Titrations

Ionic compounds are mad by ionic bonding The two parts of the compound ther for become one by means of moving electronioc and beoming stable there fore the bond and the compound is stronger that conalent compounds which just share the electrons needed for the two (or more ) elements to become a compound so they are weaker

The equivalence point represents a region where the amount of acid to base (or base to acid) concentration is equal. Before the equivalence point there is a greater amount of acid (or base, depending on the titration). After the titration there is a greater amount of base (or acid). This reverse in dominance results in a dramatic change in pH.

Indicators are weak acid. Too much will alter the titre

Standard solutions are used to check instruments and methods of analysis.

The pH was changed.

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pH must be constant by use of a buffer solution. Control of pH is important since the H+ ion plays an important role in chelation. Equation below shows complexation between metal ion and H+ ions for ligand:Thus and as mentioned before, stability of metal complex is pH dependent. Lower the pH of the solution, lesser would be the stability of complex (because more H+ ions are available to compete with the metal ions for ligand). Only metals that form very stable complexes can be titrated in acidic solution, and metals forming weak complexes can only be effectively titrated in alkaline solution. colour change of the indicator as well as the colour of the EDTA alos depend on the pH of themedium Therefor in EDTA tirtrations the pH of themedium is important :)

A chemical reaction must exist between the titrant an the ion to be analyzed.

The expected shapes of photometric titration typically follow sigmoidal curves, with a rapid increase or decrease in signal intensity as the analyte concentration changes. At the beginning, the signal intensity changes slowly, then increases more rapidly, followed by a plateau where the signal levels off. This shape is indicative of the gradual binding or reaction between the analyte and titrant.

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It is easier to answer this by using examples. Let us suppose we have 4g of NaOH in 100 mls of waste water (4%). Titrating with 1M HCl would require 100ml of titrant. That would thus mean we would need 1000ml of 0.1M HCl titrant run from a buret which is extremely impractical. The concentrations thus affect volumes and thus titration flask sizes etc. It also would affect the time taken and the practicality.

It is not mandatory; acids are also titrated.

In back titration, a known excess of a reagent is added to react with the analyte. After the reaction is complete, the amount of excess reagent is determined by titration with another reagent. The difference between the initial amount of excess reagent and the amount required in the back titration is used to determine the amount of analyte present.

An indicator shows when we have added just enough of the second reagent to react with the first. If you mean why do we add only a small amount of indicator, it is to keep the answer accurate. Some of the reagent is used changing the indicator so the answer is always slightly bigger than perfection, and the more indicator you add, the larger the error.

The platinum electrode is used in coductometry.

Phenolphthalein is used as an indicator because the color of the solution is changed according to pH.

1. Add alkali (not soda) to acid, the other way around is not favoured.
2. .... ?

1. The advantage in diluting the solution before titration is that it allows for greater accuracy in the titration; this is because the color change in the solution is easier to observe if it is a dilute solution.

During non-aqueous titration of amine salts, the halide ions, namely: chloride, bromide and iodide are very weakly basic in character so much so that they cannot react quantitatively with acetous perchloric acid. In order to overcome this problem, mercuric acetate is usually added (it remains undissociated in acetic acid solution) to a halide salt thereby causing the replacement of halide ion by an equivalent amount of acetate ion, which serves as a strong base in acetic acid as shown below: 2R.NH2.HCl ↔ 2RNH3 + + 2Cl - (CH3COO) 2 Hg + 2Cl- → HgCl2 + 2CH3COO- undissociated 2CH3COOH2+ + 2CH3COO- ↔ 4 CH3 COOH

In acid-base titration, the reaction involves the transfer of protons between the acid and base, with the endpoint usually determined by a pH indicator. Redox titration, on the other hand, involves the transfer of electrons between the oxidizing and reducing agents, with the endpoint typically determined by a change in color or potential. Acid-base titrations are used to determine the concentration of acids or bases, while redox titrations are to determine the concentration of oxidizing or reducing agents.