Question

Calculate [H+] for each of the following solutions A) [OH−]= 3.9×10−4 M B) [OH−]= 8.3×10−9 M...

Calculate [H+] for each of the following solutions

A) [OH−]= 3.9×10−4 M

B) [OH−]= 8.3×10−9 M

C) A solution in which [OH−] is 140 times greater than [H+]

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

the H+ ion concnetration is can be calculate as fololows

a) [H+] = Kw / [OH-]

[H+] = 1.0*10-14 / [OH-]

[H+] = 1.0*10-14 / 3.9*10-4

        = 2.564*10-11 M

b) [H+] = 1.0*10-14 / [OH-]

     [H+] = 1.0*10-14 /8.3*10-9

                 = 1.2048*10-6 M

c) OH- is 140 times greater so [OH-] = 140 [H+]

   so 1.0*10-14 = [H+] * 140 [H+]

=> [H+]2 = 1.0*10-14 / 140

=> [H+] = 8.45*10-9 M

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
Part D Indicate whether the solution is acidic, basic, or neutral. [OH−]=8.5×10−9 M [OH−]=3.7×10−4 M Solution...
Part D Indicate whether the solution is acidic, basic, or neutral. [OH−]=8.5×10−9 M [OH−]=3.7×10−4 M Solution in which [OH−] is 100 times greater than [H+].
#26. Calculate [OH -] and pH for each of the following solutions. (a) 0.0057 M KOH...
#26. Calculate [OH -] and pH for each of the following solutions. (a) 0.0057 M KOH [OH-] = ___ M pH =___ (b) 0.0476 g of KOH in 490.0 mL of solution [OH -] =___ M pH = ___ (c) 11.0 mL of 0.00474 M Sr(OH)2 diluted to 700 mL [OH -] = ___ M pH =___ (d) A solution formed by mixing 13.0 mL of 0.000730 M Sr(OH)2 with 27.0 mL of 1.3 x 10-3 M KOH [OH -]...
[H+]= 5.5×10−3M . Express the molarity to two significant digits. [OH−] =   M   SubmitMy AnswersGive Up...
[H+]= 5.5×10−3M . Express the molarity to two significant digits. [OH−] =   M   SubmitMy AnswersGive Up Part B [H+]= 1.5×10−9M . Express the molarity to two significant digits. [OH−] =   M   SubmitMy AnswersGive Up Part C A solution in which [H+] is 1000 times greater than [OH−]. Express the molarity to two significant digits. [OH−] =   M   SubmitMy AnswersGive Up
Calculate the pH and pOH in each of the following aqueous solutions. In each case, indicate...
Calculate the pH and pOH in each of the following aqueous solutions. In each case, indicate whether the solution is acidic or basic. a) [OH-] = 1.33 x 10-8 M b) [OH-] = 1.06 x 10-9 M
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 .
9.35 Determine the pH of water solutions with the following characteristics. Classify each solution as acidic,...
9.35 Determine the pH of water solutions with the following characteristics. Classify each solution as acidic, basic, or neutral. a) [H+] = 1.0 x10-4 M b) [OH-] = 5.0 x10-2 M c) [H+] = [OH-] d) [H+] = 8.0 x10-9 M e) [OH-] = 4.0 x10-10 M
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
1. What is the pH of the following solutions? 0.65M HNO3 0.0205 M Ba(OH)2 3.Calculate the...
1. What is the pH of the following solutions? 0.65M HNO3 0.0205 M Ba(OH)2 3.Calculate the [OH -] for the solutions with a pH of 10.82. Is the solution acidic, basic, or neutral? 4. A student is to dissolve 8.75g of Sr(OH)2 in enough water to get a pH of 13.35. What should the final volume be? 5.Which of the following is the strongest acid? Acid pOH HA 8.71 HB 9.21 HC 3.17 HD 4.29 HE 7.00 6. Label each...
For each of the following strong base solutions, determine [OH−],[H3O+] pH , pOH A)8.71×10−3 M LiOH...
For each of the following strong base solutions, determine [OH−],[H3O+] pH , pOH A)8.71×10−3 M LiOH B)1.15×10−2 M Ba(OH)2 C) 1.9×10−4 M KOH D) 4.9×10−4 M Ca(OH)2
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
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT