Carbonic acid Flashcards
(4 cards)
Explain how this increase in the concentration of carbon dioxide affects the pH of blood.
Co2 + h20 __ h2co3
h2co3 — H+ + HCO3-
when the concentration of co2 rises more h2co3 is made as the equilibrium is shifted to the right as the h2co3 increases the equilibrium of equation is shifted tp the right to make more hydrogen ions. lowering the ph
explain how the carbonic acid-hydrogencarbonate buffer system in equilibrium system 2 acts to restore the pHA OF THE BLOOD after a person has excerised
since more h+ is made equilibrium shifts to the left ti make more h2co3 restoring the ph
One of the systems controlling the pH of blood is the
carbonic acid-hydrogencarbonate buffer system.
H2CO3 _` H+
+ HCO3
–
Explain how this buffer system helps to control the pH of blood when extra
carbon dioxide is present due to strenuous exercise.
co2 dissolves in blood to form h2co3
h2o3 shifts to the right when concentration of co2 increases
h2co3 dissociates into H+ and HCO3- excess of hydrogencarbonate ions combine
with the H+ ions (to help to control blood pH)
An equilibrium exists in aqueous solution between the chromate(VI) ions and the
dichromate(VI) ions.
2CrO4
2–(aq) + 2H+
(aq) _` Cr2O7
2–(aq) + H2O(l)
Explain any change in the position of equilibrium if a few drops of
sodium hydroxide solution are added to this equilibrium system.
What happens when sodium hydroxide (NaOH) is added? NaOH is a strong base and adds OH⁻ ions to the solution. These OH⁻ ions react with H⁺ ions in the equilibrium to form water: 𝐻 + + 𝑂 𝐻 − → 𝐻 2 𝑂 H + +OH − →H 2 O This removes H⁺ ions from the equilibrium.
