A. Calculate the pH of a 2.0 x 10-7 M HNO3 solution. B. a) Calculate the pH of a

Question

A. Calculate the pH of a 2.0 x 10-7 M HNO3 solution.

B. a) Calculate the pH of a 0.0100 M solution of butylamine by making the assumption that the formal concentration is equal to the equilibrium molarity of the butylamine in solution. b) Calculate the percent error incurred by “cutting corners” with the assumption in part a) c) Solve part a) by using the technique of successive iterations. d) Solve part a) by using the quadratic.

C. a) Find the pH of a 1.00-L aqueous solution prepared with 10.00 g of imidazole (FM 68.08 g/mol) and 17.50 g of imidazole chloride (FM 104.54 g/mol) HINT: for imidazole information see Table 9-2, p 205 in 9th ed (Table 8-2, p. 179 in 8th ed). b) If 25.00 mL of 0.500 M NaOH solution are added to the buffer solution in part a), what will be the pH?

Explanation / Answer

A) HNO3 is a strong acid HNO3(aq) H+ (aq) + NO3 - (aq).

Therefore the concentration of H+ in the final solution is 2.0 x 10-7 M

pH = -log[H+ ] = - log(2.0x10-7) = 6.699

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