Titration of a 20.0 mL sample of acid rain required 1.7 mL of 0.0811 M NaOH to reach the end point. If we assume that the acidity of the rain is due to the presence of sulfuric acid, what was the concentration (in mol/l and %) of sulfuric acid in this sample of rain?

Acetic Acid Titration with NaOH. 50.00 ml of an acetic acid solution is titrated with 0.1000 M NaOH. 23.90 mL NaOH is required to reach the endpoint of the titration. What is the molarity of the acetic acid solution? (Do NOT include units)

If the concentration of the NaOH that was added was 1.0 M and the volume of oxalic acid being titrated was 75 ml, then what is the unknown concentration of the oxalic acid in this titration. The volume of NaOH is 29ml.

An analytical chemist weighs out 0.026 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 3.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g x10 mol

An analytical chemist weighs out 0.318 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 82.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol x10 x 3

A 0.491 g sample of sodium propanoate, NaC, H,O, , is added to a 55.0 mL sample of a 0.270 M solution of propanoic acid. Assume that no change in the volume of the solution occurs. How many moles of C,H,0, are present from the addition of sodium propanoate? mol C,H,05 = mol What is the volume of solution in liters? volume solution = What is the concentration of the propanoate ion, C,H,0, (aq), in the solution? [C,H,O,] = M

A chemistry student weighs out 0.0856 g of citric acid (H,CH,0,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0900 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL x10

4. A student did not read the directions to the experiment properly and mixed up where to put the NaOH and the HCl solutions. He put the HCl in the buret and the NaOH in the flask. He then added a drop of the phenolphthalein to the solution in the flask. Does the student need to empty out all of the solutions and start over again or can he go ahead and run the titration? Explain qalb ribidw qid edini olddud ris ogrel s znisimos tund entd nousu 5. How many liters of 3.4 M HI will be required to reach the equivalence point with 2.1 L of 2.0 M KOH? 9no vino to beateni nolusius to alsid sigulum ob of insttoqmi ti al VW S

Table 1: Titration Data Volume of magnesium hydroxide solution in Erlenmeyer flask Concentration of magnesium hydroxide 0.135 mol/L solution in Erlenmeyer flask Initial volume of nitric acid solution in burette Final volume of nitric acid solution in burette 10.Use the data in Table 1 to answer the folowing (a) Write the balanced chemical equatio. (b) Calculate the molar concentration of nitric acid 20.00 mL (c) Calculate the pH of the acid. 1.06 mL 23.08 mL

0.3456 g of a solid acid is dissolved in 50 mL of water in a flask  and a few drops of phenolphthalein are added to the solution.  A buret containing 0.2545 M NaOH is prepared with an initial volume of 10.50 mL.  The acid is accidentally titrated with the base beyond the end point, so 1.52 mL of 0.187 M HCl are added to the flask. The titration with the base is continued to a final volume reading of  40.55 mL.  Calculate the molar mass of the solid acid.