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Exam3BKey

# Exam3BKey - 1 A solution is labeled 0.200 M NaBrO(aq a(25...

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1) A solution is labeled 0.200 M NaBrO(aq). a) (25) What is the concentration of HBrO in this NaBrO solution? BrO 1- + H 2 O ¾ HBrO + OH 1- i 0.200 0 0 mmol -x +x +x mmol e 0.200 - x x x mmol K b = ] [BrO ] [OH [HBrO] - 1 - 1 5.0 x 10 -6 = x) - (0.200 (x) (x) ~ 200 . 0 x 2 1.0 x 10 -6 = x 2 1.0 x 10 -3 = x [HBrO] = 1.0 x 10 -3 M b) (20) What is the pH of this NaBrO solution? pOH = -log(1.0 x 10 -3 ) = 3.00 pH = 14.00 – 3.00 = pH = 11.00 c) (25) 30.0 mL of this NaBrO solution is added to 25.0 mL of 0.400 M HCl. What is the pH of the resulting mixture? start with : 30.0 ml x 0.200 M = 6.00 mmol BrO 1- 25.0 mL x 0.400 M = 10.0 mmol H 3 O 1+ BrO 1- + H 3 O 1+ ¾ HBrO + H 2 O i 6.00 10.0 0 mmol -6.00 -6.00 + 6.00 mmol e 0 4.0 6.00 mmol two acids pH = - log mL 55.0 mmol 4.0 = pH = 1.14 HCN : pK a = 8.70 CN 1- : pK b = 5.30 K b = 10 -5.30 = 5.0 x 10 -6

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2) (25) What is the pH (to nearest 0.01 pH unit) of a solution prepared by mixing 55.0 mL of 0.594 M HCl and 77.0 mL of 0.778 M NaOH? start with : 55.0 mL x 0.594 M = 32.7 mmol H 3 O 1+ 77.0 mL x 0.778 M = 59.9 mmol OH 1- H 3 O 1+ + OH 1- ¾ 2 H 2 O i 32.7 59.9 mmol -32.7 -32.7 mmol e 0 27.2 mmol strong base pOH = - log mL 132.0 mmol 27.2 = 0.69 pH = 14.00 – 0.69 = pH = 13.31
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Exam3BKey - 1 A solution is labeled 0.200 M NaBrO(aq a(25...

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