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.
Introduction In this lab, we performed three titrations to determine the mass of ASA in a caplet through the process of diluting the caplet with a solution of NaHO and isopropyl alcohol. The mixed solutions gave us a double displacement reaction. Double displacement: AB+CD = AD+CB Example: AgNO3 + NaCl = AgCl +NaNO3 This is a double displacement reaction. In the titration of HC9H7O4 = NaC9H7O4 + H2O A titration is a process in which a solution is added to another solution, such that it reacts under conditions in which the added volume may be accurately measured. Three titrations were performed to find the caplets mass.
Ocean County College Department of Chemistry [Observations of Chemical Changes] Submitted by Andrew Grimm Date Submitted: 5/31/14 Date Performed: 5/31/14 Lab Section: Chem-181DL2 Course Instructor: Amal Bassa Purpose The main goal in this experiment is to observe the properties of simple chemical reactions, and relating their chemical properties to household products. Procedure To begin this experiment I placed two drops of NaHCO3 into well A1 of the 96-well plate, and then added two drops of HCl into well A1. Next I placed two drops of HCl into well B2, and added two drops of BTB, and observed the color. Then I placed two drops of NH3 into well C1 and added one drop of BTB, and observed the color. Next I added two drops of HCl into well D1, and then added two drops of blue dye, and recorded what I saw.
Objective To determine of heats from three exothermic reactions and investigate the Hess Law Summary Based on this experiment, we have study three related exothermic reactions involving sodium hydroxide. The first reaction (Part A), solid sodium hydroxide will dissociate into water. The heat produce by this reaction (∆H1) and this called as the heat of solution of solid NaOH. From the experiment we have managed to determined that ∆H1 = -41.84 KJ/mol In the second reaction (Part B), an aqueous solution of NaOH is allowed to react with an aqueous solution of HCl. This is a neutralization reaction between a strong acid and strong base.
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.
Laboratory Report: Experiment 1 Standardization of hydrochloric acid by sodium carbonate solution Name: Cheung Chun Hin, Harry Class: 6L (12) Date: 11-9-2009 Objective: To determine the concentration of hydrochloric acid using sodium carbonate solution as a primary standard in volumetric analysis (acid-base titration) Principle of method: The concentration of the hydrochloric acid can be determined by the titration reaction between hydrochloric acid and sodium carbonate solution. Na2CO3 (aq) + 2HCl (aq) H2O (l) + CO2 (g) + 2NaCl (aq) From the above equation, We measure the volume of hydrochloric acid used in the titration (the difference of reading on the burette) and use it in calculating the concentration of hydrochloric acid. So the molarity of the hydrochloric acid Procedures: 1. The mass of anhydrous sodium carbonate required was weighed to prepare 250.0 cm3 of 0.05M sodium carbonate solution. 2.
Once the solution of sodium thiosulfate had been standardized the molarity of the solution was known and sodium thiosulfate could be used to titrate tap water and an iodine solution to determine the amount of chlorine in the tap water and iodine in the iodine solution. Procedure/ Observations: The first step of the experiment was to standardize the sodium thiosulfate solution. This was done by cleaning a 50 mL buret and rinsing it three times with sodium thiosulfate solution to ensure the surface of the buret was consistent with the sodium thiosulfate throughout. The buret was then filled with the sodium thiosulfate solution. The buret was monitored to ensure that the solution extended to the tip of the buret and that no air bubbles were present because both would cause an inaccurate titration.
Materials and Methods To first create the three distinct solutions, 50mL of phosphate buffer with a pH of 6.84 was poured into a 150mL beaker with 20 drops of 0.04% Bromothymol blue indicator. 5mL of the solution was then added to three separate 50mL beakers. 1mL of HCl was added to one of the three beakers and labeled ‘Yellow’, 1mL of NaOH was added to another and labeled ‘Blue’, and 1mL of distilled water was added to the last beaker and called ‘Green’. The spectrometer was prepared and left to warm up before calibrating it. Taking the three solutions prepared earlier, each was transferred to three separate cuvette while filling the fourth cuvette was filled with distilled water.
CHEMISTRY HL Investigation 1.2 Standardizing a solution of hydrochloric acid using a standard solution of Sodium Carbonate Candidate name: Amjad Al-Jafari 11 IBDP 1/2/2013 Preparing a standard solution of Sodium Carbonate (A) • Data Collection and Processing: 1. Data Collection: -Mass of Sodium Carbone which is the solute in this solution: 1.26 ± 0.01 grams. -Volume of distilled water which is the solvent in this solution : 250 ± 0.3 cm3 = 0.250 dm3 -Molar Mass of Sodium Carbonate: 2 Na + 1 C + 3 O = 105.99 Observations: Before beginning the experiment we observed that: • Sodium Carbonate is solid powder that has a white color, • Distilled Water is colorless. During the experiment we observed that: • As we started to add the solution of Sodium Carbonate to water its particles started to dissolve in the solvent as we are stirring until all particles are dissolved in the solvent (water). After the experiment we observed that: • However a white solid powder of Sodium Carbonate has been added to water no color change occurred, it stayed colorless, still all particles of Sodium Carbonate has dissolved in water.
Stoichiometry of Reactions in Solution Lab 18 September 2013 Introduction: In the following lab, quantitative titration reactions will be completed and the mole ratios will be calculated. Using four different chemicals, two acids, hydrochloric acid (HCl) and sulfuric acid (H2SO4), and two bases, sodium hydroxide (NaOH) and barium hydroxide (Ba(OH)2.) will be combined to see the mole ratio of the chemicals. The following four equations will be the key equations to the lab. HCl + NaOH → H2O + NaCl H2SO4 + 2 NaOH → 2 H2O + Na2SO4 H2SO4 + Ba(OH)2 → 2 H2O + BaSO4 2 HCl + Ba(OH)2 → 2 H2O + BaCl2 Using a buret and the indicator phenolphthalein, it will be visible when the solution reaches the point when the ratio is correct for the reaction to start.