25 ml of diluted unknown acid solution to 100ml beaker by using 25 volumetric pipet. 10ml of deionized water and 3 drops of phenlpthalin indicator the beaker labeled as 3. Potentiometric titration acid solutions 125 ml of NaOH was obtaining in a beaker and 50 ml of NaOH transfer to buret the tip and the meniscus is at below 0 ml. one magnetic stirring bar placed in a beaker contain one of the known solution on a stir. The pH recorded by using pH electrode before adding NaOH.
The following steps were performed to create the ionic reaction. 2 drops of Sodium Phosphate, Na3PO4?12H2O solution were placed into the five vertical wells under column number 1. Next, 2 drops of Sodium Iodide, Nal solution were placed into the five vertical wells under 2. Next, 2 drops of Sodium Sulfate, Na2SO4 solution into five vertical wells under 3. Next, 2 drops of Sodium Chloride, NaCl solution were placed into the five vertical wells under 4.
Determination of Enthalpy Change Objective: to find the enthalpy change (∆H) in the decomposition of Sodium Hydrogen Carbonate. Materials: Calorimeter, 2.00 mol HCl, NaHCO3, Na2CO3, Lab Quest, Temperature Probe, Graduated cylinder, Balance scale. Procedure | Observations | 1. Obtain 50 mL of HCl in a beaker. | N/A | 2.
Obtain between 0.1 to 0.2g of zinc metal. Making Predictions 2. Determine the amount of 6.0M HCl that will be needed to react completely with the zinc. 3. Determine the volume of hydrogen gas that will be generated by the reaction.
Sodium Hydroxide + Hydrochloric Acid Sodium Chloride + Water NaOH(aq) + HClaq → NaCl(aq) + H2O(l) Variables Independent The independent variable of the experiment was the amount of sodium hydroxide that we added to the acid. To keep the variable controlled we would measure 1 ml of the sodium hydroxide and pouring that to the hydrochloric acid. Dependent The dependent variables of the experiment were the temperature and the pH number of the mixture. To control the pH and temperature use the electronic probe and data logger. Controlled The controlled variables of the experiment were: A.
The normality of the unknown base is calculated after the solution has reached the end point. The amount of substance being delivered is calculated in units of equivalents per litre using the formula: VaNa = VbNb Experimental In order to titrate the acid with the unknown base, a solution of the acid was prepared. 5.1722 (±10%)g of potassium hydrogen phthalate acid is obtained using a weighing boat and transferred into a volumetric flask containing 250mL of boiled distilled water. Volumetric flask was shaken several times in order to assist the powder to dissolve. Once dissolved, 24.9734 (± 0.0045)mL of acid was pipetted into an Erlenmeyer flask along with 25mL of cool (recently boiled) distilled water.
About 125 mL of standard HCl with a molarity of 0.3125 and was poured into a buret. An unknown sample of soda ash was obtained, and for each trial, a little over 1 g of the soda ash was quantitatively transferred into a wide mouth Erlenmeyer flask. About 75 mL of DI water and 5 drops of methyl purple indicator was then added to the soda ash powder. The solution was titrated once until the solution turned light purple, and then the flask was put on the hotplate for about 3 minutes of gentle boiling. After, the solution was titrated once more in order to reach the endpoint that was indicated by a bullfrog green color.
The last one was nickel (II) nitrate I placed 2 drops into seven of the E well plates of the 96 well plate. In the next step going vertically, I started with sodium phosphate solution and placed 2 drops into 5 vertical rows. The next one was sodium iodide solution I placed 2 drops into 5 vertical rows. The next one was sodium sulfate solution I placed 2 drops into 5 vertical rows. The next one was sodium bicarbonate solution I placed 2 drops into 5 vertical rows.
Using a burette, run 5.0 cm3 of 0.100 mol dm-3 peroxodisulphate solution into a 100 cm3 beaker. Add 45 cm3 of distilled water, from a burette, stir gently to mix. 2. Using burettes, measure out 15 cm3 of each of the 0.500 mol dm-3 potassium iodide, 3 cm3 of 0.010 mol dm-3 sodium thiosulphate solutions and 2.0 cm3 of starch solution into the second 100 cm3 beaker. 3.
The temperature was raised to 70 degrees Celsius and 4.419 g of salicylic acid was measured out on a balance and transferred into a 125. mL Erlenmeyer flask. Next, 8.00 mL of acetic anhydride was measured out and poured into the flask containing salicylic acid, ten drops of phosphoric acid was placed inside. The flask was then immersed into the hot water bath for twenty minutes. A vacuum filtration system was set up and the contents of the flask was transferred onto the filter paper. The mass of the filter paper and watch glass was 42.7131 grams.