A buffer solution contains acetic acid (HC2H3O2) at a concentration of 0.225 M and sodium acetate
(NaC2H3O2) at a concentration of 0.164 M. The value of Ka for acetic acid is 1.75 × 10−5. What is the pH
of this buffer solution? - 4.62
Consider two beakers, one containing 1.0 M HCl and the other containing 1.0 M CH3COOH. Which
solution would have the lowest pH? - 1.0 M HCl because its solution contains a higher hydronium ion
concentration than 1.0 M CH3COOH
Which of the following correctly describes what is meant by the term neutralization? - the reaction
between an acid and a base to form a salt and water
Consider the following generalized buffer solution equilibrium:
BH+(aq) + H2O(l) H3O+(aq) + B(aq)
When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the
four species shown would experience an increase in concentration? (Hint: Use LeChatelier's principle.) -
B
Which statement concerning the relative strength of acids is FALSE? - Strong acids produce strong
conjugate bases; weak acids produce weak conjugate bases.
What is the pH of a 0.035 M HCl solution? - 1.46
A buffer solution is prepared by placing twice the concentration of propanoic acid (C2H5COOH, Ka=1.34
×10−5) as the concentration of its conjugate base sodium propanoate into a flask. The pH of the
resulting buffer solution is best described as which of the following? - less than 4.87
The species that remains after an acid donates a proton is called its conjugate base. What is the
conjugate base of the hydronium ion, H3O+? - H2O
Which one of the following is NOT a characteristic property of a base? - increases [H+] in water
, What is the conjugate acid of NH2−? - NH3
Butyric acid is a weak acid. Which reaction equation properly represents the dissociation of butyric acid
in water? - H3CH2CH2COOH(aq) + H2O(l)
= CH3CH2CH2COO-(aq) + H3O+(aq)
Morphine is used medicinally as a pain reliever. If an aqueous solution of morphine has [H3O+] = 1.1 ×
10−10 M, what is the pH of this solution? - 9.96
What is always a characteristic of a solution that contains a buffer? - The solution resists large changes
in pH when small amounts of acids or bases are added.
The reaction of an acid with a base produces a salt and another product. What is the identity of the
other product - water
A buffer solution contains carbonic acid (H2CO3) and sodium bicarbonate (NaHCO3), each at a
concentration of 0.100 M. The relevant equilibrium is shown below. What is the pH of this buffer
solution?
Which statement correctly describes conjugate acids and bases according to the Brønsted-Lowry
theory? - A conjugate base is the species formed when an acid donates a proton; a conjugate acid is the
species formed when a base accepts a proton.
If the hydronium ion concentration of an aqueous solution at 25°C is 5 × 10−6 M, what is the hydroxide
ion concentration? - : 2 × 10^−9 M
Titration of 15.0 mL of an NaOH solution required 7.4 mL of a 0.25 M HNO3 solution. What is the
molarity of the NaOH solution? - 0.12 M
What is the hydronium ion concentration of a solution with a pH of 6.0? - 1 × 10^−6 M
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