When standardizing two liters of a potassium permanganate solution, approximately 0.0100 M, with a primary standard solution of sodium oxalate, it was planned to use between 30.00 and 45.00 ml of the titrated reagent. In which mass range (in grams) the primary standard should be weighed?

A 185.0 mL sample of 1.200 M Pb(NO₃)₂ is mixed with 52.50 mL of 1.500 M NaCl, and the PbCl₂ precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr₂ precipitate is also collected and dried. What is the mass (in grams) of the PbBr₂ precipitate, assuming the yield in each precipitation step is 100%?

A 21.25 g of a mixture of the solid salts, sodium chloride and lead II nitrate, is added to distilled water and stirred. The precipitate that is formed is filtered and dried. Its mass was determined to be 11.06 g. Analysis of the remaining solution shoed that the following ions were present: Pb2+, Na+ and NO3". Determine the percent (by mass) of lead (II) nitrate in the mixture. Assume 100 % yield.

Sonomic acid is a monoprotic acid developed in the chemistry department of Sacramento state University. The storeroom staff successfully obtained a sample of sonomic acid and made a solution. They made the solution by adding 302.4 g of sonomic acid and diluting it to a volume of 10.00 L with water. Unfortunately, the stockroom attendant, Steven , does not know the molar mass of sonomic acid so he could not calculate the molarity of the solution he prepared. It would be great if you could help him.

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 antacid found in Tums™ has the active ingredient calcium carbonate, which undergoes a reaction when mixed with hydrochloric acid to produce water, calcium chloride and carbon dioxide. A tablet of this antacid had a mass of 1.774g and was dissolved completely in an excess of 30.0mL of 0.794M HCl. The resulting solution was then titrated with 0.995M NaOH. The initial buret reading was 11.05mL and the final buret reading was 28.52mL. The listed mass of active ingredient on the bottle is 325mg. a. What is the calculated mass of active ingredient in this tablet? b. What is the percent error from the listed mass? c. What percent of the tablet is inert (non-active) ingredients? explain in detail

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)?

5.00 mL of acetic acid required 37.28 mL of 0.0999 M NaOH to be neutralized in a titration. Calculate the molarity of vinegar.

A solution of NaOH(aq) was standardized by titration using oxalic acid (H₂C₂O4) as the primary standard. The following data was collected: Mass of H₂C₂O4(s) used = 1.02 g Volume of NaOH(aq) used = 40.6 ml. Calculate the concentration of the NaOH(aq)

2.0 g of a mixture containing unknown amounts of sodium carbonate, sodium bicarbonate and a neutral component were titrated according to the experimental procedure. Answer the questions that follow related to the individual steps of the titration. Calculate the number of moles of sodium bicarbonate titrated in the second step of the titration if 13.7 ml of 1.0 M HCl were used to titrate the resulting mixture from the first step of the titration with methyl orange as the indicator. Enter your numerical answer below in units of moles with the correct number of significant figures.