Laboratory Safety Guidelines Quiz

A type of chemical analysis that relies on accurately measuring the volume of a solution of known concentration needed to react completely with a substance of unknown quantity

The process of determining the exact concentration of a solution. It involves reacting a known volume of the solution with a standard solution of known concentration.

A type of titration where the reaction involves the transfer of protons (H+) between an acid and a base. The endpoint is usually determined using a pH indicator.

Titration where a known volume of a solution of known concentration (titrant) is directly added to a solution of an analyte of unknown concentration until the reaction is complete.

Titration used to determine the concentration of a substance that doesn't react directly with the titrant. It involves adding an excess of the titrant, then titrating the excess with a second standard solution.

A back titration technique where a known volume of a reagent is added to a blank solution, which does not contain the analyte. The reaction is then performed on the analyte solution and the difference between the two volumes is used to determine the concentration of the analyte.

A type of titration that involves the formation of a complex between a metal ion and a suitable reagent. The endpoint is determined by the appearance or disappearance of a color change.

The guidelines to follow when conducting experiments in a chemistry laboratory. These rules emphasize safety precautions and good lab practices.

The amount of a substance in grams that corresponds to its molecular weight.

The concentration of a solution expressed as the number of moles of solute per liter of solution.

Always wear a lab coat in the lab to protect yourself from chemicals and spills.

Never use broken glassware in the lab as it can be dangerous.

Never perform experiments that are not assigned to you, as this can be dangerous and lead to unexpected results.

If you spill any chemicals on yourself, wash the affected area immediately with plenty of water and report it to your instructor.

Never touch your eyes with your hands in the lab, as your hands are often contaminated with chemicals.

Dispose of used chemicals and broken glassware in the designated containers.

The process of neutralizing both the strong acid (HCl) and the first ionizable proton of the weak acid (H3PO4) with standard NaOH using methyl orange as the indicator.

The process of neutralizing the total HCl contents and the two ionizable protons of H3PO4 with standard NaOH using phenolphthalein as the indicator and adding NaCl to suppress hydrolysis.

This titration determines the borax content by neutralizing it with standard acid (HCl) using methyl orange as the indicator.

The glycerol increases the acidic strength of the boric acid, allowing it to be titrated with standard NaOH using phenolphthalein as the indicator.

A strong acid, like HCl, suppresses the ionization of a weak acid, like H3BO3, in a solution.

The process of adding standard sodium hydroxide solution (NaOH) to a solution containing both HCl and H3BO3, the HCl reacts first, then the glycerol is added to increase the acidity of the H3BO3 which can then be titrated.

The analysis relies on the fact that borax in solution behaves as a half-neutralized boric acid, allowing for titration using a standard acid.

The analysis involves titrating a mixture containing both borax and boric acid, first with standard acid (HCI) to determine the borax content, then the total boric acid content is determined by titration with standard alkali hydroxide (NaOH) after adding glycerol.

A method for determining the amount of chloride ions in a sample by reacting it with an excess of silver nitrate solution, followed by the removal of silver chloride and titration of the remaining silver nitrate with standard thiocyanate solution.

The technique for determining the concentration of a substance by reacting it with a solution of known concentration (titrant) until the reaction is complete.

The point in a titration at which the reaction between the analyte and the titrant is complete. It is usually indicated by a color change of the indicator.

A substance that changes color in the presence of specific chemicals, indicating the endpoint of a titration.

The amount of a substance that reacts with one mole of another substance.

A method for determining the total alkalinity of a mixture, where excess standard acid is added and the solution is boiled to remove CO2. The remaining unused acid is then titrated with a standard alkali hydroxide using methyl orange (MO) as an indicator.

A method for determining the hydroxide content of a mixture, which involves precipitating the carbonate with barium chloride, and then titrating the hydroxide with a standard acid using phenolphthalein (ph.ph.) as an indicator.

A method for determining the amount of sodium carbonate and hydroxide in a mixture, using a two-indicator approach. In the first step, the total alkalinity is determined using methyl orange as an indicator. In the second step, the hydroxide content is determined using phenolphthalein after precipitating the carbonate with barium chloride.

A method for determining the concentrations of sodium hydroxide and sodium carbonate in a mixture, using two indicators. It involves titrating the mixture with standard acid, first with phenolphthalein (ph.ph.) to determine the hydroxide and half the carbonate, and then with methyl orange (MO) to measure the total alkalinity.

A method for determining the total alkalinity of a mixture of alkali hydroxide and carbonate, using a standard acid and methyl orange (MO) as an indicator.

A method for determining the hydroxide content of a mixture of alkali hydroxide and carbonate, where the carbonate is first precipitated with barium chloride, and then the hydroxide is titrated with a standard acid using phenolphthalein (ph.ph.) as an indicator.

A method for determining the bicarbonate content of a mixture, where the carbonate is first precipitated using barium chloride. The excess unused alkali hydroxide is then titrated with standard acid using phenolphthalein (ph.ph.)

A method for determining the total alkalinity of a mixture of alkali carbonate and bicarbonate, using standard acid and methyl orange (MO) as an indicator.

A titration method used specifically for determining the concentration of chloride ions (Cl-) in a solution using a standard solution of mercuric nitrate (Hg(NO3)2).

A titration method that relies on the formation of a complex between metal ions and a chelating agent, typically EDTA. It involves adding a known amount of the chelating agent to a solution containing the metal ions.