Question

Na2CO3 + NaOH titration

Na2CO3 + NaOH titration

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
In a titration of NaOH and Na2CO3 mixture with HCl. Using 2 indicators phenolphthalein and bromocresol...
In a titration of NaOH and Na2CO3 mixture with HCl. Using 2 indicators phenolphthalein and bromocresol green. Why didn’t we use thymol blue instead of phenolphthalein since they have the same ph range
In a chemistry lab, acid-base titration was completed with Na2CO3 being titrated with HCl and HCl...
In a chemistry lab, acid-base titration was completed with Na2CO3 being titrated with HCl and HCl was titrated with NaOH. In one portion, a standard solution was made of an unkown and it was mixed with 40.00 mL of HCl, the indicator used was Phenophtalein and NaOH was added till an endpoint was used. Data: (0.1255 g of unknown + 40.00 mL HCl) was titrated with 15.60 mL NaOH when the end point was reached. Determine the weight percent of...
"A solution that possibly contains NaOH, Na2CO3, or NaHCO3 either alone or in a compatible combination...
"A solution that possibly contains NaOH, Na2CO3, or NaHCO3 either alone or in a compatible combination is analyzed by titration with 0.1202 M HCl. The first titration uses 25.00 mL of the sample solution and requires 15.67 mL of HCl to reach a phenolphthalein end-point. The second titration uses another 25.00 mL portion of the sample and requires 42.13 mL of HCl to reach a bromocresol green end-point. Calculate the number of milligrams of each solute per milliliter of solution....
Write balanced molecular and ionic equations for each. explain AgNO3+NaBr AgNO3+NaOH AgNO3+Na2CO3 Pb(NO3)2+NaBr Pb(NO3)2+Na2SO4 Pb(NO3)2+NaOH Pb(NO3)2+Na2CO3...
Write balanced molecular and ionic equations for each. explain AgNO3+NaBr AgNO3+NaOH AgNO3+Na2CO3 Pb(NO3)2+NaBr Pb(NO3)2+Na2SO4 Pb(NO3)2+NaOH Pb(NO3)2+Na2CO3 Ni(NO3)2+NaOH Ni(NO3)2+Na2CO3
Near the endpoint of the Na2CO3-HCl titration, it is necessary to heat the analyte solution almost...
Near the endpoint of the Na2CO3-HCl titration, it is necessary to heat the analyte solution almost to boiling to remove the _____ produced by the titration reaction. a. bicarbonate ion b. water c. carbon dioxide d. sodium chloride
What solution is more basic and why NaOH, Nh3/h2o, na2co3
What solution is more basic and why NaOH, Nh3/h2o, na2co3
Consider the titration of H3C6H5O7 with NaOH. If it requires 0.00343 mol of NaOH to reach...
Consider the titration of H3C6H5O7 with NaOH. If it requires 0.00343 mol of NaOH to reach the endpoint, and if we had originally placed 16.41 mL of H3C6H5O7 in the Erlenmeyer flask to be analyzed, what is the molarity of the original H3C6H5O7 solution?
You determine the concentration of a solution of HCl by titration with NaOH. The titration reaction...
You determine the concentration of a solution of HCl by titration with NaOH. The titration reaction is: HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq) Using a volumetric pipet, you transfer 10.00 mL of the HCl solution into an Erlenmeyer flask, then dilute it with ~50 mL of water and add 3 drops of phenolphthalein. The endpoint is reached after you have added 44.00 mL of 0.1250 M NaOH solution from a buret. Calculate the molarity of the original HCl solution....
A solution contains both NaHCO3 and Na2CO3. Titration of a 50.00mL portion to a phenolphtalein end...
A solution contains both NaHCO3 and Na2CO3. Titration of a 50.00mL portion to a phenolphtalein end point requires 20.19 mL of 0.1029 M HCl. A second 50.00mL aliquot requires 47.28 mL of the HCl solution when titrated to a bromocresol green end point. Calculate the molar concentration of NaHCO3 in the solution.
Calculate the pH during the titration of 30.0 ml of 0.40M HCl with a 0.20M NaOH...
Calculate the pH during the titration of 30.0 ml of 0.40M HCl with a 0.20M NaOH solution at the following point during the titration. a) 0.00ml of NaOH added millimoles acid initially=__________ Millimoles base added= ___________ pH = ____________ b) 20.0 ml of NaOH added millimoles acid initially=__________ Millimoles base added = ___________ pH = ____________ c)60.0ml NaOH added millimoles acid initially=__________ Millimoles base added = ___________ pH = ____________ d) 65.00ml NaOH added millimoles acid initially=__________ Millimoles base added...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT