Calculate the number of moles of NaOH used when 15.45 mL of the 0.0985 M solution was delivered to reach the endpoint of the titration. Remember to report the answer with the correct number of significant figures and accepted abbreviated units. Keep in mind the example format below: 0.1025 mL

Ammonium oxalate dissociates when it dissolves in water.   If the concentration of the oxalate ions is 3.2 mol/L, then what is the concentration of the ammonium oxalate solution? Record only your numerical answer with the correct number of significant digits.  You do not need to include units as the units appear for you beside the answer box already.

A student titrating a sample of a powdered aspirin tablet to find out how much acetylsalicylic acid is in the sample finds that it requires 30.4 mL of a 0.0902M sodium hydroxide solution to neutralize the acid in the sample.  How many milligrams of acetylsalicylic acid did the sample contain?  Use the correct number of significant figures.  Do not include units or your answer will be counted wrong.

A sample with a mass of 1.340 g was dissolved in water, releasing chlorine ions. The aqueous solution was treated with access AgNO3(aq), the AgCl precipitate collected and weighted. Its mass was 2.709 g. What percentage by mass was the original sample? Make sure to use the correct number of significant figures in your answer.

The iodine contained in every one mL of the 0.010 M iodine solution in the buret will react with 1.76 mg of vitamin C. (In other words, every mL of iodine solution needed for the titration indicates the presence of 1.76 mg of vitamin C in the juice sample.) If your titration used 5.86 mL of iodine solution, what mass of vitamin C is in your fruit juice sample (in milligrams, mg)?

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A 25.0 mL sample of solution of unknown acid, HX, is titrated with 2.11 M KOH. If 67 mL of KOH was required to neutralize the sample, find the molarity of the original HX solution. Only enter your numerical answer. Do not enter units.

A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1840 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 13.34 mL of the standard solution. What is the concentration of the original sulfuric acid solution? concentration: M

An analytical chemist weighs out 0.206 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1200 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 19.9 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. x10 mol