The percentage of NH 3 , which is present in NH 4 + , is to be determined. Concept introduction: The ionization of a weak base takes place as B ( aq ) + H 2 O ( l ) ⇌ OH − ( aq ) + HB + ( aq ) The formula to calculate the pOH of the solution from the concentration of hydroxide ions is pOH = − log [ OH − ] …… (1) K b is a measure of dissociation of a base and is known as base-ionization constant, which is specific at a particular temperature. K b = [ OH − ] [ BH + ] [ B ] …… (2) Percent ionization is the percentage of base that gets ionized upon addition of water. It depends on the hydroxide ion concentration or the conjugate acid concentration. % ionization = [ OH − ] eq [ B ] o × 100 % = [ BH + ] eq [ B ] o × 100 % …… (3) Here, [ OH − ] eq is hydroxide ion concentration at equilibrium, [ BH + ] eq is the conjugate acid concentration at equilibrium, and [ B ] o is original base concentration.
The percentage of NH 3 , which is present in NH 4 + , is to be determined. Concept introduction: The ionization of a weak base takes place as B ( aq ) + H 2 O ( l ) ⇌ OH − ( aq ) + HB + ( aq ) The formula to calculate the pOH of the solution from the concentration of hydroxide ions is pOH = − log [ OH − ] …… (1) K b is a measure of dissociation of a base and is known as base-ionization constant, which is specific at a particular temperature. K b = [ OH − ] [ BH + ] [ B ] …… (2) Percent ionization is the percentage of base that gets ionized upon addition of water. It depends on the hydroxide ion concentration or the conjugate acid concentration. % ionization = [ OH − ] eq [ B ] o × 100 % = [ BH + ] eq [ B ] o × 100 % …… (3) Here, [ OH − ] eq is hydroxide ion concentration at equilibrium, [ BH + ] eq is the conjugate acid concentration at equilibrium, and [ B ] o is original base concentration.
Solution Summary: The author explains the formula to calculate the pOH of the solution from the concentration of hydroxide ions.
The percentage of NH3, which is present in NH4+, is to be determined.
Concept introduction:
The ionization of a weak base takes place as
B(aq)+H2O(l)⇌OH−(aq)+HB+(aq)
The formula to calculate the pOH of the solution from the concentration of hydroxide ions is
pOH=−log[OH−] …… (1)
Kb is a measure of dissociation of a base and is known as base-ionization constant, which is specific at a particular temperature.
Kb=[OH−][BH+][B]
…… (2)
Percent ionization is the percentage of base that gets ionized upon addition of water. It depends on the hydroxide ion concentration or the conjugate acid concentration.
Here, [OH−]eq is hydroxide ion concentration at equilibrium, [BH+]eq is the conjugate acid concentration at equilibrium, and [B]o is original base concentration.
A student proposes the transformation below in one step of an organic synthesis. There may be one or more reactants missing from the left-hand side, but there
are no products missing from the right-hand side. There may also be catalysts, small inorganic reagents, and other important reaction conditions missing from
the arrow.
• Is the student's transformation possible? If not, check the box under the drawing area.
. If the student's transformation is possible, then complete the reaction by adding any missing reactants to the left-hand side, and adding required catalysts,
inorganic reagents, or other important reaction conditions above and below the arrow.
• You do not need to balance the reaction, but be sure every important organic reactant or product is shown.
+
T
X
O
O
лет-ле
HO
OH
HO
OH
This transformation can't be done in one step.
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell