Sodium hydroxide

1. Limewater Test: As we exhaled CO2 in the limewater solution, the CO2 reacted with Ca(OH)2 and changed the clear colorless limewater solution to precipitated white solution. The precipitation was caused due to the calcium in the limewater solution. It took us 5 attempts to turn the clear colorless limewater solution to a milky white solution. 2. Phenolphthalein Indicator Test: As phenolphthalein indicator was added to NaOH and H2O solution, it made the solution turn clear pink. The phenolphthalein

by performing a series of titrations between sodium hydroxide and potassium phthalate in order to standardized the sodium hydroxide to be used to identify the concentration of the hydrochloric acid.During each of the titrations, sodium hydroxide (NaOH) was used to titrate potassium hydrogen phthalate (KHP); during each of the trials, sodium hydroxide was gradually added to the KHP from the burette to the beaker. After each addition of sodium hydroxide, the pH was recorded in order to form the titration

a greater number of drops of sodium hydroxide than substances with an insignificant amount of substrate. On the second day, if the starting reactants affect the yield of the product then obtaining solid copper from a salt will result in a greater yield. If aluminum foil is the limiting reactant of the experiment, then the percent yield will increase as the amount of foil increases. Materials/Methods: Project A, Day 1 In Part 1, 50 milliliters of 5% sodium hydroxide solution was obtained and observed

The titration of vinegar has a solution composed of acetic acid (HC2H3O2), water and other substances. When adding sodium hydroxide (basic solution) to acetic acid (acid) it causes a neutralization reaction. The phenolphthalein is colorless in acid, and it will change color when adding the sodium hydroxide. In this experiment, there were four trials to reach the amount of sodium hydroxide needed to reach the end point. When you reach the end point of the experiment, the solution should be pink and if

hairline. This step is for a base relaxer. There are non-base relaxers as well. It depends on the type of relaxer one decided to use. The protective base can be applied to other areas of the hair. This ultimately depends on the manufacturer. In the sodium hydroxide relaxer, the formula can have built in ingredients to protect the scalp of the client. This is calls a base formula. A no base formula does not have this petroleum cream which in turn has a milder reaction. The process is the same just without

In this experiment we will be titrating the titrant sodium hydroxide against the analyte, which is the substance being analyzed, hydrochloric acid. Titration is the process of analyzing base and acid added together. The objective is to calculate the unknown concentration of hydrochloric acid with the standardized solution of solid sodium hydroxide. The standardized solution is the known concentration but since sodium hydroxide naturally reacts with air, we must first determine the true concentration

Chem II Background Info The neutralization of hydrochloric acid with sodium hydroxide solution is represented by the following equation. HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) Using a calorimeter, you will determine the enthalpy change for this reaction. Question What is the relationship between the number of moles of reactants used and the change in enthalpy of neutralization reaction? Hypothesis As the number of moles of reactants used increases, the change in enthalpy of a neutralization

The zinc and sodium hydroxide solution, when heated formed sodium zincate* (Na2ZnO2) which when introduced to the copper penny the zincate ions (ZnO2-2) in the solution to bind to the copper of the penny, after a minute it gets reduced to metallic zinc that coats the penny. This process involved a chemical change as the sodium zincate formed, and a physical change as it coated the penny, a new substance was not formed

nitric acid, sulfuric, and acetic acids) on top of the bench. Place one drop of each acid on a blue and red litmus paper and then place a drop of each liquid on (pH) paper. Record the observations. For the Base, place one drop of each liquid (sodium hydroxide, ammonium

the mixing and 2 mL of the 0.25 M sodium hydroxide was added expeditiously. The exact amount of sodium hydroxide solution added to the flask was recorded and the solution turned pink. The pink color produced when sodium hydroxide was added, eventually faded due to the production of hydrochloric acid. The time that had elapsed from the zero time of the t-butyl chloride addition to the color fade was recorded as well as the temperature. 2 mL of sodium hydroxide was added in increments and the times