A permanganate solution is prepared by dissolving 20.0123 g KMNO4 in 500 mL of distilled water and boiled for 1 hour to remove any organic material. Following sintered-glass filtration, the solution is quantitatively transferred to a 1.0 L volumetric flask and diluted to volume with distilled water. The permanganate solution was titrated against 0.1023 M oxalic acid prepared in sulfuric acid solution. A 50.00 mL aliquot of oxalic acid solution required 16.68 mL of permanganate solution. A titration blank required 0.04 mL of permanganate. What is the permanganate molarity? 5 H2C204 + 2 MnO4 + 6H* s 10 CO2 + 2 Mn²* + 8 H2O

The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret contains 0.110 M NaOH.0.110 M NaOH. It requires 31.4 mL31.4 mL of the NaOHNaOH solution to reach the end point of the titration. What is the initial concentration of HClHCl?

A chemist needs to determine the concentration of a solution of nitric acid, HNO3. She puts 905 mL of the acid in a flask along with a few drops of indicator. She then slowly adds 0.200 mol L Ba(OH)2 to the flask until the solution turns pink, indicating the equivalence point of the titration. She notes that 225 mL of Ba(OH)2 was needed to reach the equivalence point. Solution map In this titration, the concentration of base is known and can be used to calculate the unknown acid concentration: concentration of base → moles of base → moles of acid → concentration of acid Part A How many moles of Ba(OH)2 are present in 225 mL of 0.200 mol L-1 Ba(OH)2? Express your answer numerically in moles. • View Available Hint(s) Vo AEO ? mol Ba(OH)2 Submit

A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point.   A.) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!)   B.) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar.   C.) Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.

A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 13.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 11.9mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.

Normal calcium levels in the blood should be between 9.0 and 10.5 mg/dL. Calcium levels in the blood can be determined by adding oxalate ion to precipitate calcium oxalate, CaC2O4, followed by dissolving the precipitate in aqueous acid and titrating the resulting oxalic acid (H2C2O4) with KMnO4. 5 H2C2O4 (aq) + 2 MnO4–(aq) + 6 H+(aq) yields 10 CO2 (g) + 2 Mn2+(aq) + 8 H2O(l) What is the concentration of Ca2+ (mg/dL) in a 10.0 mL sample of blood if 10.54 mL of 9.88 x 10–4 M KMnO4 solution is needed for the titration.

A student weights out 1.118g of impure KHP, dissolves the sample in deionized water and titrate it with 0.1001 M NaOH solution. If the titration requires 27.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample?

Ca(OH)2​(aq)+2HCl(aq)CaCl2​(aq)+H2​O(l)An aqueous solution of Ca(OH)2with a concentration of 0.209 M was used to titrate 25.00 mL of aqueous HCl. 15.93 mL of the Ca(OH)2was required to reach the endpoint of the titration.   A. How many moles of base were required to react completely with the acid in this reaction?   _____mol Ca(OH)2      B. How many moles of HCl were present in the original 25.00 mL of acid?______mol HCl

A 25.00-mL sample of a household cleaning solution was diluted to 250.0 mL in a volumetric flask. A 50.00-mL aliquot of this solution required 41.27 mL of 0.1943 M HCI to reach a bromocresol green end point. Calculate the mass/volume percentage of NH3 in the sample. (Assume that all the alkalinity results from the ammonia.)

The total cation content of natural water is often determined by exchanging the cations for hydrogen ions on a strong acid ion-exchange resin. A 25.00 mL sample of a natural water was diluted to 100.00 ML with distilled water, and 2.06 g of a cation - exchange resin was added. After stirring, the mixture was filtered and the solid remaining on the filter paper was washed with three 15.00 mL portions of water. The filtrate and washings required 16.30 mL of 0.0282 M NaOH to give a bromocresol green end point. a) Calculate the number of millimoles of cation present in exactly 1.00 L of sample.  b ) Report the results in terms of milligrams of CaCO3 per liter. Only typed solution.