Question

Calculate the pH of each of the following strong acid solutions.

(a) 0.00757 M HBr pH =

(b) 0.264 g of HCl in 16.0 L of solution pH =

(c) 60.0 mL of 6.70 M HBr diluted to 4.50 L pH =

(d) a mixture formed by adding 80.0 mL of 0.00838 M HBr to 80.0 mL of 0.00258 M HCl pH =

Answer 1

Nollow a) HAS = HT = 0.00757 pHartog () e Tog (0.00757) - 2.121 b) Ose, Min = Me, was & moles of Hele man -0.264 - 7.237 810) molarman, 36.5 mobrity-molex - 7.23 3x10 I volume any) 16 i He=Hae 4.5218104 pha-log (4.5218104) = 3.345 c) une, mil, = M.No anch & 6.70 X 60.0 = M2 X 4.50 x 10) Inne & 4.5218104 12x (4.50 x 10 In one fo r M₂ - 0.0893 109 (0.0893) - 1.049 d) mmoles of HBO- moloridyx volume (In me) & 0.00838 x 80 – 0.6704 minoles of H = 0.6704 mmoles of Hel= 0.00258x80 = 0.2064 mmoles of the = 0.2064 Total Hi= 0.6204 +0. 2064 = 0.8766 0.8766 - 5.4BXlos total volume (Inn) (80 180) PM = log (he) = log (5-4B X 10) = 2.2612 HI molority =

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