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

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #2

answered by: anonymous
0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

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 .
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.
Calculate OH- and pH in a solution in which CH3NH2 is 0.300 M and CH3NH3+ is:...
Calculate OH- and pH in a solution in which CH3NH2 is 0.300 M and CH3NH3+ is: (kb ch3nh2: 4.2 x 10^-4 A). 0.0500 M B). 0.200 M C). 0.300 M D).0.500 M Please show steps.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT