The ammonia solution that is purchased for a stockroom has a molarity of . (a) Determine the volume of that must be diluted to 250. mL to prepare . (b) An experiment requires . The stockroom manager estimates that 8.10 L of the base is needed. What volume of will be required for the preparation

200. ml of 3.00 m nacl solution is diluted to a final volume of 500. ml. what is the molarity of the final solution?

If i can still dissolve more sugar into the solution at a certain temperature what would i call that solution

Achemistry student needs to standardize a fresh solution of sodium hydroxide. he carefully weighs out of oxalic acid , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in of distilled water. the student then titrates the oxalic acid solution with his sodium hydroxide solution. when the titration reaches the equivalence point, the student finds he has used of sodium hydroxide solution.calculate the molarity of the student's sodium hydroxide solution. be sure your answer has the correct number of significant digits.