0
When excess of hydrogen or hydronium ions are present in the solution , the solution will have pH less than 0. Phenolphthalein possesses dark orange color to the solution having pH less than 0. Hence, phenolphthalein will possess dark orange color in the presence of excess of hydrogen or hydronium ions.
What else can I help you with?
What is the solution that contains more hydronium ions than hydroxide ions?
If it is in water (supposedly meant by questioneer), the pH value is below 7.0, so it is an acid solution: more H+ than OH-
Is an acid base or salt used to excess hydroxide ions?
Maybe if you asked the question properly, we could answer.
Why does aluminium hydroxide redissolve in excess sodium hydroxide?
Al(OH)3 (s) + OH- (aq) -------> [Al(OH)4]- (aq) Aluminium hydroxide undergoes further reaction with hydroxide ion to from a complex ion, which is of course, soluble in water. Some other metal hydroxides also have similar reaction, like zinc hydroxide, and lead (II) hydroxide.
Copper reacts with sodium hydroxide?
Copper metal itself does not react with sodium hydroxide. But when NaOH is added to a solution of copper ions, it would form a light blue precipitate, which is copper(II) hydroxide, and will NOT dissolve with the excess alkali.
Why zinc hydroxide is soluble in excess of sodium hydroxide solution?
Zinc hydroxide Zn(OH)2 is an inorganic chemical compound. It also occurs naturally as 3 rare minerals: wülfingite (orthorhombic), ashoverite and sweetite (both tetragonal).Like the hydroxides of other metals, such as lead, aluminium, beryllium, tin and chromium, zinc hydroxide (and zinc oxide), is amphoteric. Thus it will dissolve readily in a dilute solution of a strong acid, such as HCl, and also in a solution of an alkali such as sodium hydroxide.It can be prepared by adding sodium hydroxide solution, but not in excess, to a solution of any zinc salt. A white precipitate will be seen: Zn2+ + 2OH- → Zn(OH)2.If excess sodium hydroxide is added, the precipitate of zinc hydroxide will dissolve, forming a colorless solution of zincate ion: Zn(OH)2 + 2OH- → Zn(OH)42-. This property can be used as a test for zinc ions in solution, but it is not exclusive, since aluminum and lead compounds behave in a very similar manner. Unlike the hydroxides of aluminum and lead, zinc hydroxide also dissolves in aqueous ammonia to form a colourless, water-soluble ammine complexThe reason that the zinc hydroxide will dissolve is because the ion is normally surrounded by water ligands; when excess sodium hydroxide is added to the solution the hydroxide ions will reduce the complex to a -2 charge and make it soluble. When excess ammonia is added, it sets up an equilibirum which provides hydroxide ions; the formation of hydroxide ions causes a similar reaction as sodium hydroxide and creates a +2 charged complex with a co-ordination number of 4 with the ammonia ligands - this makes the complex soluble so that it dissolves
Which ion is excess in alkali solution?
OH- ions are present in excess in alkaline solution
Which indicators are used for alkalinity titration?
The indicators commonly used for alkalinity titration include phenolphthalein and bromcresol green. Phenolphthalein turns pink in the presence of excess base (at a pH greater than 8.2), while bromcresol green changes color from yellow to blue in the pH range of 3.8 to 5.4, indicating the endpoint of the titration.
Why is phenolphthalein an appropiate indicator for back titration?
Phenolphthalein is appropriate for back titration because it undergoes a color change in a specific pH range (pH ~8.2-10), making it useful for detecting excess acid or base after a reaction is complete. In back titrations, where the analyte is in excess and the titrant is limited, phenolphthalein helps determine the amount of excess analyte present by signaling the endpoint of the reaction.
Does it take more NaOH in back titration with phenolphthalein?
Yes, it takes more NaOH in a back titration with phenolphthalein compared to a direct titration because the indicator reacts with the excess acid in the sample before the endpoint is reached. This means more base is required to neutralize the excess acid present.
What is the predicted effect on the reaction of zinc nitrate and excess sodium hydroxide?
The reaction of zinc nitrate and excess sodium hydroxide begins with precipitation of zinc hydroxide ( Zn(OH)2 ), followed by dissolvement after adding excess sodium hydroxide ( 2 OH- ) to formation of zinc aat-ions ( [Zn(OH)4]2- )
What happens when sodium hydroxide is added to acetic acid?
When sodium hydroxide is added to acetic acid, a neutralization reaction occurs, resulting in the formation of sodium acetate and water. This reaction also releases heat. Additionally, the resulting solution will be basic due to the presence of excess hydroxide ions.
What is the balanced equation for zinc hydroxide react with excess sodium hydroxide?
There is no reaction between zinc hydroxide and sodium hydroxide.
What is the solution that contains more hydronium ions than hydroxide ions?
If it is in water (supposedly meant by questioneer), the pH value is below 7.0, so it is an acid solution: more H+ than OH-
Is an acid base or salt used to excess hydroxide ions?
Maybe if you asked the question properly, we could answer.
When Ammonium Hydroxide excess is added to ferrous sulphate?
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Why do the solution of the white precipitate of Zinc hydroxide dissolve in excess of Ammonium hydroxide?
The white precipitate of zinc hydroxide dissolves in excess ammonium hydroxide because of the formation of the complex ion [Zn(NH3)4]2+. This complex ion is soluble in water, leading to the dissolution of the precipitate. The excess ammonium hydroxide provides additional ammonia molecules to form more of the soluble complex ions, increasing the solubility of zinc hydroxide.
Why does aluminium hydroxide redissolve in excess sodium hydroxide?
Al(OH)3 (s) + OH- (aq) -------> [Al(OH)4]- (aq) Aluminium hydroxide undergoes further reaction with hydroxide ion to from a complex ion, which is of course, soluble in water. Some other metal hydroxides also have similar reaction, like zinc hydroxide, and lead (II) hydroxide.
