[H+] [OH-] pH acid/base/neutral 2.6 x 10^-3 ? ? ? ? 6.2 x 10^-6 ? ? ? ? 12 ? 2.Calculate the [H+] and the pH of the following solutions: A)0.025 M
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[H+] [OH-] pH acid/base/neutral

2.6 x 10^-3 ? ? ?

? 6.2 x 10^-6 ? ?

? ? 12 ?

2.Calculate the [H+] and the pH of the following solutions:


A)0.025 M HCl





B)0.048 M H2SO4





C) 0.0065 M NaOH




D)0.0032 M Ba(OH)2


3.Which solute combinations can make a buffer? Assume all are aqueous solutions.

  1. HCl and NaCl
  2. HNO2 and NaNO2
  3. NH4NO3 and HNO3
  4. NH4NO3 and NH3


4.Which solute combinations can make a buffer? Assume all are aqueous solutions.

  1. H3PO4 and Na3PO4
  2. NaHCO3 and Na2CO3
  3. NaNO3 and Ca(NO3)2
  4. HN3 and NH3


5.For each combination in Exercise 3 that is a buffer, write the chemical equations for the reactions of the buffer components when a strong acid and a strong base is added.



6.For each combination in Exercise 4 that is a buffer, write the chemical equations for the reaction of the buffer components when a strong acid and a strong base is added.


7.Two solutions are made containing the same concentrations of solutes. One solution is composed of phosphoric acid and sodium phosphate, while the other is composed of hydrocyanic acid and sodium cyanide. Which solution should have the larger capacity as a buffer?

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