Acid-base titration & analytical chemistry
A 0.213-g sample of uranyl(VI)nitrate, UO2(NO3)2, is dissolved in 20.0 mL of 1.0 M H2SO4 and shaken with Zn. The zinc reduces the uranyl ion, UO2 (with a charge of 2+), to a uranium ion, Un+ (where n+ is the charge of the uranium ion). To determine the value of n, this solution is titrated with KMnO4. Permanganate is reduced to ...continues
A 0.7834 g sample of primary standard KHP was titrated with 38.45 ml of NaOH solution to a phenolphthalein end-point? What is the molarity of the NaOH solution?
A student decided to measure the amount of salt that would dissolve in 50 ml of water at different temperatures. The student found that the solubility at 10 degrees centigrade (10° C), was .56 grams of salt. At 40° C, 2.35 grams dissolved and the solubility at 70° C was 3.85 grams of salt. Create a "Best fit" graph for the e ...continues
Titrations: Finding Concentration
A 35.00 mL solution containing an unknown concentration of pyruvic acid required 25.13 mL of 0.2011 M NaOH to reach the end point. What is the concentration of the pyruvic acid solution ?
Titrations: Finding Mass Percent of Arsenic in a Pesticide
The arsenic in a 1.0211-g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized and exactly 40.00 mL of 0.05922M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and in the washings from the precipitate was titrated with 14.76 mL o ...continues
A 0.0560-g quantity of acetic aid is dissolved in enough water to make 50.0 mL of solution.
A 0.0560-g quantity of acetic aid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H+, CH3COO-, and CH3COOH at equilibrium).
A solution containing 100g of an unknown substance and 900g of water. The solution has a Freezing Point of -3.33*C. What is the molar mass of the substance?
An aqueous solution is made by dissolving 33.2g of the compound in 250mL of water. The solution has an Osmotic Pressure of 1.2 atm at 250*C. What is the molar mass of the compound?
Emperical and Molecular Formula
Determine the empirical and molecular formulas given 75.69% C 8.80% H 15.51% O molar mass about 206 g/mol
Estimation of Mass Required in a Reaction
With the reaction, CaCO3+2Hcl->CaCl2+H2O+CO2. Using percent by mass what is the weight of HCl needed to react with calium carbonate? The weight of calcium carbonate that reacted with hydrochloric acid is 2.66.
