The pH of a 0.1 M solution of NaOH. 0.1 1 10 (D) 12 (E) 0.01 True or False, at e

Question

The pH of a 0.1 M solution of NaOH. 0.1 1 10 (D) 12 (E) 0.01 True or False, at equilibrium the forward rate is not equal to the reverse rate. The equilibrium constant for a gas phase reaction is K_eq = 2.8* 10^2 at 999 K. At equilibrium, products predominate reactants predominate roughly equal amounts of products and reactants are present (D) only products are present (E) only reactants are present How is the reaction quotient used to determine whether a system is at equilibrium? The reaction quotient must be satisfied for equilibrium to be achieved. At equilibrium, the reaction quotient is undefined. The reaction is at equilibrium when Q K_eq. (E) The reaction is at equilibrium when Q = K_eq. An acid that releases more than proton is called? polyprotic neutral a buffer (D) amphiprotic (E) none of the above

Explanation / Answer

1. pH of base = 14 - (-log(OH-))

   = 14 - (-log0.1)

pH = 13

2. false , at equilibrium both are equal

3. if K>1 , the products predominate

answer: A

4. answer: E

the reaction is at equilibrium when Q=Keq

5. answer: E.none of the above.

acid releases proton and gives conjugate base.

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