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Question

1. You mix 100.0 mL of a 0.100 M NaOH solution and 150.0 mL of a 0.100 M HCl solution. Determine the concentration of H⁺ in the final mixture after the reaction is complete.

A. 0.0500 M

B. 0.0600 M

C. 0.0200 M

D. 0.150 M

E. 0.100 M

 

4. Which of the following is the strongest conjugate base?

A. All the same

B. C₂H₃O₂^- or CH₃COO-

C. Cl-

D. HSO4-

E. NO3-

 

9. What is the limiting reactant when 15.0 mL of 0.150 M lead(II) nitrate solution is reacted with 20.0 mL of 0.200 M sodium iodide solution?

A. Pb(NO3)2

B. Nal

C. PbNO3

D. There is no limiting reactant

E. Pbl2

 

10. Choose the case that is not a Bronsted conjugate acid-base pair.

A. C₂O₄²-, HC2O4-

B. HC₂H₃O₂, H₂C₂H₃O₂⁺

^{C. NH₃, NH4+}

^{D. O2-, OH+}

^{E. SO₃2-, SO₄2-}

 

12. To make 44.6 mL of a 0.405 M solution of NaCl, what mass of NaCl is required?

A. 58.4 G

B. 23.7 G

C. 2.66 G

D. 1.08 G 

E. None of these

 

13. You react 250.0 mL of a 0.10 M barium nitrate solution with 200.0 mL of a 0.10 M potassium phosphate solution. What ions are left in solution after the reaction is complete?

A. potassium ion, nitrate ion, barium ion

B. barium ion, nitrate ion, phosphate ion

C. potassium ion, nitrate ion, phosphate ion

D. potassium ion, barium ion, phosphate ion

E. potassium ion, nitrate ion

 

18. A solution has [H⁺] = 4.2 ´ 10^-3 M. The [OH^-] in this solution is

A. 1.0 ´ 10^-14 M

B. 4.2 ´ 10^-3 M

C. 4.2 ´ 10^-11 M

D. 2.4 ´ 10^-12 M

E. None of these

 

19. What mass of solute is contained in 25.4 mL of a 1.56 M potassium bromide solution?

A. 119 G

B. 4.72 G

C. 3.02 G

D. 186 G

E. None of these