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# Calculate the [OH-] of a solution with pH=4 Muliple Choice Questions

Question posted by  Calculate the [OH-] of a solution with pH=4
a-1.0 x 10^-4
b- 4 x 10^ -1
c-1.0 x 10^10
d- 1.0 x !0^-10

Calculate the [H3O+] of a solution with pH =2
a- 2 x 10^-10
b-1 x 10^10
c- 1.0 x 10^+2
d- 1 x 10^-12
e- 1 x 10^-2

What is the solubility constant expression Ksp, for copper (II) hydroxiide, Cu(OH)2?
a-Ksp= [Cu^2+] [2OH-]
b-Ksp= [Cu^2+] [OH-]^2
c-Ksp= [Cu(OH)2]/[Cu^2+][OH-]^2
e-Ksp= [Cu^2+] [OH-]^2/[Cu(OH)2]

The rate of any chemical reaction can be determined by observing
a- the ratio of product concentraion to reactant concenration
b- the precent composition of the final product
c- the amount of product formed in a unit of time
d- the theoretical yield of the reaction
e- the number of chemical bonds broken and remade

in the following gas phase reaction what is the effect of adding more NO2 to the starting reaction mixture? 2 NO2 <=> N2O4
a- it would decease the final quanity of products
b- it would slow the reaction down
c- it would make the reaction more endothermic
d- it would make the reaction more exothermic
e- i would increase the final quantity of products

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## [Solved] Calculate the [OH-] of a solution with pH=4 Muliple Choice Questions

• This Solution has been Purchased 1 time
• Submitted On 19 Jan, 2015 11:33:10  Calculate the [OH-] of a solution with pH=4
a-1.0 x 10^-4
b- 4 x 10^ -1
c-1.0 x 10^10
d- 1.0 x !0^-10

Calculate the [H3O+] of a solution with pH =2
a- 2 x 10^-10
b-1 x 10^10
c- 1.0 x 10^+2
d- 1 x 10^-12
e- 1 x 10^-2

What is the solubility constant...

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