Sodium hydroxide

a technique used to find the concertation of an unknown acid, called the analyte, through the use of a base with a known concentration, called the titrant. In this experiment the analytes used were sulfuric and acetic acid and the titrant was sodium hydroxide. In order to find the concertation of these acids, the acid and base were mixed until they reached the equivalence point, or the point when the amount of titrant is equal to the amount of the analyte needed to fulfill the mole to mole ratio necessary

was unknown A, an originally clear solution of hydrochloric acid that turned hot pink after having added approximately 14.50 and 14.40 milliliters of sodium hydroxide, for trials 1 and 2 respectively. The molarity calculated for this acid was found to be 0.86 M, but this value is not accurate because the indicator showed that too much sodium hydroxide was added to the solution, eventually passing the endpoint, resulting in a vibrant pink color instead of the intended light pink hue. The true concentration

purpose of this experiment is to examine the stoichiometric relationship between reagents and the identity of the products by using three acid/base neutralization reactions of a triprotic acid, phosphoric acid, and varying molar equivalents of sodium hydroxide. The data will be used to determine the formula weight of the products and identify the remaining salt for all three reactions. Introduction In this experiment, we learned about stoichiometry, empirical formula, molecular formula, polyprotic

added 50 mL of .1 M NaCl. I added sodium acetate to the rest of the beakers: 1 gram to 3 and 8, 5 grams to 4 and 9, and 10 grams to 5 and 10. I then filled the beakers that contained the solid sodium acetate with 50 ml of .10 M acetic acid. Specifics can be found on page 84 of the lab manual. Though the lab manual instructed to use a pipet, we did not have an accurate 1 mL pipet or a graduated pipet, so we instead prepared two graduated burets with 1 M Sodium Hydroxide and 1 M hydrochloric acid. Using

were performed order to experimentally determine the rate constant(k), for the rate of the reaction of the crystal violet solution and sodium hydroxide. To start, a Beers Law calibration experiment was conduction. Also, two kinetic experiments were ran using both 5ml and 10ml of sedum hydroxide in order to determine the reaction order(k^1), of the sodium hydroxide. The Beers Law calibration experiment used many concentrations of crystal violet solutions. Each of these solutions were test and analyzed

tap water has been in contact with various other compounds. From this test, it can be concluded that water is naturally acidic and is only displays base like qualities after it has interacted with other compounds and molecules. B5 was filled with sodium bicarbonate and turned the pH strip a light, almost lime green, the pH was recorded at eight,

solution. 6. 12.5 cm3 of 0.9992 M sodium hydroxide solution was transferred to a 250 cm3 volumetric flask by burette and de-ionized water was added to the mark. The flask was shaken to ensure homogeneity of the solution. 7. A clean burette was filled with the diluted sodium hydroxide solution (~ 0.05M). The initial burette reading, accurate to the nearest 0.05cm3, was recorded. During trial run, about 2-3 drops of methyl orange was added as an indicator. 8. Sodium hydroxide solution was run from the burette

distilled water. A clean 150mL beaker was used to obtain approximately 100mL of 0.0474 M NaOH solution. The buret was rinsed by sodium hydroxide. The buret was filled with sodium hydroxide by a clean funnel. The funnel was removed, and the stopcock was opened for a short time. The level of the solution was lowered. The leaking was checked, and then the initial volume of sodium hydroxide solution was recorded. The carbonic acid in the soda was previously removed by boiling. Prior to each

included sodium nitrate, 4-sulfanilic acid, sodium hydroxide, triclosan, and a glycine buffer. An antibacterial soap sample made from 0.4382 g of the green Dial soap and was placed into a 50-ml beaker. Approximately 20-ml of 0.01 M sodium hydroxide solution was added. The mixture was placed in a sonic bath for 5 minutes and then transferred to a 50-ml volumetric flask. An additional 10 ml of the sodium hydroxide solution was added and the flask was filled to the line with .01 M sodium hydroxide. This

INTRODUCTION Concentration is the profusion of a component divided by the solvent. Dilute solutions contain relatively little solute in a particular volume of solvent. While concentrated solution has relatively great amount of solute in a particular quantity of solvent. There are many term that can be used to describe concentration and two of them are percent by mass and molarity. Molarity means number of moles of a solute in a litre of solution. molarity(M)=(mole of solute)/(liter of solution) Percent