The dissociation of the weak acid, nitrous acid, HNO2, takes place according to the reaction: HNO2 (aq) ⇌ H+ (aq) + NO2 – (aq) K=7.2 X 10-4 When 1.00 mole of HNO2 is added to 1.00 L of water, the H+ concentration at equilibrium is 0.0265 M. A) Calculate the value of Q if 1.00 L of water is added? B) How will reaction shift if 1.00 L of water is added?
The dissociation of the weak acid, nitrous acid, HNO2, takes place according to the reaction: HNO2 (aq) ⇌ H+ (aq) + NO2 – (aq) K=7.2 X 10-4 When 1.00 mole of HNO2 is added to 1.00 L of water, the H+ concentration at equilibrium is 0.0265 M. A) Calculate the value of Q if 1.00 L of water is added? B) How will reaction shift if 1.00 L of water is added?
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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4) The dissociation of the weak acid, nitrous acid, HNO2, takes place according to the reaction:
HNO2 (aq) ⇌ H+
(aq) + NO2
–
(aq) K=7.2 X 10-4
When 1.00 mole of HNO2 is added to 1.00 L of water, the H+ concentration at equilibrium is 0.0265 M.
A) Calculate the value of Q if 1.00 L of water is added?
B) How will reaction shift if 1.00 L of water is added?
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You did not divide by any reactants for Q. Is that becuase the concentration of HNO2 is 1 M? ...and if so, why would it not be 0.5M?
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