The pH of a 0.30-M solution of a weak base is 10.66 at 25 o C . The K b of the given base has to be calculated. Concept Information: Strong base and weak base: Strong base dissociates into its constituent ions fully. It produces more of hydroxide ions while dissolved in water. Weak bases partially dissociates into its constituent ions. According to Bronsted-Lowry, strong base is a good proton acceptor whereas weak base is a poor proton acceptor Since, the ionization of a weak base is incomplete; it is treated in the same way as the ionization of a weak acid. The ionization of a weak base B is given by the below equation. B (aq) +H 2 O (l) → HB + (aq) +OH - (aq) The equilibrium expression for the ionization of weak base B will be, K b = [ HB + ] [ OH - ] [ B ] Where, K b is base ionization constant, [ OH − ] is concentration of hydroxide ion [ HB + ] is concentration of conjugate acid [ B] is concentration of the base pOH definition: The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion [OH - ] concentration. pOH scale is analogous to pH scale. pOH = -log[OH - ] Relationship between pH and pOH pOH is similar to pH . The only difference is that in pOH the concentration of hydroxide ion is used as a scale while in pH , the concentration of hydronium ion is used. The relationship between the hydronium ion concentration and the hydroxide ion concentration is given by the equation, pH + pOH = 14, at 25 o C As pOH and pH are opposite scale, the total of both has to be equal to 14.
The pH of a 0.30-M solution of a weak base is 10.66 at 25 o C . The K b of the given base has to be calculated. Concept Information: Strong base and weak base: Strong base dissociates into its constituent ions fully. It produces more of hydroxide ions while dissolved in water. Weak bases partially dissociates into its constituent ions. According to Bronsted-Lowry, strong base is a good proton acceptor whereas weak base is a poor proton acceptor Since, the ionization of a weak base is incomplete; it is treated in the same way as the ionization of a weak acid. The ionization of a weak base B is given by the below equation. B (aq) +H 2 O (l) → HB + (aq) +OH - (aq) The equilibrium expression for the ionization of weak base B will be, K b = [ HB + ] [ OH - ] [ B ] Where, K b is base ionization constant, [ OH − ] is concentration of hydroxide ion [ HB + ] is concentration of conjugate acid [ B] is concentration of the base pOH definition: The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion [OH - ] concentration. pOH scale is analogous to pH scale. pOH = -log[OH - ] Relationship between pH and pOH pOH is similar to pH . The only difference is that in pOH the concentration of hydroxide ion is used as a scale while in pH , the concentration of hydronium ion is used. The relationship between the hydronium ion concentration and the hydroxide ion concentration is given by the equation, pH + pOH = 14, at 25 o C As pOH and pH are opposite scale, the total of both has to be equal to 14.
The pH of a 0.30-M solution of a weak base is 10.66 at 25oC. The Kb of the given base has to be calculated.
Concept Information:
Strong base and weak base:
Strong base dissociates into its constituent ions fully. It produces more of hydroxide ions while dissolved in water. Weak bases partially dissociates into its constituent ions.
According to Bronsted-Lowry, strong base is a good proton acceptor whereas weak base is a poor proton acceptor
Since, the ionization of a weak base is incomplete; it is treated in the same way as the ionization of a weak acid.
The ionization of a weak base B is given by the below equation.
B(aq)+H2O(l)→HB+(aq)+OH-(aq)
The equilibrium expression for the ionization of weak base B will be,
Kb=[HB+][OH-][B]
Where,
Kb is base ionization constant,
[OH−] is concentration of hydroxide ion
[HB+] is concentration of conjugate acid
[B] is concentration of the base
pOH definition:
The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion [OH-] concentration. pOH scale is analogous to pH scale.
pOH=-log[OH-]
Relationship between pH and pOH
pOH is similar to pH. The only difference is that in pOH the concentration of hydroxide ion is used as a scale while in pH, the concentration of hydronium ion is used.
The relationship between the hydronium ion concentration and the hydroxide ion concentration is given by the equation,
pH+pOH=14,at25oC
As pOH and pH are opposite scale, the total of both has to be equal to 14.
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Question 59 of 70
The volume of
1
unit of plasma is 200.0 mL
If the recommended dosage
for adult patients is 10.0 mL per kg of body mass, how many units are needed for
a patient with a body mass of 80.0
kg ?
80.0
kg
10.0
DAL
1
units
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X
4.00
units
1
1
Jeg
200.0
DAL
L
1 units
X
200.0 mL
= 4.00 units
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200.0
2.00
1.60 × 10³
80.0
4.00
0.0400
0.250
10.0
8.00
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Identify the starting material in the following reaction. Click the "draw structure" button to launch the
drawing utility.
draw structure ...
[1] 0 3
C10H18
[2] CH3SCH3
H
In an equilibrium mixture of the formation of ammonia from nitrogen and hydrogen, it is found that
PNH3 = 0.147 atm, PN2 = 1.41 atm and Pн2 = 6.00 atm. Evaluate Kp and Kc at 500 °C.
2 NH3 (g) N2 (g) + 3 H₂ (g)
K₂ = (PN2)(PH2)³ = (1.41) (6.00)³ = 1.41 x 104