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11 Nov 2019
8-8 The molarity of the NaOH solution is found by completing the reaction table and associated calculations as directed. Na C:04 (an) HzC:Os (aq) 2NaOH (aq) 2HO (aq) EXAMPLE PRACTICE EXAMPLE PRACTICE 4) 0.0026240 4) 5) 0.01630 5)_ 6) 0.1610 6) Moles, mol 1)0.0013120) Volume, L 2)0.02500) Molarity, M 3) 0.052481 3) Enter the volume of oxalic acid solution titrated, in liters, and the molarity of this solution in the appropriate locations in the table above. EXAMPLE: 0.02500 L of oxalic acid solution; 0.052481 M oxalic acid PRACTICE: Use the above data to determine the number of moles of oxalic acid that were titrated. Show your work below and enter your result in the appropriate location in the table above. Express this result to at least one more digit than allowed by applying the rules of significant figures. EXAMPLE: 0.0013120mol (Note: the highlighted digit is not significant but carried along as directed. Doing this minimizes rounding errors) PRACTICE Determine the moles of NaOH required to titrate this many moles of oxalic acid. Show your work below and enter your result in the appropriate location in the table above. Express this result to the same decimal place as the preceding result. EXAMPLE: 0.0026240mol PRACTICE Enter the average volume of NaOH solution used in the titration, in liters, in the appropriate location in the table. EXAMPLE: 0.01630 L PRACTICE: Determine the molarity of the NaOH solution. Show your work below and enter your result in the appropriate location in the table above. Round this result to the correct number of significant figures allowed by the calculation. EXAMPLE: 0.1610 M (Note: four significant figures are allowed.) PRACTICE
8-8 The molarity of the NaOH solution is found by completing the reaction table and associated calculations as directed. Na C:04 (an) HzC:Os (aq) 2NaOH (aq) 2HO (aq) EXAMPLE PRACTICE EXAMPLE PRACTICE 4) 0.0026240 4) 5) 0.01630 5)_ 6) 0.1610 6) Moles, mol 1)0.0013120) Volume, L 2)0.02500) Molarity, M 3) 0.052481 3) Enter the volume of oxalic acid solution titrated, in liters, and the molarity of this solution in the appropriate locations in the table above. EXAMPLE: 0.02500 L of oxalic acid solution; 0.052481 M oxalic acid PRACTICE: Use the above data to determine the number of moles of oxalic acid that were titrated. Show your work below and enter your result in the appropriate location in the table above. Express this result to at least one more digit than allowed by applying the rules of significant figures. EXAMPLE: 0.0013120mol (Note: the highlighted digit is not significant but carried along as directed. Doing this minimizes rounding errors) PRACTICE Determine the moles of NaOH required to titrate this many moles of oxalic acid. Show your work below and enter your result in the appropriate location in the table above. Express this result to the same decimal place as the preceding result. EXAMPLE: 0.0026240mol PRACTICE Enter the average volume of NaOH solution used in the titration, in liters, in the appropriate location in the table. EXAMPLE: 0.01630 L PRACTICE: Determine the molarity of the NaOH solution. Show your work below and enter your result in the appropriate location in the table above. Round this result to the correct number of significant figures allowed by the calculation. EXAMPLE: 0.1610 M (Note: four significant figures are allowed.) PRACTICE
Jarrod RobelLv2
8 Jan 2019