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.
Questions: How would you prepare 10 mL of a 0.25M HCl solution if 1M HCl was available? How much 1M HCl is needed? How much distilled water is used? Dilute 2.5ml of 1M solution with 7.5ml of dihydrogen monoxide. From the graph of Molarity vs. Density, created in Data Table 10, what was the relationship between the molarity of the sugar solution and the density of the sugar solution?
Calculate the exact normality of Na2S2O3 knowing that in this chemical reaction 1 gram-equivalent of K2Cr2O7 react with 1 gram-equivalent of Na2S2O3 (1 mole K2Cr2O7 react with 6 moles Na2S2O3). Determination of peroxide value. Weigh 3.00 g oil (with precision of 0.001 g) into a 250 ml Erlenmeyer flask. Add 10 ml chloroform and swirl to dissolve oil. Add 15 ml acetic acid,
(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.
Introduction: Thyme contains a surprising amount of iron compounds. This experiment enables us to determine the amount of iron(II) present in dried thyme by means of a redox reaction. Method: 1. Weigh accurately about 1g of dried thyme and put into a 250cm3 beaker. Record the mass of thyme used.
: Se, calculated molar mass 78.93 g] 4) A 0.3528 gram mixture of H2SO4 (molar mass 98 grams) and H3PO4 (molar mass 98 grams) was mixed with a little water and titrated with 9.70 mL of 1.000 M NaOH: 3NaOH(aq) + H3PO4(aq) →3H2O(l) + Na3PO4(aq) 2NaOH(aq) + H2SO4(aq) →2H2O(l) + Na2SO4(aq) What was the percent by mass H2SO4 in the original mixture? [Ans. : 30.6] 5) A 0.9030 gram sample of Z(OH)2 and 20.00 mL of 2.000 M HCl were put into a 100.0 mL volumetric flask and mixed with enough extra water to make 100.0 mL of solution. A 10.00 mL aliquot of this solution was taken and titrated with 17.64 mL of 0.05121 M NaOH. What is the identity of the element Z?
The buffer checks out because pH=pKa ± 1.0. Results: Phosphate buffer: The initial pH for the phosphate buffer is 6.83 and it takes 18 drops to equal 1.0 mL of 1.0 M HCl. The volume of HCl required to break the buffer was 1mL, and the known concentration of the HCl 1.0 M The number of moles of HCl consumed by the buffer was 0.02. [pic] Acetate buffer: The target pH of NaCH3CO2 was 5.25 and the actual measured pH for the acetate buffer was 11.21. The number of drops to equal 1Ml of NaOH is 17 drops.
Title: 1pt Stoichiometry Of A Precipitation Reaction 2. Procedure: 2pt (Write the procedure in your own words after you have read the lab manual) Put on goggles the weigh 1.0 of CaCl*2H2O and put it in 100ml beaker. Add 25 mil of water and stir. I will then use stoichmetry to figure out how much Na2CO3 I will need for a full reaction. I will weigh this and put it in a separate cup.
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.
NaCl 1 Na+ and 1 Cl- are formed). Calculate the osmolarity of that solution. What is the molar concentration of ALL particles? e.g. 0.15 M NaCl solution = 0.15 moles of Na+ atoms + 0.15 moles of Cl- atoms = 0.30 Osmoles In other words, the solution is said to have an osmolarity of 0.30 Osm (or 300 mOsm) Assume the osmolarity of the ICF of body cells to be 0.300 Osm (300 mOsm) 2nd, determine if the solute is a PENETRATING particle or is NON-PENETRATING.