The equilibrium constant for the reactionN,O,(2) = 2NO,(8)is 6.10 x 10 ' at 25'C. Calculate the value of K for thisreaction:NO,(g) = 1/2N,O4(g)(A) 327(B) 164(C) 12.8(D) 3.05 × 10 ³How many moles of HCOON must be added to 1.0 L of0.10 M HCOOH to prepare a buffer solution with a pH of3.4? (HCOOH K, = 2 × 10 “)(A) 0.01(B) 0.05(C) 0.1(D) 0.2What is the percent ionization of a 0.10 M solution of formic acid at 25°C? Formic acid, HCOOH, has aKa value of 1.9 x 104 at 25°C.(A) 0.19%(B) 1.4%(C) 4.4%(D) 14%

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The equilibrium constant for the reaction N,O,(g) = 2NO,(2) is 6.10 x 10' at 25'C. Calculate the value of K for this reaction: NO,(g) = 1/2N,0,(g) (A) 327 (B) 164 (C) 12.8 (D) 3.05 × 10

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Chapter1: Chemical Foundations

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Question

The equilibrium constant for the reaction
N,O,(2) = 2NO,(8)
is 6.10 x 10 ' at 25'C. Calculate the value of K for this
reaction:
NO,(g) = 1/2N,O4(g)
(A) 327
(B) 164
(C) 12.8
(D) 3.05 × 10 ³
How many moles of HCOON must be added to 1.0 L of
0.10 M HCOOH to prepare a buffer solution with a pH of
3.4? (HCOOH K, = 2 × 10 “)
(A) 0.01
(B) 0.05
(C) 0.1
(D) 0.2
What is the percent ionization of a 0.10 M solution of formic acid at 25°C? Formic acid, HCOOH, has a
Ka value of 1.9 x 104 at 25°C.
(A) 0.19%
(B) 1.4%
(C) 4.4%
(D) 14%

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