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The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25C of 1.8 x 10-5. The reaction is as follows : CH3COOH (aq) CH3COO- (aq) + H+ (aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO- is 8.1 x 10-3 moles in the same 0.500 L, calculate [H+] for the reaction.
Complete the following acid base reactions, indicate the conjugate acid-base pairs, and state whether the reaction has a large or small equilibrium constant.
a. CH3COOH(aq) + NH3(aq)
b. H2CO3 (aq) + NO3 - (aq)
c. H2CO3 (aq) + H2O (l)
d. HCO3 - (aq) + H2O (l)
e. NH3 (aq) + H2O (l)
a. Write the balanced equation for the ionization reaction.
b. Write the expression for Ka.
c. What can we say about the size of Ka for this reaction?
Consider the reaction: NaNO3(s) + H2SO4(l) → NaHSO4(s) + HNO3(g) ΔH° = 21.2 kJ How much heat must absorbed by the reaction system to convert 100g of NaNO3 into NaHSO4(s)?
a) H2C=CH+ b) H2C=CH- and c) H2C=CH.
hydroxide?
3.
H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l) ΔH
