The pH of a solution is 9. What is the concentration of OH−OH^-OH− ions?
a) 1×10−91 \times 10^{-9}1×10−9 M
b) 1×10−51 \times 10^{-5}1×10−5 M
c) 1×10−71 \times 10^{-7}1×10−7 M
d) 1×10−141 \times 10^{-14}1×10−14 M
Answer: b
Which of the following substances is an acid anhydride?
a) Na₂O
b) SO2SO_2SO2
c) MgOMgOMgO
d) CaOCaOCaO
Answer: b
The ion product of water, KwK_wKw, increases with:
a) Increasing temperature
b) Decreasing temperature
c) Increasing pressure
d) Decreasing pressure
Answer: a
Which of the following salts is formed from a weak acid and a strong base?
a) NaCl
b) NH4ClNH_4ClNH4Cl
c) CH3COONaCH_3COONaCH3COONa
d) KNO3KNO_3KNO3
Answer: c
What is the effect of adding a common ion to a solution of a weak acid?
a) Increases ionization
b) Decreases ionization
c) Increases pH
d) No effect on ionization
Answer: b
The pH of a solution with a hydroxide ion concentration of 1×10−41 \times 10^{-4}1×10−4 M is:
a) 4
b) 10
c) 7
d) 14
Answer: b
Which of the following salts will form a basic solution when dissolved in water?
a) NaCl
b) NH4ClNH_4ClNH4Cl
c) CH3COONaCH_3COONaCH3COONa
d) KNO3KNO_3KNO3
Answer: c
The dissociation constant of a weak acid KaK_aKa is related to the pH of the solution by:
a) Henderson-Hasselbalch equation
b) van ‘t Hoff equation
c) Arrhenius equation
d) None of the above
Answer: a
Which of the following acids is the weakest?
a) Hydrochloric acid
b) Sulfuric acid
c) Acetic acid
d) Nitric acid
Answer: c
The pH of a buffer solution depends on:
a) The concentration of acid and base
b) The volume of the solution
c) The temperature of the solution
d) All of the above
Answer: d
In the reaction NH3+H2O⇌NH4++OH−NH_3 + H_2O \rightleftharpoons NH_4^+ + OH^-NH3+H2O⇌NH4++OH−, NH3NH_3NH3 acts as:
a) An acid
b) A base
c) A salt
d) A solvent
Answer: b
The pKapK_apKa value of acetic acid is 4.76. What is the pKbpK_bpKb of its conjugate base?
a) 9.24
b) 14
c) 10
d) 7
Answer: a