Calculate the concentration of grams of sodium stearate per milliliter of diluted solution. To do this, multiply the concentration of sodium stearate in the dishwashing liquid by the dilution of the solution (1.50 mL dishwashing liquid per 100 mL solution). Answer = 1.5 *10^-4 g/mL 4. Calculate the number of moles of sodium stearate in a single layer. To do this, first take the number of drops used to achieve the monolayer (1 drop) and convert it to mL using the calibrated number of drops per mL.
Chem 1110 - Stoichiometry 1) A 25.00 mL aliquot of H3PO4 was titrated with 43.12 mL of 0.002548 M Ca(OH)2: 2H3PO4(aq) + 3Ca(OH)2(aq) → Ca3(PO4)2(s) + 6H2O(l) What was the concentration of the H3PO4 solution before titration? Express your answer in moles/L. [Ans. : 0.002930 M] 2) In one experiment, 22.9841 grams of 75.25% pure Pb(NO3)2 (pure Pb(NO3)2 has a molar mass of 331.2 grams) was mixed with 51.2354 grams of 81.21% pure CsI (pure CsI has a molar mass of 259.80992 grams): 2CsI(aq) + Pb(NO3)2(aq) → 2CsNO3(aq) + PbI2(s) After the reaction, 10.4025 grams of PbI2(s) (molar mass 461.0 grams) were collected. What is the percent yield of the reaction?
Find the volume of 2.40 mol of gas whose temperature is 50.0 °C and whose pressure is 202 kPa. 6. How many moles of gas are contained in a 50.0 L cylinder at a pressure of 10100 kPa and a temperature of 35.0 °C? 7. Determine the number of grams of carbon dioxide in a 450.6 mL tank at 1.80 atm and minus 50.5 °C.
(b) Calculate the volume of 0.2M UO3- needed to react with 20.00 cm3 of 0.1M Cr2O72-. 3. 24.40 g of hydrated iron(II) sulphate, FeSO4.xH2O was dissolved and made up to 1.0 dm3 of aqueous solution, acidified with sulphuric acid. 25.00 cm3 of the solution was titrated with 20.00 cm3 of 0.022M potassium manganate(VII) solution for complete oxidation. a) Write the equation for the reaction.
MATERIALS/APPARATUS: Beaker- 50cm3 Volumetric Flask-250cm3 Conical Flask- Burette-50cm3 Pipette-25cm3 Diammonium Iron (ii) Sulphate 0.1M Sulphuric Acid 0.01M Potassium Manganate (vii) Beaker Digital Balance - 3. d.p METHOD: 5g of Diammonium iron (ii) sulphate is weighed and dissolved into 100cm3 of 0.1M Sulphuric Acid. The solution was then poured into a 250cm3 volumetric flask including all the washings. The solution, was then made up to the 250cm3 mark with distilled water. RESULTS: Table 1 The table above shows the titer value when Iron solution was titrated against potassium Manganate (vii). Calculation: The Equation for the reaction is: 5Fe2+ + MnO4- +8H+ → 5Fe3+ + Mn2+ + 4H2O 1.
In each trial, the initial reading, final reading and the volume of HCl used was recorded down as quantitative results. The average volume of hydrochloric acid was found to be 12.03mL. The amount of sodium carbonate in the 10.00ml of solution was found to b 0.05 mol. The amount of hydrogen chloride that was dissolved in the average volume of acid is 0.365g. Through these calculations, the concentration of hydrochloric acid was found to be 8.3 mol•L-1.