Standardization of NaOH solution Accurately weigh out a sample of approximately 0.3-0.4 g of primary standard potassium hydrogen phthalate, KHPh, which has been previously dried at 120°C. Do not use more than 0.4 g. To obtain an accurate mass, weigh the sample on weighing paper, slide it into a clean (but not necessarily dry) 250 mL Erlenmeyer flask and reweigh the paper to account for any KHPh that may remain on it. Dissolve the KHPh sample in about 50 mL of CO2-free water and add 2-3 drops of 0.1% phenolphthalein indicator. Begin adding the approximately 0.1 M sodium hydroxide solution from the buret while continuously swirling the flask contents. Do not open the stopcock completely.
This solution was diluted with diluents to gae a concentration of 0.1 mg/ml solution each of Amoxicillin trihydrate. The HPLC method was applied to the solutions and the results obtained were shown in table 4.6.11. System suitability solution: 25.0 µg/mL each of of USP Amoxicillin RS in Diluent. Precision
Positive results should be red-purple residue. The principles involved in this test were oxidation of purine by concentrated HNO3; condensation reaction of alloxan to form alloxanthin; and neutralization which forms the red purple murexide or the potassium salt of purpurate. In the sample, the red-purple residue did not appear which means that there is the absence of purines in the DNA
From the bromination of 0.05g aniline, 0.156g of the product was collected. The percent yield was calculated to be 88.1%. Some amount of the product was lost when transferring the product from the Buchner funnel to the balance to measure its mass. To ensure the formation of the desired product, melting point of the product was measured to be 119.8-121.90c, which is in the range of the normal melting point of 2,4,6-tribromoanilne, 120-1220c. Thus, the product was indeed
6 H2O) in 100 ml distilled water. (vi) 0.2(N) Sodium Hydroxide solution: Dissolve 8.0 gm sodium hydroxide in 1 l distilled water. (vii) Acetic acid: Dilute 1 part of glacial acid with 4 parts of water. (viii) Stock cyanide solution: Dissolve 2.51 gm potassium cyanide (A.R. Grade) in 1 l water, standardize this solution with 0.0192(N) silver nitrate solution.
Linoleic acid peroxidation was initiated by the addition of 4 mM FeSO4.7H2O, incubated for 60 min at 37oC and terminated by the addition of 2 mL of ice cold trichloroacetic acid (10% v/v). An amount of 1 mL of thiobarbituric acid (1% w/v in 50 mM NaOH) was added to 1 mL of the reaction mixture, followed by heating at 95oC for 60 min. The reaction sample was read at 532 nm.7 The percentage of linoleic acid peroxidation inhibition activity was calculated using the following equation: % Inhibition = [(AB - AA)/AB] x 100, where AB, absorption of blank sample, AA, absorption of test sample. 2.5.4. Metal chelating activity Briefly, 2 mM FeCl2 was added to different concentrations of test sample and reaction was initiated by the addition of 5 mM ferrozine.
As we know acid reacts with bubbles when combined with sodium bicarbonate. 2. Write the chemical equation for the reaction in well A6. B BoldI ItalicsU Underline Bulleted list Numbered list Superscript Subscript3 Words NaOh + AgNO3>>>>NaNO3 + AgOH 3. One of the reactions you observed resulted in this product: NaCl + H2O + CO2 (g)?
The theoretical yield for Zinc Sulfide is 0.49 grams but the actual yield is 0.38 grams. So if 0.38 is divided by 0.49 and multiplied by 100 then the percent yield for Zinc Sulfide would be 77.6%. When it comes to Sodium Chloride, the theoretical yield is 0.58 grams and the actual yield is 0.45 grams. So when 0.45 grams is divided by 0.58 grams and multiplied by 100, the percent yield would be 77.5% of Sodium chloride. The actual yield is directly taken from the mass of the products in the experiment while the theoretical yield is determined by using stoichiometric calculations.
Results With Respect to Potassium Bromate(V) The table below shows my results when varying the concentration of potassium bromate(V): ￼ ￼ ￼ Concentration of Potassium Bromate(V) (mol/dm-3) Time Take For the Mixture to Turn Colourless (seconds) ￼ ￼ ￼￼￼￼￼￼ Trial 1 Trial 2 Trial 3 Trial 3 Trial 5 Average Reaction Rate (seconds-I) ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.01 31.9 ±0.01 32.2±0.01 31.7±0.01 31.8±0.01 32.0±0.01 31.92±0.05 0.0313 ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.008 45.6±0.01 45.1±0.01 45±0.01.3 45.4±0.01 45.2±0.01 45.32±0.05 0.0221 ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.006 62.8±0.01 63.4±0.01 ±0.0162.7 62.9±0.01 6±0.013.2 63.00±0.05 0.0159 ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.005 88.8±0.01 88.3±0.01 89.0±0.01 88.5±0.01 88.7±0.01 88.66±0.05 0.0113 ￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼￼ ￼￼￼￼￼￼ 0.004
The purpose of this lab was to determine the percent water in magnesium sulfate heptahydrate, or Epsom salt. The experimental percent water is determined to be 42.06% in both trials, making the average also 42.06%. To determine this percent water a heating and cooling procedure was used. First, the vials were cleaned of impurities using the lab oven and were not touched after this point. The 2 vials were then weighed and vial 1 weighed 14.7681 grams and the second vial weighed 14.7451 grams.