Question

The pH of a solution of Ba(OH)2 is 12.99 at 25

The pH of a solution of Ba(OH)2 is 12.99 at 25

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

pH of barium hydroxide is given 12.99, however the [OH-] is also given as 9.8x 10-2.

Since one molecule of barium hydroxide gives 2 moles of OH- ions [Ba(OH)2] = 4.9 x 10-2M

We have the relation of molarity to weight of substance as

                M = (w .1000)/( Molar massxvolume of solution)

Substituting the values, M = 4.9 x 10-2 , molar mass = 171g/mol, volume =120mL we get

Weight of Ba(OH)2 = 1.0055g

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
12 - Assuming complete dissociation, what is the pH of a 3.10 mg/L Ba(OH)2 solution? 14-...
12 - Assuming complete dissociation, what is the pH of a 3.10 mg/L Ba(OH)2 solution? 14- At 25 °C, how many dissociated OH– ions are there in 1227 mL of an aqueous solution whose pH is 1.97?
18. Calculate the pH of a 0.027 M Ba(OH)2 solution. pH = Enter your answer in...
18. Calculate the pH of a 0.027 M Ba(OH)2 solution. pH = Enter your answer in the provided box. How much NaOH (in grams) is needed to prepare 681 mL of solution with a pH of 9.570? g NaOH
Assuming complete dissociation, what is the pH of a 4.56 mg/L Ba(OH)2 solution?
Assuming complete dissociation, what is the pH of a 4.56 mg/L Ba(OH)2 solution?
Assuming complete dissociation, what is the pH of a 4.67 mg/L Ba(OH)2 solution?
Assuming complete dissociation, what is the pH of a 4.67 mg/L Ba(OH)2 solution?
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
What is the pH of a solution prepared by mixing 43 mL of 0.050 M Ba(OH)2...
What is the pH of a solution prepared by mixing 43 mL of 0.050 M Ba(OH)2 and 38 mL of 0.35 M KOH?
The solubility rules say that Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble hydroxides. Calculate the pH...
The solubility rules say that Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble hydroxides. Calculate the pH of a saturated solution of Sr(OH)2. Ksp = 4.4 x10-4 for Sr(OH)2.
What is the pH of a solution that results from adding 0.053 mol Ba(OH)2 (s) to...
What is the pH of a solution that results from adding 0.053 mol Ba(OH)2 (s) to 1.57 L of a buffer comprised of 0.31 M HF and 0.31 M NaF? its not 3.40
A 100.0mL sample of 0.10M Ba(OH)2 is titrated with 0.10M HCl. determine the PH of the...
A 100.0mL sample of 0.10M Ba(OH)2 is titrated with 0.10M HCl. determine the PH of the solution after the addition of 100.0mL HCl
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