In the reaction of an acid with a base, the common ionic reaction involves ions

Question

In the reaction of an acid with a base, the common ionic reaction involves ions of a. hydrogen and hydroxide 10. sodium and chloride c. hydrogen and hydronium d. hydroxide and nitrate 11. Which of the following is NOT a conjugate acid-base pair? a. NH4+/NH3 b. H30 /OH d. C2H302 /HC2H302 Place the following in order of increasing acid strength. HBrO, HBrO, HBro HBro 12. Calculate the hydronium ion concentration in an aqueous solution with a pOH of 9.85 at 25°C a. 7.1 x 10-5 M b. 4.2 x 10-10 M c. 8.7 x 10-10 M d. 1.4×10-10M 13. Which of the following statements is TRUE? The rate constant does not depend on the activation energy for a reaction where the products are lower in energy than the reactants. A catalyst raises the activation energy of a reaction. Rate constants are temperature dependent. The addition of a homogeneous catalyst does not change the activation energy of a given reaction. 14. a. b. c. d. e. None of the above are true. 15. What element is being reduced in the following redox reaction? Mn04-(aq) + H2C204(aq) Mn2+(aq) + CO2(g) a. C c. Mn d. H 16. Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H' and Fe3+ in the balanced reaction? 5 CHM 2046 Pre-Post Test Effective 08/2015

Explanation / Answer

Q10

acid base will have always

XOH + HY = H2O + XY

therefore,

hydrogen and hydroxide (H+ and OH-)

Q11

First, let us define Bronsted Lowry acid/base:

Bronsted Lowry acid: any species that will donate H+ (protons) in solution, and makes pH lower (i.e HCl)

Bronsted Lowry base: any species that will accept H+ (protons) in solution, and makes pH higher (NH3 will accept H+ to form NH4+)

Typically, acid/bases are shown in the left (reactants)

when we write the products:

Bronsted Lowery conjugate base = the base formed when the B.L. acid donates its H+ proton ( i.e. HCl -> Cl-

Bronsted Lowery conjugate acid = the acid formed when the B.L. base accept its H+ proton ( i.e. NH4+ has accept H+ proton)

therefore

H#O4+ vs. OH- since there is no H2O in between!

Q12

The strenght is directly proprtional to Oxygen

so

O < O2 < O3 < O4

choose d

Q13

pH = 14-pOH = 14-9.85

pH = 4.15

[H++] = 10^-4.15 = 7.08*10^-5

choose a

Q14

a)

false, it DOES depend

b)

false, it lowers activation energy

c)

true, since K is f(T)

d)

false, hasno effect

e)

false, since c is true

Q15

Reduction = species that GAINS electrons

Oxidation = process in which a specie will LOSS electrons

Reducing agent = The species that favors reduction, i.e. it will oxidize in order to reduce another species

Oxidizing agent = The species that favors oxidation, i.e. it will reduce in order to oxidise another species

therefore

Mn goes from +7 to +2, then it gains 5 electrons, it is getting reduced

choose Mn

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