a) Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF. The Ka for HF is 7.2×10-4. pH =  b)  Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0014 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. Ka = 4.3×10-7 Сoncentration =  M c) You have 75.0 mL of 0.10 M HA. After adding 30.0 mL of 0.10 M NaOH , the pH is 5.50. What is the Ka  value of HA ?  =  d) Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added. 40.0 mL pH =  50.0 mL pH =

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Chapter1: Chemical Foundations
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a) Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF.
The Ka for HF is 7.2×10-4.

pH = 

b) 

Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0014 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40.

Ka = 4.3×10-7

Сoncentration =  M

c) You have 75.0 mL of 0.10 M HA. After adding 30.0 mL of 0.10 M NaOH , the pH is 5.50. What is the Ka  value of HA ?

 = 

d) Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.

  1. 40.0 mL

    pH = 

  2. 50.0 mL

    pH = 

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