The concentrations of HCO 3 - , CO 3 2 − and H + ions in a 0.025 M H 2 CO 3 solution has to be calculated. Concept Information: Acid ionization constant K a : Acids ionize in water. Strong acids ionize completely whereas weak acids ionize to some limited extent. The degree to which a weak acid ionizes depends on the concentration of the acid and the equilibrium constant for the ionization. The ionization of a weak acid HA can be given as follows, HA (aq) → H + (aq) +A - (aq) The equilibrium expression for the above reaction 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 To Calculate: The concentrations of HCO 3 - , CO 3 2 − and H + ions in a 0.25 M H 2 CO 3 solution
The concentrations of HCO 3 - , CO 3 2 − and H + ions in a 0.025 M H 2 CO 3 solution has to be calculated. Concept Information: Acid ionization constant K a : Acids ionize in water. Strong acids ionize completely whereas weak acids ionize to some limited extent. The degree to which a weak acid ionizes depends on the concentration of the acid and the equilibrium constant for the ionization. The ionization of a weak acid HA can be given as follows, HA (aq) → H + (aq) +A - (aq) The equilibrium expression for the above reaction 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 To Calculate: The concentrations of HCO 3 - , CO 3 2 − and H + ions in a 0.25 M H 2 CO 3 solution
Solution Summary: The author calculates the acid ionization constant and equilibrium constant for a weak acid HA.
Calculate the pH of a solution that was prepared by mixing 25.00 mL of a 0.1630 M HClO4 solution with 20.00 mL of a 0.1350 Ba(OH)2 solution
The acidity of a solution is measured by its pH.
If Ht represents the concentration of hydrogen ions (in moles/liter) in the solution,
the pH is defined by pH = – log H+
Based on careful measurements and calculations, a chemist examines two solutions and asserts:
"The hydrogen ion concentration of Solution A
is 158 times greater than
the hydrogen ion concentration of Solution B."
If the pH of solution B is 3.4, determine the pH of Solution A.
Report your answer to one decimal place.
Solution A has pH equal to
Number
(Report to the nearest 0.1)
Calculate the number of H+(aq)H+(aq) ions in 1.2 mLmL of pure water at 25 ∘C∘C.
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