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NaOH and KOH both are strong alkalis the difference is in their solubilities in organic solvents and organic reactions for example alkyl halides undergo substitution in aq. NaOH but elimination in alcoholic KOH'''
KOH (like NaOH) is hygroscopic. Even at high temperatures, solid KOH does not dehydrate readily.
Approximately 121 g of KOH will dissolve in 100 mL of water at room temperature (compared with 100 g of NaOH in the same volume).
KOH, like NaOH, serves as a source of OH−, a highly nucleophilic anion that attacks polar bonds in both inorganic and organic materials.While KOH and NaOH are both strong bases, potassium is further down on the Periodic Table than sodium. That gives you valuable information regarding the nature of these elements. A general rule of thumb is that atoms are more reactive going down a column, and are more reactive as you go toward the left of a row.
The pKb value of potassium hydroxide is 0.5, while the value for sodium hydroxide is 0.2 (the smaller the value of pKb, the stronger the base). Therefore, NaOH is stronger than KOH. In addition, sodium is less electronegative than potassium, so NaOH is more willing to release the hydroxy group and it is stronger base.
Their first ionization energies are different as well: 496kJ/mol for sodium, 419kJ/mol for potassium. The relatively small excess of hydroxide- released by KOH compared with NaOH doesn't seem like it would impart that much added reactivity.
In industrial scale, KOH is more expensive than NaOH (depends on concentration of KOH), so NaOH is widely used instead of KOH. But they both shows many similarities.
- NaOH creates the solids and KOH creates liquid soap.
What else can I help you with?
What is the difference between NaOH and NaOH?
NaOH and KOH both are strong alkalis the difference is in their solubilities in organic solvents and organic reactions for example alkyl halides undergo substitution in aq. NaOH but elimination in alcoholic KOH'''KOH (like NaOH) is hygroscopic. Even at high temperatures, solid KOH does not dehydrate readily.Approximately 121 g of KOH will dissolve in 100 mL of water at room temperature (compared with 100 g of NaOH in the same volume).KOH, like NaOH, serves as a source of OH−, a highly nucleophilic anion that attacks polar bonds in both inorganic and organic materials.While KOH and NaOH are both strong bases, potassium is further down on the Periodic Table than sodium. That gives you valuable information regarding the nature of these elements. A general rule of thumb is that atoms are more reactive going down a column, and are more reactive as you go toward the left of a row.The pKb value of potassium hydroxide is 0.5, while the value for sodium hydroxide is 0.2 (the smaller the value of pKb, the stronger the base). Therefore, NaOH is stronger than KOH. In addition, sodium is less electronegative than potassium, so NaOH is more willing to release the hydroxy group and it is stronger base.Their first ionization energies are different as well: 496kJ/mol for sodium, 419kJ/mol for potassium. The relatively small excess of hydroxide- released by KOH compared with NaOH doesn't seem like it would impart that much added reactivity.In industrial scale, KOH is more expensive than NaOH (depends on concentration of KOH), so NaOH is widely used instead of KOH. But they both shows many similarities.NaOH creates the solids and KOH creates liquid soap.
What is the reaction equation between NaOH and Potassium Hydrogentartrate or KHT?
The reaction equation between NaOH and potassium hydrogen tartrate (KHT) is: 2KHT + 2NaOH → 2KNaTartrate + 2H2O
Is A base which dissolves in water is called an alkali?
Yes, a base that dissolves in water is called an alkali. Alkalis are bases that release hydroxide ions (OH-) in water, resulting in a basic solution. Examples of alkalis include sodium hydroxide (NaOH) and potassium hydroxide (KOH).
Why NAOH reacts with Phenol while KOH doesn't?
They both react with phenol. KOH is actually a slightly stronger base than NaOH. At low concentrations, like less than 0.1M, both NaOH and KOH are essentially 100% dissociated. However, at higher concentrations, a little more of the KOH is dissociated. The point is, both bases will remove virtually all of the H+ from phenol. You received some incorrect information.
What are the examples of basic solutions?
Examples of basic solutions include sodium hydroxide (NaOH) and potassium hydroxide (KOH). These solutions have a pH greater than 7 and can neutralize acids. They are commonly used in various industrial processes and as laboratory reagents.
What is the difference between NaOH and NaOH?
NaOH and KOH both are strong alkalis the difference is in their solubilities in organic solvents and organic reactions for example alkyl halides undergo substitution in aq. NaOH but elimination in alcoholic KOH'''KOH (like NaOH) is hygroscopic. Even at high temperatures, solid KOH does not dehydrate readily.Approximately 121 g of KOH will dissolve in 100 mL of water at room temperature (compared with 100 g of NaOH in the same volume).KOH, like NaOH, serves as a source of OH−, a highly nucleophilic anion that attacks polar bonds in both inorganic and organic materials.While KOH and NaOH are both strong bases, potassium is further down on the Periodic Table than sodium. That gives you valuable information regarding the nature of these elements. A general rule of thumb is that atoms are more reactive going down a column, and are more reactive as you go toward the left of a row.The pKb value of potassium hydroxide is 0.5, while the value for sodium hydroxide is 0.2 (the smaller the value of pKb, the stronger the base). Therefore, NaOH is stronger than KOH. In addition, sodium is less electronegative than potassium, so NaOH is more willing to release the hydroxy group and it is stronger base.Their first ionization energies are different as well: 496kJ/mol for sodium, 419kJ/mol for potassium. The relatively small excess of hydroxide- released by KOH compared with NaOH doesn't seem like it would impart that much added reactivity.In industrial scale, KOH is more expensive than NaOH (depends on concentration of KOH), so NaOH is widely used instead of KOH. But they both shows many similarities.NaOH creates the solids and KOH creates liquid soap.
What is the reaction equation between NaOH and Potassium Hydrogentartrate or KHT?
The reaction equation between NaOH and potassium hydrogen tartrate (KHT) is: 2KHT + 2NaOH → 2KNaTartrate + 2H2O
What are the examples of a base?
NaOH KOH Ca(OH)2
OH- exceptions?
NaOH, LiOH, KOH. (BaOH, CaOH)
What are some inorganic compounds?
KOH, NaOH, KCl, KBr, NaBr
Which bases are in a soap?
NaOH and KOH.{sodium hydroxide and pottassium hydroxide}
What is an example of ionic bond?
NaCl, NaOH, NaBr, KBr, KOH
Is A base which dissolves in water is called an alkali?
Yes, a base that dissolves in water is called an alkali. Alkalis are bases that release hydroxide ions (OH-) in water, resulting in a basic solution. Examples of alkalis include sodium hydroxide (NaOH) and potassium hydroxide (KOH).
Why NAOH reacts with Phenol while KOH doesn't?
They both react with phenol. KOH is actually a slightly stronger base than NaOH. At low concentrations, like less than 0.1M, both NaOH and KOH are essentially 100% dissociated. However, at higher concentrations, a little more of the KOH is dissociated. The point is, both bases will remove virtually all of the H+ from phenol. You received some incorrect information.
What are the examples of basic solutions?
Examples of basic solutions include sodium hydroxide (NaOH) and potassium hydroxide (KOH). These solutions have a pH greater than 7 and can neutralize acids. They are commonly used in various industrial processes and as laboratory reagents.
When KOH absorbs CO2 can this concept be used to control emission of CO2 from automobiles?
Definately, CO2 absorbed by KOH or NaOH. But it require enormously large quantity of KOH or NaOH. KOH is more effective to absorb CO2, because NaOH also absorb water. So I don't think that this is the treatment of global warming.
What compound that produces OH in solution?
Bases, for example NaOH, KOH, LiOH, etc.
