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W10_MT2_Grey_ans.pdf

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Department
Chemistry
Course
CHEM 1040
Professor
Lori Jones
Semester
Winter

Description
Part B. [Total of 10 points] GREY VERSION 1. A buffer was prepared by adding 125.0 mL of 0.255 M LiOH to 250.0 mL of 0.565 M HBrO (a.) Write the net ionic equation for the chemical reaction (including states) & calculate the pHof this buffer solution. Show all your work! Net Ionic EquationHBrO (aq) + OH –(aq) ? BrO (aq) + H O (l) –1 for each mistake; 2 pts total 2 –9 0.565 M 0.255M Ka(HBrO) = 2.0×10 0.2500L 0.1250L pK aHBrO) = 8.70 I 0.141(2) mol 0.0318(8) mol (LR) 0 mol VTotal = 0.1250 L + 0.2500 L C – 0.03188 – 0.03188 +0.03188 = 0.3750 L E 0.109(3) mol 0 0.0318(8) mol (0.2915 M) ( 2 pts for reaction)(0.08501 M) 6 /6 – + – pH = pK +alog (BrO /HBrO) OR K aHBrO) = {[H O3][BrO ]}/[HBrO] pH = 8.70 + log (0.03188/0.1093) 2.0×10 –9 = {[H 3 ] (0.08501)}/( 0.2915) –9 + pH = 8.70 – 0.5351 2.0×10 = 0.2916[H O3] pH = 8.16 [H O ] = 6.858×10 –9 3
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