A student from the Industrial Chemistry course wishes to prepare a 3mol/L solution of phosphoric acid (H3PO4). For this procedure, the student used a 0.2N NaOH solution. Knowing that for 25 mL of the sample (acid), they used 30 mL of the alkaline solution (NaOH), determine the actual concentration of the acid and how much of this same solution is needed to prepare 500 mL of a 0.1N solution. (Data: Molar Mass of H3PO4 = 98g/mol; density = 1.685g/mL; T (%) = 85).
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A student from the Industrial Chemistry course wishes to prepare a 3mol/L solution of phosphoric acid (H3PO4). For this procedure, the student used a 0.2N NaOH solution. Knowing that for 25 mL of the sample (acid), they used 30 mL of the alkaline solution (NaOH), determine the actual concentration of the acid and how much of this same solution is needed to prepare 500 mL of a 0.1N solution. (Data: Molar Mass of H3PO4 = 98g/mol; density = 1.685g/mL; T (%) = 85).
Please, help me
The student used a 0.2N (0.2 normal) NaOH solution, which means there are 0.2 moles of NaOH in 1 liter of the solution.
The student used 30 mL of this NaOH solution, which is equivalent to 0.03 liters. Therefore, the number of moles of NaOH used is:
0.2 N * 0.03 L = 0.006 moles of NaOH
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