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1- Calculating [H+] for Pure Water: In a certain acidic solution at 25 ∘C, [H+] is...

1- Calculating [H+] for Pure Water: In a certain acidic solution at 25 ∘C, [H+] is 100 times greater than [OH −]. What is the value for [OH −] for the solution? In a certain acidic solution at 25 , [] is 100 times greater than [ ]. What is the value for [ ] for the solution?

1.0×10−8 M
1.0×10−7 M
1.0×10−6 M
1.0×10−2 M
1.0×10−9 M

2. ± Acid-Base Relationships in Water: Water ionizes by the equation H2O(l)⇌H+(aq)+OH−(aq)The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H+] and [OH−]: Kw=[H+][OH−] Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature.

partA What is the H+ concentration for an aqueous solution with pOH = 2.51 at 25 ∘C? [H+]=?

partB Arrange the following aqueous solutions, all at 25 ∘C, in order of decreasing acidity, most acidic to most basic. (pH=5.45, 0.0018 M KOH, 0.0023 M HCL, pOH=8.55)

partcC At a certain temperature, the pH of a neutral solution is 7.83. What is the value of Kw at that temperature? Kw=?

3. To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid. Sulfuric acid, H2SO4, is a strong acid. Its complete dissociation in aqueous solution is represented as H2SO4→H++HSO4− A HSO4− anion can dissociate further by HSO4−⇌H++SO42− but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as Ka2=[H+][SO42−][HSO4−]=0.012

partA Calculate the concentration of H+ ions in a 0.010 M aqueous solution of sulfuric acid. [H+]=?

partB Calculate the concentration of SO42− ions in a 0.010 M aqueous solution of sulfuric acid. [SO42−] =?

partC Calculate the concentration of HSO4− ions in a 0.010 M aqueous solution of sulfuric acid.[HSO4−]=?

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