You need 500 mL of a 0.5 M iron(III) chloride solution. You only have a 3.0 M FeCl3 solution on hand. How much of the higher concentrated stock solution do you need to make the desired solution?                       How much water to you then need to add?

Will the calculated Molarity of NaOH be too high or too low or unaffected if the following happen: When you answer the question, consider how the situation affects the calculation of molarity of NaOH and moles NaOH, which is calculated from the mass of KHP. For each answer, you must supply a clear explanation for your answer. Often times, students will restate the facts rather than explaining why they chose the answer they chose. a) You add the weighed KHP to a flask containing a 60mL of water rather than 50 mL of water. Explain. Your answer must contain a well-thought-out and clearly written explanation. b) The buret is still wet with water on the inside when you add your NaOH solution. Explain c) The KHP is wet when you weigh it. Explain. d) You titrate past the equivalence point by 0.50mL Answer a-d

You have a standard stock 1.65 M solution of NaH₂PO4. For an experiment you require 236 mL of a 0.82 M solution of NaH2PO4. How much of the 1.65 M solution do you need? Write your answer to 3 significant figures in mL.

The normality of an aqueous solution of hydrobromic acid is determined by titration with a 0.151 N sodium hydroxide solution. If 32.8 mL of sodium hydroxide are required to neutralize 16.7 mL of the acid, what is the normality of the hydrobromic acid solution? N