Acid Base Chemistry
Acids are proton (donors or acceptors) and bases are proton (donors or acceptors).
Acids are proton donors and bases are proton acceptors.
Will a molecule with localized or delocalized electrons be more stable?
A molecule with delocalized electrons will be more stable - when electrons are able to delocalize/spread out over a large area, the molecule is more stable that it would be otherwise.
Consider this molecule: H3O+. Based on the fact that this molecule can donate protons, will it act as an acid or base?
Acid. Acids donate protons and bases accept protons.
Which is more electronegative: Oxygen (O) or Fluorine (F)?
Fluorine (F)
When a base gains a proton, it forms a ________ (conjugate acid or conjugate base)
Conjugate acid.
Acids have a pH (above or below) 7 and bases have a pH (above or below) 7.
Acids have a pH below 7 and bases have a pH above 7.
The carbon of a tertiary carbocation is attached to how many carbon groups?
Three.
Is a solution with a pH of 10 acidic, basic, or neutral?
Basic - basic solutions have pH's above 7.
Is this molecule polar or nonpolar: CH3OH
This molecule is polar - oxygen is an electronegative atom.
Which will act as a better acid: an amine or a carboxylic acid?
A carboxylic "acid." "Carboxylic acids are the most common organic acids and amines are the most common organic bases."
Which of the following acids is more acidic: HCl or HBr?
Cl and Br are in the same column, therefore we compare the size of them in order to compare their acidity. Br is a larger atom than Cl, therefore HBr is more acidic than HCl.
Is a conjugated carbon ring more or less stable than a carbon ring that is not conjugated?
A carbon ring that is conjugated is more stable than carbon ring that is not conjugated because conjugation is a stabilizing factor: conjugated molecules experience resonance and have delocalized electrons.
In a reaction, H2O gains a proton. The resulting compounds is called the _____________(conjugate base or conjugate acid).
The resulting compound is called the conjugate acid. In this case, H2O is acting as a proton acceptor. Therefore, it is acting as a base and will result in a protonated molecule (the conjugate acid).
Give the hybridization of the electrons on the oxygen atom in the following molecule: CH3-CH2-OH.
The electrons on the oxygen atom have the same hybridization as the oxygen atom itself. The oxygen atom is sp3 hybridized, therefore its electrons are sp3 hybridized.
Determine which of the following molecules is more basic: a molecule with a H+ concentration ([H+]) of
10-8 or a molecule with a H+ concentration of 10-4
Using the equation pH=-log[H+], you can determine that the molecule with a [H+] of 10-8 has a pH of 8 and the molecule with a [H+] of 10-4 has a pH of 4. Therefore, the molecule with a [H+] of 10-8 is more basic since bases have pH values above 7.
Will a solution with a pH of 2 have a higher or lower concentration of H+ ions than a solution with a pH of 9?
A solution with a pH of 2 is acidic...acidic solutions have high concentrations of H+ (protons) and basic solutions have lower concentrations of H+... therefore, the solution with a pH of 2 will have a higher concentration of H+ ions.
True or false: you can move a pair of pi electrons towards a sp2 carbon that is a doubly bonded carbon.
True. See example!
What is the conjugate base of H2O?
The question implies that H2O is acting as an acid, therefore H2O loses/donates a proton and the conjugate base is OH-.
Which of the following molecules contains the stronger C-C bond? CH3CH3 or CHCH?
The bond between the CHCH is a carbon-carbon triple bond, therefore it is the shortest bond and the strongest bond.
What is the Ka value of an acid with a pKa of 2.5?
Using the formula pKa=-logKa, you can calculate that the Ka value is approx 0.003. See board for explanation.
Explain why a carboxylic acid with a Fluorine substituent is more acidic than a carboxylic acid without a Fluorine substituent.
A carboxylic acid with a fluorine substituent experiences more inductive electron withdrawl, therefore increasing the strength of its acidity.
"The more stable the base, the stronger its conjugate acid"...... based on this concept, will a base that experiences resonance have a strong or weak conjugate acid?
Based on this concept, a base that experiences resonance will have a strong conjugate acid because resonance is a stabilizing factor.
A compound has a pKa value of 2.3. It is placed in a solution that has a pH value of 1. Will the compound be in its protonated or deprotonated form in this solution.
When the pH of the solution is below the pKa of the compound, the compound will be in its acidic (protonated) form. Therefore, this compound will be protonated when placed in this particular solution.
Give the hybridization of every carbon in the following molecule: CH3CH2CHCH2
C1:sp3
C2:sp3
C3:sp2
C4:sp2
In a reaction, the starting acid has a pKa value of 2 and the conjugate acid has a pKa value of 13. Will equilibrium favor the reactant or product side of this reaction?
Equilibrium favors formation of the weaker acid. Strong acids have low pKa values and weak acids have high pKa values. Therefore, equilibrium favors the product side of this reaction.