The pH of a 0.20 M ammonium acetate 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 pH definition: The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale. The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration. pH = -log[H 3 O + ] To Calculate: The pH of a 0.20 M ammonium acetate solution
The pH of a 0.20 M ammonium acetate 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 pH definition: The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale. The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration. pH = -log[H 3 O + ] To Calculate: The pH of a 0.20 M ammonium acetate solution
Solution Summary: The author explains that the pH of a 0.20 M ammonium-acetate solution has to be calculated. The equilibrium expression for the reaction is given below.
The pH of a 0.20 M ammonium acetate solution has to be calculated
Concept Information:
Acid ionization constant
Ka:
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 constant
Kb
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
pH definition:
The concentration of hydrogen ion is measured using
pH scale. The acidity of aqueous solution is expressed by
pH scale.
The
pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.
pH=-log[H3O+]
To Calculate: The pH of a 0.20 M ammonium acetate solution
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