charge will be stabilized. This increases the stability of the conjugate base and in turn the compound will be more acidic. Pull of the electron density by the more electronegative atom is known as induction. The inductive effects can stabilize or destabilize the conjugate base. If the inductive effect stabilize the conjugate base, then the compound will be acidic. The orbital in which the negative charge is present also plays an important role in stability of the conjugate base. A negative charge on s p hybridized orbital is more stable than the negative charge that is present on s p 3 hybridized orbital. In order to find whether the compound is more acidic or not, the first step is to remove the proton to form conjugate base. Then look for the above four factors.

Question

Want to see the full answer?

Answer 1

Question

Chapter 3.5, Problem 3.31P

Interpretation Introduction

Interpretation:

The more acidic compound has to be predicted among the given pair of compound.

Concept Introduction:

Acids donate protons, base accepts protons. The strength of the acid can be said by finding the willingness of the acid to give proton. An acid giving away the proton can be represented in the form of equation as shown below,

H−A ⇌−H+ A−

If the acid “HA” is very much willing to give the proton it holds means then it is known as a strong acid. If it is not very much willing means it is a weak acid. The strength of the acid can be figured out by looking into the conjugate base that is formed on removal of proton. After loss of proton, a negative charge will be created. If the formed negative charge is more stabilized means then the acid is a strong acid and if it is not stabilized means then it is a weak acid.

There are few factors which determine the strength of the acid and they are,

What atom the charge is present

Resonance

Induction

Orbitals

If the charge is on a more electronegative atom, then it is stabilized more. Hence, the compound will be more acidic.

If the negative charge is made to participate in resonance, then the negative charge will be stabilized. This increases the stability of the conjugate base and in turn the compound will be more acidic.

Pull of the electron density by the more electronegative atom is known as induction. The inductive effects can stabilize or destabilize the conjugate base. If the inductive effect stabilize the conjugate base, then the compound will be acidic.

The orbital in which the negative charge is present also plays an important role in stability of the conjugate base. A negative charge on sp hybridized orbital is more stable than the negative charge that is present on sp3 hybridized orbital.

In order to find whether the compound is more acidic or not, the first step is to remove the proton to form conjugate base. Then look for the above four factors.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

1) Draw the structures of D-lysine and L-lysine and assign R/S configuration (showing your workings). 2) Draw the predominant ionisation forms of the free amino acid lysine, at pH 1.0, 8.0, and 11.0. pKa values: 2.2 (-COOH), 9.0 (α-NH3+), 10.5 (side-chain). 3) Calculate (showing your workings) the % of the different ionized species that are present in a 1.00 M solution of L-proline at pH = 10.0. pKa values: 1.95 (- COOH), 10.64 (α-NH3*). 4) a) Draw the tripeptide Tyr-Pro-Lys once with a trans peptide bond between Tyr and Pro and once with a cis peptide bond between Tyr and Pro. b) The electrospray ionization mass spectrum (ESI-MS) of the tripeptide you designed in part (a) shows peaks indicative of mono-protonation and di- protonation of the tripeptide. At what values of m/z would these peaks be expected (no fragmentation)? Briefly explain your answer (showing your workings). 5) How could the sequence of Ala-Met-Thr be distinguished from that of Thr-Ala- Met by tandem ESI-MS-MS?…

LABORATORY REPORT FORM Part I. Determination of the Formula of a Known Hydrate 1. Mass of empty evaporating dish 3. Mass of hydrate Using subtraction or mass by difference, find the mass of the hydrate 76.96 -75.40 75.40g 76.968 1.568 01.56 76.90 g 2. Mass of evaporating dish + hydrate 4. Mass of evaporating dish + hydrate (after heating) First 76.98 g Third 76.66g Second Fourth (if necessary) 76.60g 5. Mass of anhydrate 6. Mass of water lost by the hydrate 7. Percent of water of hydration (Show Calculations) 8. Moles of water (Show Calculations) mol mass of water = MM of water (g/m) 9. Moles of anhydrate (Show Calculations) 10. Ratio of moles of water to moles of anhydrate 11 F(Show Calculations) 11. Formula of hydrate - Mass of water (g) x 100 % water hydration g g % Mass of hydrate (9) x IC % = (Mass of hydrate- mass of an) mass of hydrate (g) % = (1.569- × 100= mol 1.569 mol Mol Mass of anhydrate/MM of anhydrate 12. What was the color of the hydrate? blue What was the color of the…

compared t-critical with t-calculated and 95% confidence interval to answer this question