Introduction Strong acids and strong acids both dissociate completely in water forming ions. However, strong acids donate a proton to form H3O+ along with a conjugate base and strong bases accept a proton to form OH- along with a conjugate acid. The chemical behavior of acids and bases are opposite. When they are together, their ions cancel out and form a neutral solution. In this experiment, HCl and NaOH will react to form NaOH and H2O with these two steps: The overall reaction is: Both Na+ and Cl- ions combine to form NaCl.
Eventually using the NaOH and the acid’s consumed moles, the equivalent mass will be determined. Procedure: Part 2: Obtain 45mL of NaOH, and then weigh 0.3-0.4g of the unknown acid (KH2PO4). Dissolve the acid into 20.00mL water. Record the buret readings, and slowly titrate the NaOH into
10 ml NaOH was again added and mixed for 15 seconds to make lump free slurry. The mixture was stirred and allowed to stand for 3 minutes. An additional 10 ml of caustic soda was poured in the beaker and stirred for 10 minutes to mix thoroughly. In between the stirring, remaining 30 ml of 17.5% caustic soda was added at 2.5, 5 and 7.5 minutes in installments of 10 ml each. This mixture was allowed to remain in the beaker for 30 minutes further, making the total treatment time of 45 minutes from the beginning.
Data Table: Experiment ml NaClO ml Solution B Temperature of Precipitate (degrees) 1 5 45 27.0 2 15 35 35.0 3 25 25 44.0 4 30 20 49.0 5 35 15 52.0 6 40 10 46.5 7 50 0 24.0 8 45 5 22.0 9 43 7 21.0 Graph: I eliminated the last two data points because it was making my graph weird. 20 ml of NaClO is equal to 30 ml of solution B, 40 ml of NaClO is equal to 10 ml of solution B, etc. Mole Ratio: Intersection is at (35, 15) → 35/15= 2.333… __2__NaClO + __1__ Solution B → Products
Lab Final Mrs. Hsi/Horne Redmond High School January 6th 2015 Maddi Bibby and Lisa Brinton Abstract The purpose of this lab is to observe the reaction between sodium bicarbonate and calcium chloride take place, determine which of the reactants is the limiting reactant and which is the excess reactant, determine the theoretical mass of the precipitate that should form, and compare the actual mass with the theoretical mass of the precipitate and calculate the percent yield. In the lab, it was determined that Na CO had an average final mass of 7.41g after the three trials were performed. It was found that CaCl had an average final mass of 5.53g from the three trials performed. (Data Table 1) When Na CO was mixed with water, it
3- Put the large tube in an ice bath and start to add alcohol by an increasing rate . 4- Put the tube in hot water (70º C) for 5 minutes . 5- Add 8 drops of water with constant shaking then leave the reaction to cool to room temprature. 6- Add 6 mL of ( 3 mL saturated NaCl +3 mL distilled water) i.e : half-saturated sodium chloride solution to the test tube with vigorous shaking and then wait until two layers form (upper layer is ester while lower layer which consists of a water solution of sulfuric and acetic acids ,should be discarded
The line of best fit gives the respiration rate of day-old seedlings as the concentration of NaCl they are exposed to increases. As NaCl Concentration increases the rate of cellular respiration decreases by .108 ppm CO2/g per second. This overall decrease throughout the data further supports our hypothesis. Discusion: The data collected in the experiment does support our hypothesis. By examining the data as a whole a trend of decreased cellular respiration in seedlings soaked in solutions with increased NaCl concentrations.
The NaH2PO4 and Na2HPO4 powdered were weighted by using weighing machine, followed the mass that has been calculated in step (3). The NaH2PO4 and Na2HPO4 powdered were mix in a 500 mL beaker. 500 mL of distilled water were measured by using a 500 mL measuring cylinder, then is poured inside the 500 mL beaker containing both the powdered. The mixture were stirred by using a glass rod until the mixture is fully dissolved. The solution were tested by using calibrated pH meter to get the pH value of the solution.