Question

what is the molarity of 10.0mL Ba(OH)2 which can be completely neutralized by 25.0ml of 0.100M...

what is the molarity of 10.0mL Ba(OH)2 which can be completely neutralized by 25.0ml of 0.100M HCl?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
The volume of 0.300 mol/L HCl that can be completely neutralized by 2.00 g of Ca(OH)2...
The volume of 0.300 mol/L HCl that can be completely neutralized by 2.00 g of Ca(OH)2 in a stomach antacid tablet is? Please help me show the work.
How many milliliters of .405 Ba(OH)2 solution are required to completely react with 17.5 milliliters of...
How many milliliters of .405 Ba(OH)2 solution are required to completely react with 17.5 milliliters of .244M HCl according to the balanced chemical equation? (your answer should have 3 significant figures and not include units) 2 HCl + Ba(OH)2 --> 2 H2O + BaCl2
if 16.9 mL of an acetic acid (HC2H3O2) solution are completely neutralized by 22.4 mL of...
if 16.9 mL of an acetic acid (HC2H3O2) solution are completely neutralized by 22.4 mL of 0.464 M Ba(OH)2 . a. what is the molarity of the HC2H3O2? and b.what is the molar concentration of barium ion in the resulting solution? for a I have 0.615 M of HC2H3O2 and for b I havr 20.1 M but I think its off. please help
What is the molarity of an aqueous phosphoric acid solution if 10.33 mL is completely neutralized...
What is the molarity of an aqueous phosphoric acid solution if 10.33 mL is completely neutralized by 17.24 mL of 0.1301 M NaOH? First, calculate the moles of H3PO4 at the dilution based on the volume and molarity of NaOH used.
A flask contains 0.015 mol of HCL in 10.0mL of solution. What is the molarity of...
A flask contains 0.015 mol of HCL in 10.0mL of solution. What is the molarity of the HCl solution? In a titration with NaOH, how many moles of NaOH will be required to reach the end point? If 12.5 mL of NaOH are required to reach the end point, what is the molarity of the NaOH solution? What must be added to the HCl solution in order to observe the end point?
If 0.00300 mol NaOH and 0.00300 mol Ba(OH)2 are completely dissolved in water to make1.00 L...
If 0.00300 mol NaOH and 0.00300 mol Ba(OH)2 are completely dissolved in water to make1.00 L of solution at 25oC, what is the pOH of the solution?
A solution is made by dissolving 15.1 g of barium hydroxide, Ba(OH)2, in enough water to...
A solution is made by dissolving 15.1 g of barium hydroxide, Ba(OH)2, in enough water to make exactly 100. mL of solution. Calculate the molarity of each species: Ba(OH)2 _______ mol/L Ba2+ _________ mol/L OH- _________ mol/L
91.2 mL of 0.120 M HCl is mixed with 50.0 mL of 0.101 M Ba(OH)2 solution....
91.2 mL of 0.120 M HCl is mixed with 50.0 mL of 0.101 M Ba(OH)2 solution. 2 HCl(aq) + 1 Ba(OH)2(aq) →   1 BaCl2(aq) + 2 H2O(l) What amount of hydronium ion (in mole) would be present at the end of the reaction?
In a constant‑pressure calorimeter, 65.0 mL65.0 mL of 0.320 M Ba(OH)20.320 M Ba(OH)2 was added to...
In a constant‑pressure calorimeter, 65.0 mL65.0 mL of 0.320 M Ba(OH)20.320 M Ba(OH)2 was added to 65.0 mL65.0 mL of 0.640 M HCl.0.640 M HCl. The reaction caused the temperature of the solution to rise from 21.87 ∘C21.87 ∘C to 26.23 ∘C.26.23 ∘C. If the solution has the same density and specific heat as water (1.00 g/mL1.00 g/mL and 4.184J/g⋅°C,)4.184J/g⋅°C,) respectively), what is Δ?ΔH for this reaction (per mole H2OH2O produced)? Assume that the total volume is the sum of...
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
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT