Part A If the pH of the solution is 9.5, what is the [H3O+]? Express your answer
ID: 1006161 • Letter: P
Question
Part A If the pH of the solution is 9.5, what is the [H3O+]? Express your answer to one significant figure. Part B If the pH of the solution is 9.5, what is the [OH]? Express your answer to one significant figure. Part C If the solution is neutral, what is the [H3O+]? Express your answer to one significant figure. Part D If the solution is neutral, what is the [OH]? Express your answer to one significant figure. Part E If the solution is neutral what is the value of pH? Express your answer using one decimal place. If the [OH] in a solution is 2×105M, what is the [H3O+]? Express your answer to one significant figure. Part G If the [OH] in a solution is 2×105M, what is the pH of the solution? Express your answer using one decimal place. If the [H3O+] in a solution is 1×102M, what is the [OH]? Express your answer to one significant figure. Part I If the [H3O+] in a solution is 1×102M, what is the pH? Express your answer using one decimal place Part J If the pH of the solution is 11.8, what is the [H3O+]? Express your answer to one significant figure. Part K If the pH of the solution is 11.8, what is the [OH]? Express your answer to one significant figure.
Explanation / Answer
Part A If the pH of the solution is 9.5, what is the [H3O+]? Express your answer to one significant figure.
pH = - log [H+]
[H+]= 10^-pH
= 3.0*10^-10
Part B If the pH of the solution is 9.5, what is the [OH]? Express your answer to one significant figure.
pH + pOH = 14
pOH = 14-9.5=4.5
pOH = - log [OH-]
[OH-]= 10^-pOH
= 3.0*10^-5
Part C If the solution is neutral, what is the [H3O+]? Express your answer to one significant figure.
In neutral solution; the [H3O+] = 1.0*10^-7
Part D If the solution is neutral, what is the [OH]? Express your answer to one significant figure.
In neutral solution; the [OH-] = 1.0*10^-7
Part E If the solution is neutral what is the value of pH? Express your answer using one decimal place.
In neutral solution; the [H3O+] = 1.0*10^-7
pH = - log [H+]
pH = 7.0
If the [OH] in a solution is 2×105M, what is the [H3O+]? Express your answer to one significant figure.
[H+][OH-]= 1.0*10^-14
[H+]2×105M = 1.0*10^-14
[H+]= 5*10^-10
Part G If the [OH] in a solution is 2×105M, what is the pH of the solution? Express your answer using one decimal place.
pOH = - log [OH-]
pOH = - log 2×105
= 4.69 OR 5.0
If the [H3O+] in a solution is 1×102M, what is the [OH]? Express your answer to one significant figure.
[H+][OH-]= 1.0*10^-14
1×102M [OH-]= 1.0*10^-14
[OH-]=1.0*10^-12
Part I If the [H3O+] in a solution is 1×102M, what is the pH? Express your answer using one decimal place
pH = - log [H+]
pH = - log 1×102
=2
Part J If the pH of the solution is 11.8, what is the [H3O+]? Express your answer to one significant figure.
pH = - log [H+]
[H+]=10^-pH
=1.58*10^-12
=2*10^-12
Part K If the pH of the solution is 11.8, what is the [OH]? Express your answer to one significant figure.
pH = - log [H+]
[H+]=10^-pH
=1.58*10^-12
=2*10^-12
[H+][OH-]= 1.0*10^-14
2*10^-12 [OH-]= 1.0*10^-14
[OH-]=5.0*10^-3