Question

Calculate the [H+] and the pH of a solution with an [OH−]=0.054 M at 25 °C...

Calculate the [H+] and the pH of a solution with an [OH−]=0.054 M at 25 °C .

[H+]= M

pH=

Calculate the [H+] and the [OH−] of a solution with a pH=1.07 at 25 °C .

[H+]= M [

OH−]= M

Homework Answers

Answer #2

answered by: anonymous
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the [H+] and the [OH−] of a solution with a pH=11.45 at 25 °C ....
Calculate the [H+] and the [OH−] of a solution with a pH=11.45 at 25 °C . calculate the [H+][H+] and the pH of a solution with an [OH−]=0.0063 M at 25 °C. Calculate the [ OH − ] [OH−] and the pH pH of a solution with an [ H + ]=9.3× 10 −13 M [H+]=9.3×10−13 M at 25 °C
The pH of a very concentrated solution of a base M(OH)2 at 25 degree C is...
The pH of a very concentrated solution of a base M(OH)2 at 25 degree C is 15.00. What is the molarity of this solution in M(OH)2?
For each of the following solutions, calculate the pH, pOH, [H3O+], and [OH-] at 25⁰C. A...
For each of the following solutions, calculate the pH, pOH, [H3O+], and [OH-] at 25⁰C. A solution of 0.047 M LiOH A solution of 0.0011 M HNO3 A solution with a pH of 9.12 A solution of 0.010 M HClO3
Calculate [H ], [ClO4–], and [OH–] in an aqueous solution that is 0.135 M in HClO4(aq)...
Calculate [H ], [ClO4–], and [OH–] in an aqueous solution that is 0.135 M in HClO4(aq) at 25 °C. H^+ = ClO-4 = OH- = Is the solution acidic basic or neutral?
Part A Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 4.3×10−4 M ....
Part A Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 4.3×10−4 M . Part B Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 1.6×10−12 M . Part C Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 3.0×10−2 M .
Calculate the [H+] and [OH-] in each of the following aqueous solutions. solution           [H+]           ...
Calculate the [H+] and [OH-] in each of the following aqueous solutions. solution           [H+]            [OH-]          acidic/basic a) pH = 9.21 b) pOH = 14 c) pH = 11.58 d) pOH = 8.37 e) pH = 9.33 f) pH = 6.04
There are four aqueous solutions at 25 degrees celsius. Solution A Given [H+] = 1.3 x...
There are four aqueous solutions at 25 degrees celsius. Solution A Given [H+] = 1.3 x 10-9 M, find [OH-], pH, and pOH. Solution B Given [OH-] = 0.098 M, find [H+], pH, and pOH. Solution C Given pH = 8.16, find [H+], [OH-], and pOH. Solution D Given pOH = 1.03, find [H+], [OH-], and pH.
Calculate [H3O^-], [ClO4^-], and [OH^-] in an aqueous solution that is 0.165 M in HClO4(aq) at...
Calculate [H3O^-], [ClO4^-], and [OH^-] in an aqueous solution that is 0.165 M in HClO4(aq) at 25 degree C. [H^+]= ???? M [ClO4^-]= ??? M [OH^-]= ???? M Is the solution acidic, basic or neutral?
1.Calculate the pH of an 0.0452 M Ba(OH)2 solution at 298 K 2. calculate the pH...
1.Calculate the pH of an 0.0452 M Ba(OH)2 solution at 298 K 2. calculate the pH of an 0.229 M HNO2 solution at 298 K. Assume ka for HNO2 is 4.5x10^-4 3.Calculate the pH of an 0.292 M NH3 solution at 298 K. assume the Kb for NH3 is 1.8x10^-5
Calculate the pH at 25° C of a 0.055 M solution of a weak acid that...
Calculate the pH at 25° C of a 0.055 M solution of a weak acid that has Ka = 1.4 × 10−5.