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What is the pKb value for the acetate ion?
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Aijaz Haider
What is the pKb value for the acetate ion?
To give you an answer I would have to look it up, since I don't routinely carry this type of information in my head. It would be quicker and easier for you to do the same.
To give you an answer I would have to look it up, since I don't routinely carry this type of information in my head. It would be quicker and easier for you to do the same.
According to the information in the Wikipedia article on the acid dissociation constant, [math] ext{p}K_ ext{b}[/math], the logarithmic form of the base association constant [math]K_ ext{b}[/math], is [math] ext{p}K_ ext{b}= ext{p}K_ ext{w}- ext{p}K_ ext{a}[/math], where [math] ext{p}K_ ext{a}[/math] is the logarithmic form of the acid’s dissociation constant [math]K_ ext{a}[/math] and [math] ext{p}K_ ext{w}[/math] is the logarithmic form of water’s self-ionization constant [math]K_ ext{w}[/math].
At 25 °C, [math] ext{p}K_ ext{w}[/math] = 13.997 and [math] ext{p}K_ ext{a}[/math] (in water solution) is 4.756, so [math] ext{p}K_ ext{b}[/math] = 9.241.
According to the information in the Wikipedia article on the acid dissociation constant, [math]ext{p}K_ext{b}[/math], the logarithmic form of the base association constant [math]K_ext{b}[/math], is [math]ext{p}K_ext{b}=ext{p}K_ext{w}-ext{p}K_ext{a}[/math], where [math]ext{p}K_ext{a}[/math] is the logarithmic form of the acid’s dissociation constant [math]K_ext{a}[/math] and [math]ext{p}K_ext{w}[/math] is the logarithmic form of water’s self-ionization constant [math]K_ext{w}[/math].
At 25 °C, [math]ext{p}K_ext{w}[/math] = 13.997 and [math]ext{p}K_ext{a}[/math] (in water solution) is 4.756, so [math]ext{p}K_ext{b}[/math] = 9.241.
To give you an answer I would have to look it up, since I don't routinely carry this type of information in my head. It would be quicker and easier for you to do the same.
To give you an answer I would have to look it up, since I don't routinely carry this type of information in my head. It would be quicker and easier for you to do the same.
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What is the pKb value for the acetate ion?
According to the information in the Wikipedia article on the acid dissociation constant, [math] ext{p}K_ ext{b}[/math], the logarithmic form of the base association constant [math]K_ ext{b}[/math], is [math] ext{p}K_ ext{b}= ext{p}K_ ext{w}- ext{p}K_ ext{a}[/math], where [math] ext{p}K_ ext{a}[/math] is the logarithmic form of the acid’s dissociation constant [math]K_ ext{a}[/math] and [math] ext{p}K_ ext{w}[/math] is the logarithmic form of water’s self-ionization constant [math]K_ ext{w}[/math].
At 25 °C, [math] ext{p}K_ ext{w}[/math] = 13.997 and [math] ext{p}K_ ext{a}[/math] (in water solution) is 4.756, so [math] ext{p}K_ ext{b}[/math] = 9.241.
What is the pKb value for the acetate ion?
According to the information in the Wikipedia article on the acid dissociation constant, [math]ext{p}K_ext{b}[/math], the logarithmic form of the base association constant [math]K_ext{b}[/math], is [math]ext{p}K_ext{b}=ext{p}K_ext{w}-ext{p}K_ext{a}[/math], where [math]ext{p}K_ext{a}[/math] is the logarithmic form of the acid’s dissociation constant [math]K_ext{a}[/math] and [math]ext{p}K_ext{w}[/math] is the logarithmic form of water’s self-ionization constant [math]K_ext{w}[/math].
At 25 °C, [math]ext{p}K_ext{w}[/math] = 13.997 and [math]ext{p}K_ext{a}[/math] (in water solution) is 4.756, so [math]ext{p}K_ext{b}[/math] = 9.241.
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