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To calculate the molarity of the unknown NaOH solution you will need to follow the example in Figure 6 (provided below for reference but note that it is a different reaction altogether!). Show your work below using the Math Editor. (Be sure to include units on each number and round the answer to the correct number of significant figures at the end) NOTE: You will need to know: the balanced chemical equation, the volume of H2SO4 you put into the Erlenmeyer flask (using the graduated cylinder), the concentration of the H2SO4 solution (found on the carboy in the hood), the amount of the unknown NaOH solution it took to neutralize the solution. Figure 6: Finding an Unknown Molarity from a Known Molarity Example Question: Given the following equation: 3 KOH (aq) + 1 H3PO4(aq) -> 1 K3PO4(aq) + H2O (aq) What is the M of a KOH solution if it took 17.2 mL of a 1.7M solution of H3PO4 to neutralize 10.0mL of the KOH? Molarity Moles per 1 Liter 2.0M = 2.0 mol / 1 Liter Answer: 17.2 mL H3PO4 | 1 L H3PO4 / 1000mL | 1.7 mol H3PO4 / 1 L H3PO4 | 3 mol KOH / 1 mol H3PO4 = 0.088 mol KOH in 10.0mL = 8.8M KOH

          To calculate the molarity of the unknown NaOH solution you will need to follow the example in Figure 6 (provided below for reference but note that it is a different reaction altogether!). Show your work below using the Math Editor. (Be sure to include units on each number and round the answer to the correct number of significant figures at the end) NOTE: You will need to know: the balanced chemical equation, the volume of H2SO4 you put into the Erlenmeyer flask (using the graduated cylinder), the concentration of the H2SO4 solution (found on the carboy in the hood), the amount of the unknown NaOH solution it took to neutralize the solution. Figure 6: Finding an Unknown Molarity from a Known Molarity Example Question: Given the following equation: 3 KOH (aq) + 1 H3PO4(aq) -> 1 K3PO4(aq) + H2O (aq) What is the M of a KOH solution if it took 17.2 mL of a 1.7M solution of H3PO4 to neutralize 10.0mL of the KOH? Molarity Moles per 1 Liter 2.0M = 2.0 mol / 1 Liter Answer: 17.2 mL H3PO4 | 1 L H3PO4 / 1000mL | 1.7 mol H3PO4 / 1 L H3PO4 | 3 mol KOH / 1 mol H3PO4 = 0.088 mol KOH in 10.0mL = 8.8M KOH

To calculate the molarity of the unknown NaOH solution you will need to follow the example in Figure 6 (provided below for reference but note that it is a different reaction altogether!). Show your work below using the Math Editor. (Be sure to include units on each number and round the answer to the correct number of significant figures at the end) NOTE: You will need to know: the balanced chemical equation, the volume of H2SO4 you put into the Erlenmeyer flask (using the graduated cylinder), the concentration of the H2SO4 solution (found on the carboy in the hood), the amount of the unknown NaOH solution it took to neutralize the solution. Figure 6: Finding an Unknown Molarity from a Known Molarity Example Question: Given the following equation: 3 KOH (aq) + 1 H3PO4(aq) -> 1 K3PO4(aq) + H2O (aq) What is the M of a KOH solution if it took 17.2 mL of a 1.7M solution of H3PO4 to neutralize 10.0mL of the KOH? Molarity Moles per 1 Liter 2.0M = 2.0 mol / 1 Liter Answer: 17.2 mL H3PO4 | 1 L H3PO4 / 1000mL | 1.7 mol H3PO4 / 1 L H3PO4 | 3 mol KOH / 1 mol H3PO4 = 0.088 mol KOH in 10.0mL = 8.8M KOH

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