The K a of a 0 .400 M formic acid HCOOH solution has to be calculated Concept Information: Acid ionization constant K a : The equilibrium expression for the reaction HA ( a q ) → H + ( a q ) + A - ( a q ) is given below. K a = [ H + ][A - ] [ HA] Where K a is acid ionization constant, [ H + ] is concentration of hydrogen ion, [ A - ] is concentration of acid anion, [ HA] is concentration of the acid Base ionization constant K b The equilibrium expression for the ionization of weak base B will be, B ( a q ) + H 2 O ( l ) → HB + ( a q ) + OH - ( a q ) 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 Relationship between K a and K b K a × K b =K w
The K a of a 0 .400 M formic acid HCOOH solution has to be calculated Concept Information: Acid ionization constant K a : The equilibrium expression for the reaction HA ( a q ) → H + ( a q ) + A - ( a q ) is given below. K a = [ H + ][A - ] [ HA] Where K a is acid ionization constant, [ H + ] is concentration of hydrogen ion, [ A - ] is concentration of acid anion, [ HA] is concentration of the acid Base ionization constant K b The equilibrium expression for the ionization of weak base B will be, B ( a q ) + H 2 O ( l ) → HB + ( a q ) + OH - ( a q ) 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 Relationship between K a and K b K a × K b =K w
Solution Summary: The author explains that the equilibrium expression for the ionization of weak base B is given below.
Definition Definition State where the components involved in a reversible reaction, namely reactants and product, do not change concentration any further with time. Chemical equilibrium results when the rate of the forward reaction becomes equal to the rate of the reverse reaction.
Chapter 15, Problem 15.138QP
Interpretation Introduction
Interpretation:
The Ka of a 0.400 M formic acid HCOOH solution has to be calculated
Concept Information:
Acid ionization constantKa:
The equilibrium expression for the reaction HA(aq)→H+(aq)+A-(aq) is given below.
Ka=[H+][A-][HA]
Where Ka is acid ionization constant, [H+] is concentration of hydrogen ion, [A-] is concentration of acid anion, [HA] is concentration of the acid
Base ionization constantKb
The equilibrium expression for the ionization of weak base B will be,
B(aq)+H2O(l)→HB+(aq)+OH-(aq)
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
43) 10.00 ml of vinegar (active ingredient is acetic acid) is titrated to the endpoint
using 19.32 ml of 0.250 M sodium hydroxide. What is the molarity of acetic acid
in the vinegar? YOU MUST SHOW YOUR WORK.
NOTE: MA x VA = MB x VB
424 Repon Sheet Rates of Chemical Reactions : Rate and Order of 1,0, Deception
B. Effect of Temperature
BATH TEMPERATURE
35'c
Yol of Oh
نام
Time
485
Buret rend
ing(n)
12
194
16.
6
18
20
10
22
24
14
115 95
14738
2158235
8:26 CMS
40148
Total volume of 0, collected
Barometric pressure 770-572
ml
mm Hg
Vapor pressure of water at bath temperature (see Appendix L) 42.2
Slope
Compared with the rate found for solution 1, there is
Using the ideal gas law, calculate the moles of O; collected
(show calculations)
times faster
10
Based on the moles of O, evolved, calculate the molar concentration of the original 3% 1,0, solution (sho
calculations)
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