Question

A sample of sodium carbonate unknown is dissolved in 50.0 mL of water. After performing experiment...

A sample of sodium carbonate unknown is dissolved in 50.0 mL of water. After performing experiment 3, student determines that the second equivalence point occurs at 32.86 mL of 0.1115 M HCl. What is the theoretical pH of the solution at the second equivalence point? Report your answer to two significant figures.

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
A 0.872 gram sample of an unknown monoprotic acid is dissolved in 50.0 mL of water...
A 0.872 gram sample of an unknown monoprotic acid is dissolved in 50.0 mL of water and titrated with a a 0.424 M aqueous sodium hydroxide solution. It is observed that after 9.40 milliliters of sodium hydroxide have been added, the pH is 3.350 and that an additional 5.50 mL of the sodium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol (2) What is the value of Ka for...
A 1.26 gram sample of an unknown monoprotic acid is dissolved in 50.0 mL of water...
A 1.26 gram sample of an unknown monoprotic acid is dissolved in 50.0 mL of water and titrated with a a 0.306 M aqueous potassium hydroxide solution. It is observed that after 12.7 milliliters of potassium hydroxide have been added, the pH is 3.193 and that an additional 19.3 mL of the potassium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? ____ g/mol (2) What is the value of Ka...
After performing Experiment 3, you have determined that your second equivalence point occurred after adding 42.50...
After performing Experiment 3, you have determined that your second equivalence point occurred after adding 42.50 mL of 0.1000 M HCl. Assuming that you dissolved your unknown sample in 150.00 mL of water, calculate the concentration of all species in solution AND the pH of the solution after 30.00 mL of HCl has been added? (Note: Kw = 1.00 x 10-14, Ka1= 4.44 x 10-7 and Ka2 = 4.69 x 10-11)
a. A student dissolves 1.1007 grams of their KHP unknown in 50.0 mL of water. The...
a. A student dissolves 1.1007 grams of their KHP unknown in 50.0 mL of water. The molarity of the student’s NaOH titrant is 0.0999 M. If it takes 40.25 mL of the sodium hydroxide titrant to reach the equivalence point, what is the wt% KHP (MW=204.23) in the unknown? b. If the student uses 55.0 mL of water instead of 50.0 mL to dissolve the unknown, what affect, if any, does this have on the calculated weight % of the...
The pKa of hypochlorous acid is 7.530. A 50.0 mL solution of 0.142 M sodium hypochlorite...
The pKa of hypochlorous acid is 7.530. A 50.0 mL solution of 0.142 M sodium hypochlorite (NaOCl) is titrated with 0.338 M HCl. Calculate the pH of the solution: a) after the addition of 7.12 mL of 0.338 M HCl. b) after the addition of 21.8 mL of 0.338 M HCl. c) at the equivalence point with 0.338 M HCl.
A 0.4016 g sample of impure sodium carbonate (soda ash) is dissolved in 50 mL of...
A 0.4016 g sample of impure sodium carbonate (soda ash) is dissolved in 50 mL of distilled water. Phenolphthalein was added and 11.40 mL of 0.09942 M HCL was required to reach the first end point. Excess volume of HCL was added according to the lab procedure (if x is the amount of acid needed to complete the first titration, you will add a total of 2x + 10mL of acid to ensure excess). After boiling, the excess acid was...
A 1.54 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water...
A 1.54 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.225 M aqueous potassium hydroxide solution. It is observed that after 19.3 milliliters of potassium hydroxide have been added, the pH is 7.171 and that an additional 34.5 mL of the potassium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid?  g/mol (2) What is the value of Ka for the...
A 1.22 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water...
A 1.22 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water and titrated with a a 0.299 M aqueous potassium hydroxide solution. It is observed that after 10.4 milliliters of potassium hydroxide have been added, the pH is 3.039 and that an additional 19.4 mL of the potassium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol (2) What is the value of Ka for...
An experiment was to identify the unknown solution as sodium carbonate or sodium bicarbonate by reacting...
An experiment was to identify the unknown solution as sodium carbonate or sodium bicarbonate by reacting it with HCl and taking pressure measurements. My chemical equations are: NaHCO3+HCl--->CO2+H2O+NaCl Na2CO3+2HCl--->CO2+H2O+2NaCl. The instructor said that it can be determined by looking at the chemical equation. My response was the pressure measurements were from the unknown were closer to sodium bicarbonate than sodium carbonate. Is this a correct assumption?
120 mg of morphine are dissolved in 20.0 mL water. This solution is titrated with 0.0225...
120 mg of morphine are dissolved in 20.0 mL water. This solution is titrated with 0.0225 M HCl. Calculate the pH at the equivalence point of the titration
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT