7. (16 point) (a) The pH of a 1.00 L buffer solution containing 0.15 M HOCl...

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Chemistry

7. (16 point) (a) The pH of a 1.00 L buffer solution containing0.15 M HOCl and 0.15 M NaOCl is 7.52.
HOCl (aq) + H20 (l) ---> OCl- (aq) + H3O+ (aq)
(a) Calculate the pH change when 0.40 g of NaOH is added to 1.00 Lof a buffer solution containing 0.15 M HOCl and 0.15 M NaOCl.Neglect any volume change. Ka of HOCl is 3.0 x 10-8.

(b) Calculate the pH change when 0.200 L of 0.100 M HCl is added to1.00 L of a buffer solution containing 0.15 M HOCl and 0.15 MNaOCl. Assume the total volume of the solution is 1.20 L. Ka ofHOCl is 3.0 x 10-8.

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Q7 a Ka of HOCl 30 x 108 pKa logKa pKa log30 x 108 pKa 752 mass of NaOH added 040 g moles of NaOH added mass of NaOH added molar mass of NaOH moles of NaOH added 040 g 40 gmol moles of NaOH added 0010 mol concentration of NaOH in buffer moles of NaOH added volume of buffer concentration of NaOH in buffer 0010 mol 100 L concentration of NaOH in buffer 0010 M NaOH is a strong See Answer

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