A) A water sollution has the pH = 10.00, determine the molar concentration of H3

Question

A) A water sollution has the pH = 10.00, determine the molar concentration of H3O+ in this solution.

           a) determine the molar concentration of OH- in this solution

B) Consider a neutral water solution, determine the molar concentration of H3O+ in this solution

           a) determine the molar concentration of OH- in this solution

C) Consider a water solution with molar concentration of H3O+ = 6.4 x 10^-12. Determine the molar concentration of OH- in this solution

          a) Determine the pH of this solution

D) Consider a water solution with pH= 11.3, determine the molar concentration of H3O+ in this solution

         a) determine the molar concentration of OH- in this solution

E) A 12.0mL sample of vinegar, which is an aqueous solution of acetic acid, HC2H3O2, requires 20.5 mL of 0.550M NaOH to reach the endpoint in a titration

HC2H3O2(aq) + NaOH(aq) --> NaC2H3(aq) + H2O(l)

What is the molarity of the acetic acid solution?

Explanation / Answer

A)a)pH=10

pOH=14-10

=4

so [H3O+]=10^-10

so [OH-]=10^-4 M

B) for neutral water,

[OH-]=[H3O+]=10^-7 M

C)[OH-]=10^-14/(6.4*10^-12)

=1.56*10^-3 M

pH=-log(6.4*10^-12)

=11.19

D)[H3O+]=10^-11.3

=5.01*10^-12 M

[OH-]=10^-2.7

=2*10^-3 M

E)let the molarity be m.so equating the number of moles,

12*m=20.5*0.55

or m=0.939 M

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