Acids and Bases – Flashcards

Write a balanced equation for the dissociation of the Bronsted-Lowry acid HSO4- in water.

What is the concentration of the hydronium ions in a neutral solution?

What is the hydronium ion concentration of a 0.1 M hypochlorous acid solution with Ka= 3.5 x 10^-8? The equation for the dissociation of hypochlorous acid is: HOCl(aq) + H2O(l) <--> H3O+(aq) + OCl-(aq)

A 25.0 ml sample of .105 M HCl was titrated to the equivalence point with 31.5 mL of NaOH. What is the concentration of the NaOH?

What are the conjugate acid-base pairs in the following chemical reaction: NH3(aq) + H2O(l) <--> NH4+(aq) + OH-(aq)

The pH of .255 M HCN is 4.95. What is the value of Ka for hydrocyanic acid?

What is the hydronium ion concentration of acid rain sample that has a pH of 3.15?

In order for a solution to be acidic: A) [H3O+] = [OH-] B) [H3O+] < [OH-] C) pH = pOH D) [H3O+] > [OH-] E) None of the above

What is the concentration of hydronium ions in a solution given that the concentration of hydroxide ions is 2.31 x 10^-4 M?

What is the strongest monophonic acid of the following set if all the acids are at 0.100 M concentration? A) hydrofluoric acid with Ka = 3.5 x 10^-4 B) hypochlorous acid with Ka = 3.5 x 10^-8 C) acetic acid with Ka = 1.8 x 10^-5 D) benzoin acid with Ka = 6.5 x 10^-5

Which Brønsted-Lowry acid has the strongest conjugate base? A) HF B) HClO4 C) HI D) HBr

A 35.0 mL sample of .225 M HBr was titrated with 42.3 mL of KOH. What is the concentration of the KOH?

Which solution below has the highest concentration of hydronium ions? A) pH = 7.00 B) pH = 9.82 C) pH = 7.93 D) pH = 3.21 E) pH = 12.6

Indicate all the Brønsted-Lowry acids in the following chemical reaction: HCl(aq) + H2O(aq) <--> H3O+(aq) + Cl-(aq)

The Bronsted-Lowry definition of a base is:

An aqueous solution contains 0.10 M NaOH. The solution is A) very dilute B) Neutral C) basic D) acidic E) highly colored

Which of the following is not an acid-base conjugate pair? A) H2S and OH- B) H2CO3 and HCO3- C) NH4+ and NH3 D) H2O and OH- E) none of the above

Which of the following Brønsted-Lowry acids does not behave as a strong acid when it is dissolved in water? A) HClO4 B) HCl C) HNO2 D) HBr

The magnitude of Ka indicates that:

Nitric acid is a strong acid. This means that A) aqueous solutions of HNO3 contain equal concentrations of H+(aq) and OH-(aq) B) HNO3 produces a gaseous product when it is neutralized C) HNO3 does not dissociate at all when it is dissolved in water D) HNO3 cannot be neutralized by a weak base E) HNO3 dissociates completely to H+(aq) and NO3-(aq) when it dissolves in water

In the following reaction: HCO3-(aq) + H2O(aq) -> H2CO3(aq) + OH-(aq) A) H2O is an acid and HCO3- is its conjugate base B) HCO3- is an acid and OH- is its conjugate base C) H2O is an acid and H2CO3 is its conjugate base D) HCO3- is an acid and H2CO3 is its conjugate base E) H2O is an acid and OH- is its conjugate base

What solution below has the highest concentration of hydroxide ions? A) pH = 12.49 B) pH = 10.12 C) pH = 7.93 D) pH = 7.00 E) pH = 3.21

The Arrhenius definition of an acid is:

The Bronsted-Lowry definition of an acid is:

What is the equilibrium constant expression (Ka) for the acid dissociation of hydrocyanic acid HCN? The equation of interest: HCN(aq) + H2O(l) <--> H3O+(aq) + CN-(aq)

What is the hydroxide ion concentration of a lye solution that has a pH of 11.20?

In the following reaction: NH4+(aq) + H2O(aq) -> NH3(aq) + H3O+(aq) A) H2O is a base and NH3 is its conjugate acid B) Nah4+ is an acid and H2O is its conjugate base C) NH4+ is a base and H2O is its conjugate acid D) NH4+ is an acid and H3O+ is its conjugate base E) H2O is a base and H3O+ is its conjugate acid

The pH of 0.150 M CH3CO2H, acetic acid, is 2.78. What is the value of Ka for acetic acid?

In which of the following aqueous solutions does the weak acid exhibit the lowest percentage ionization? A) .01 M HNO2 (Ka = 4.5 x 10^-4) B) .01 M HClO (Ka = 3.0 x 10^-8) C) .01 M HC2H3O2 (Ka = 1.8 x 10^-5) D) .01 M HF (Ka = 6.8 x 10^-4) E) These will all exhibit the same percentage ionization

Calculate the pH for an aqueous solution of pyridine that contains 2.15 x 10^-4 M hydroxide ion.

What is the pH of a .020 Ba(OH)2 solution?

In a solution that has a pH = 7.0, A) [H3O+] > [OH-] B) [H3O+] + [OH-] = Kw C) [H3O+] < [OH-] D) [H3O+] = [OH-] E) none of the above

What is the second stepwise equilibrium constant expression for phosphoric acid H3PO4?

What is the value of the ion product constant for water (Kw) at 25*C?

At 25*C, the pH of a vintage solution is 2.60. What are the values [H3O+] and [OH-] in the solution?

The pH of a solution is 5.00. Which of the following is TRUE about the solution? A) it's [H3O+] is 1.0 x 10^5 M B) it's [H3O+] is 1.0 x 10^-5 M C) it's [H3O+] is 1.0 x 10^-9 D) it's more acidic than a solution whose pH is 4.00 E) none of the aboce

What is the pOH of a solution that has a OH- concentration equal to 1.3 x 10^-10 M?

What statement is most consistent for an acid with a pH = 3? A) one hundred times as strong as an acid with a pH = 5 B) one one-hundredth as strong as an acid with a pH of 5 C) twice as strong as an acid with a pH of 5 D) half a strong as an acid with a pH = 5

What is the hydronium ion concentration of a 0.100 M acetic acid solution with a Ka = 1.8 x 10^-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq) + H2O(l) <--> H3O+(aq) + CH3CO2-(aq)

What is the [H+] in a solution that has pH of 3.35?

What is the pH of a solution prepared by diluting 25.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 x 10^-3 M hydronium ion.

Which of the following acids is diprotic? A) H2SO4 B) HNO3 C) HI D) HClO4 E) none of the above

What is the concentration of the hydroxide ion given that the concentration of the hydronium ion is 1.5 x 10^-5 M?

Using the data in the table, which of the conjugate bases below is the weakest base? HOAc: Ka = 1.8 x 10^-5 HC7H5O2: Ka = 6.3 x 10^-5 HNO2: Ka = 4.5 x 10^-4 HF: Ka = 6.8 x 10^-4 CHOICES: A) OAc- B) F- C) NO2- D) C7H5O2