1) What is the pH of a hydrocyanic acid/sodium cyanide buffer in which the concentration of the weak acid component is 0.129 M and the concentration

1) What is the pH of a hydrocyanic acid/sodium cyanide buffer in which the concentration of the weak acid component is 0.129 M and the concentration of the conjugate base is 0.091 M? 

2) The pH of a hydrocyanic acid/sodium cyanide buffer in which the concentration of the weak acid component is 0.140 M and the concentration of the conjugate base is 0.070 M is 8.91. Suppose 0.113 g of solid NaOH are added to 100 mL of this buffer solution. What is the pH after the addition? 

3) What must be the minimum concentration of hypoiodous acid in 1.00L buffer solution of a pH=10.56 hypoiodous acid/sodium hypoiodite buffer if the pH changes by 0.2 units when 0.026 moles HCl are added? 

4) The pH of a 25.0 mL sample of a buffer changed by one unit when 4.17 mL of 0.33 M NaOH was added to it. What is the base buffer capacity of this buffer? 

Express your answer in moles base per L of buffer, according to the buffer capacity definition in your lab manual. 

5) A student was required to prepare 250.0 mL of a hypochlorous acid/sodium hypochlorite buffer in which the concentration of the weak acid component was 0.076 M and the concentration of the conjugate base was 0.055 M. The student was supplied with 0.393 M hypochlorous acid and 1.0M NaOH to perform this task. What volume (in L) of the acid would the student need to prepare this buffer solution?  

Hint: assume that all of the conjugate base comes directly from the reaction of NaOH with the weak acid (in other words, there is negligible dissociation of the weak acid).

Provide the solutions for each please. Thank you.

These values on table can be used: