Carefully immerse the electrons in the solution. Turn the function knob to “pH”. Turn the standardize knob until the meter indicate the exact pH of the buffer solution. Record the pH at which the meter is standardized. Titrating HCl solution with NaOH solution Obtain 25mL of 0.100M HCL solution
Experiment For this experiment, The weight of a graduated cylinder (10mL) was taken by the scale. 4 mL of water was poured into the first graduated cylinder and then weighed. The volume of the water was 10.06g/mL and was written down. Next, the mass of was calculated and written down. In order to figure out what the mass was, the weight of the cylinder (42.16g) subtracted by the weight of the cylinder by itself (37.85g).
If 0.100 mol of hydrogen iodide is placed in a 1.0 L container and allowed to reach equilibrium, find the concentrations of all reactants and products at equilibrium. 2 HI (g) === H2 (g) + I2 (g) Ke = 1.84(10-2 [H2]=[I2]= 1.07(10-2 mol/L, [HI]=7.86(10-2 mol/L 6. A 1.00 L reaction vessel initially contains 9.28(10-3 moles of H2S. At equilibrium, the concentration of H2S of 7.06(10-3 mol/L. Calculate the value of Ke for this system.
For the first beaker, we add 1 mL of 0.1 M potassium phosphate. The purpose is to test the excess of lead, and it is positive due to the presence of white precipitation. We add 1 mL of 0.1 M silver nitrate into the second beaker to test for excess iodide. It is positive due to the presence of yellow precipitation. Next, take out the filter paper and add 50 mL of water.
Investigating the Chemical Composition of Alka Selzter Problem: How much sodium bicarbonate is in a tablet of Alka Seltzer? Purpose: To discover the amount of sodium bicarbonate, in grams, in a one tablet of Alka Seltzer. Materials: one Alka Seltzer tablet 50 mL of vinegar post-it note Triple beam balance beaker Procedure: 1) Put the post-it on the triple beam balance and zero the balance. 2) Measure the masses of the alka-seltzer tablet, and the beaker + vinegar. Record them.
Record several points of pH and NaOH added (especially near equivalence point) to be use later to prepare a titration curve. Observations and Results Part I: Solution | pH | 0.1 M HCl | .70 | 0.1 M NaOH | 13.30 | Part II: Volume of 0.1 M NaOH at equivalence point: 35mL pH at equivalence point: 11.45 Molarity of the Unknown Acid A (HCl): 2.0 x 10-4 Discussion In this lab, we found out that water self ionizes itself into hydrogen ion and hydroxide ion naturally to a very small extent. An indicator, in an acid base reaction, is a substance whose color changes over a particular pH range. Phenolphthalein is an example of an indicator which changes from colorless to pink as pH goes from 8 to 10. We plotted the pH against the amount of base added producing a
Steps 1-10 were repeated using Copper (II) Sulfate and sodium hydroxide solution Part B: 12. 5 ml of hydrochloric acid was poured into the larger test tube. 13. One scoop of sodium bicarbonate was put into the beaker 14. The test tube was placed in the beaker and the total mass of the reactants, test tube and beaker were determined using the balance.
Abstract The interaction at equilibrium between acids and bases during a titration can be used to determine several characteristics of the acid or the base. In this experiment 0.05 M of KHP titrate with the strong base NaOH. From the plot of pH versus the volume of sodium hydroxide added was found that acid ionization constant Ka for KHP at half point was equal to 8.3176x10-6, also the dissociation constant Kb for conjugate base of weak acid was equal to 1x10-9. This value was established by observing the pH versus volume of NaOH graph. The equivalence point of titration occurred at a volume of 31 mL 0.081M NaOH (aq).
Each beaker was filled with either 1mL of 1.0 M HCl, 1mL of 1.0 M NaOH, or 1mL of water with a pipette, in order to create three solutions that had varying pH levels. Three cuvettes were filled with one of the solutions and a fourth cuvette was filled with distilled water to act as a blank. The cuvette was labeled “Yellow”, “Blue”, “Green”, or “Blank” according to its color, which was determined by either the mixture of HCl, NaOH, or distilled water. The second part of the experiment consisted of measuring the transmittance of each solution at numerous wavelengths using the spectrophotometer. The original setting of the Spec 20 was set to 360nm and the transmittance of the three colored solutions was taken.