Please arrange the following acids in order of increasing strength.

H3PO4 < H2PO4- < HPO4 ^-2

H2PO4- < H3PO4 < HPO4 ^-2

HPO4-2 < H2PO4- < H3PO4

H3PO4 < HPO4 ^-2 < H2PO4-

All of these acids have the same strength

Consider the following Ka values;

acetic acid Ka[CH3COOH (aq)] = 1.80 x 10^-5

chloroacetic acid Ka[CH2ClCOOH (aq)] = 1.40 x 10^-3

hypochlorous acid Ka[HClO (aq)] = 2.90 x 10^-8

hydrofluoric acid Ka[HF (aq)] = 6.30 x 10^-4

formic acid Ka[HCOOH (aq)] = 1.80 x 10^-4

Which of the following is a correct statement?

Hypochlorous acid is the weakest acid listed

Acetic acid is a weaker acid than hypochlorous acid

Chloroacetic acid is the strongest acid on the list

Formic acid is a stronger acid than acetic acid

Formic acid is a weaker acid than hydrofluoric acid

Which of the following statements strong and weak acids is correct?

Weak acids completely dissociate in solution

Strong acids completely dissociate in solution

A 0.05 M solution of an acid is a weak acid

Strong acids only partially dissociate in solution

Weak acids completely dissociate in solution

Which of the following is not an Arrhenius acid, but is a Lewis acid??

HSO4-

AlCl3

CH3COOH

HCl

H2O

Which of the following compounds is not amphoteric?

H2O

H2CO3

HSO4-

HCO3-

H2PO4-

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Elin HesselLv2

11 Nov 2019

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Related questions

1. The K_a for hydrofluoric acid, HF is 7.20 x 10^-4. The K_a for acetic acid, CH₃COOH, is 1.80 x 10^-5. The K_a for benzoic acid, C₆H₅COOH. is 6.30 x 10^-5. What is the formula for the strongest acid?

2. The K_a for phenol (a weak acid), C₆H₅OH. is 1.00 x 10^-10. The K_a for benzoic acid, C₆H₅COOH, is 6.30 x 10^-5. The K_a for formic acid, HCOOH, is 1.80 x 10^-4. What is the formula for the strongest conjugate base?

3. The K_a for acetylsalicylic acid (aspirin), HC₉H₇O₄, is 3.00 x 10^-4. The K_a for formic acid, HCOOH, is 1.80 x 10^-4. The K_a for acetic acid, CH₃COOH, is 1.80 x 10^-5. What is the formula for the weakest acid?

sangriaporcupine175

For conjugate acid-base pairs, how are Ka and Kb related?

Consider the reaction of acetic acid in water:

CH₃CO₂H (aq) + H₂O (l) ⇌ CH₃CO₂⁻ (aq) + H₃O⁺ (aq) where Ka = 1.8 × 10⁻⁵

Which two bases are competing for the proton?
Which is the stronger base?
In light of your answer to part b. why do we classify the acetate ion (CH₃CO₂⁻) as a weak base? Use an appropriate reaction to justify your answer.
In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH₃ is a weak acid.

To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1× 10⁶, calculate Kb for the conjugate base of this strong acid.

Why do conjugate bases of strong acids have no basic properties in the water?

List the conjugate bases of the six common strong acids.

To tie it all together, some instructors have students think of Li⁺, K⁺, Rb⁺, Cs⁺, Ca²⁺, Sr²⁺, and Ba²⁺ as the conjugate acids of the strong bases LiOH, KOH, RbOH, CsOH, Ca(OH)₂, Sr(OH)₂, and Ba(OH)₂. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. ( Hint: Weak gives you weak and strong gives you worthless.)