Calculate the grams of phosphorus in a 100 mL sample. It requires 21.16 mL of 0.01000...
Calculate the grams of phosphorus in the 100 ml sample: The acid-base titration procedure depends on the ability of a certain stoichiometric amount of sodium hydroxide being capable of transforming the precipitate as follows: X OH- + (NH4 )3[P(Mo12O40)]×12H2O -> 3 NH4+ + HP042- + 12 MoO42- + Y H2O Balance this equation to find numerical values for X and Y. 50.00 mL of 0.1000 M sodium hydroxide is added to the sample, enough to have enough NaOH to react plus...
1. What is the concentration of a citric acid sample if a 25.00 mL aliquot requires 18.4 mL of 0.200 M KOH titrant to reach the endpoint. 2. How much 0.200 M KOH titrant will be required to reach the endpoint of a titration of 10.00 mL of 0.361 M citric acid?
2. A 10.00 mL sample of aqueous H2SO, requires 20.00 mL of 0.201 M NaOH to reach the endpoint. Calculate the molarity of H2SO4
1. A potassium hydroxide titrant is standardized using potassium hydrogen phthalate. What is the concentration of the titrant if 0.6082 g of KHP requires 38.17 mL to reach the phenolphthalein endpoint? 2. What is the concentration of citric acid in an unknown sample if a 10.00 mL aliquot requires 42.78 mL of the above standardized titrant to reach the phenolphthalein endpoint? 3. How many grams of potassium hydrogen phthalate should be used to standardize 0.200 M potassium hydroxide titrant in...
If the first 10.0 mL vinegar sample requires 2945 ml. to reach an endpoint, what volume should be required for the second and third samples, assuming they are 10.0 mL of vinegar? the volume will vary 29.45 ml 39.45 mL 100 mL 19.45 ml
18. A 25.00 ml sample of the 50.00 ml solution was titrated with 0.1359 M potassium thiocyanate and 12.90 mL were required to reach the endpoint. Calculate the gram of silver (MM= 107.87 g/mol) in the sample.
A sample of an unknown containing Fe2+ in the dissolved sample requires 23.15 mL of a 0.0020 M KMnO4 solution to reach the end point of the titration. 1)Calculate the moles of KMnO4 reacted. 2) Based on the moles you calculated , calculate how many grams of Fe2+ are in the unknown solution.
Calculate the weight percent of ascorbic acid in a tablet of Vitamin C from the following data: A 100 mg sample of a crushed Vitamin C tablet was dissolved in 40 mL of H2SO4 and 20 mL of water. Two grams of KI and 35 mL of 0.0107 M KIO3 solution was added, and the mixture titrated to a starch endpoint. The titration required 12 mL of 0.0790 M thiosulfate solution.
A 15.44 mL sample of acetic acid requires 32.10 mL of 0.0500 M Ba(OH)2 to reach the endpoint. a) Calculate the molarity of the unknown acid b) what is the theoretical pH when 15.8 mL of Ba(OH)2 is added? c) What is the theoretical pH at the point when a total of 32.10 mL Ba(OH)2 is added?
The Fe2+ (55.845 g/mol) content of a 2.370 g steel sample dissolved in 50.00 mL was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 39.51 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per grams of steel (g Fe2+1 g steel). Mno, +8H+ + 5Fe2+ = Mn2+ + 5Fe'+ + 4H,0 Number g Fe2+1 g steel