Question

a- 10 mL of gastric juice sample (HCl) has been taken from a patient and placed...

a- 10 mL of gastric juice sample (HCl) has been taken from a patient and placed in an erlenmeyer flask. After the addition of 50 mL of distilled water the sample was titrated with 1M NaOH solution. If 13 mL of NaOH is required to reach the endpoint of the titration what is the pH of the sample?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

I am hereby attaching your answer in image i hope it will help you please share your views in comment box and gives a thumbs up thank you

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 20.0 mL sample of gastric juice was taken from a patient suspected of having hypochloridia...
A 20.0 mL sample of gastric juice was taken from a patient suspected of having hypochloridia (low stomach acid). The sample was taken several hours after a meal so there was no ingested food or drink, and it was assumed no buffers were present. The sample required 4.7 mL of 0.0019 M NaOH to titrate the sample to neutrality. What was the pH of the gastric juice?
You are given a sulfuric acid solution of unknown concentration. You dispense 10.00 mL of the...
You are given a sulfuric acid solution of unknown concentration. You dispense 10.00 mL of the unknown solution into an Erlenmeyer flask and add 12.20 mL of distilled water and a drop of phenopthalein to the flask. You fill your buret with 0.103 M NaOH (aq) solution and begin the titration. During the titration you rinse the tip and the sides of the Erlenmeyer flask with 3.52 mL of distilled water. It requires 10.38 mL of your NaOH (aq) solution...
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH....
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH. To reach the endpoint of the titration, 30.00 mL of NaOH solution is required. Ka = 1.8 x 10-4 What is the pH of the solution after the addition of 10.00 mL of NaOH solution? What is the pH at the midpoint of the titration? What is the pH at the equivalence point?
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 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH....
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH. To reach the endpoint of the titration, 30.00 mL of NaOH solution is required. Ka = 1.8 x 10-4 What is the concentration of formic acid in the original solution? What is the pH of the formic acid solution before the titration begins (before the addition of any NaOH)?
10 mL of 0.10 M HCl is being titrated with 0.10 M NaOH. What would the...
10 mL of 0.10 M HCl is being titrated with 0.10 M NaOH. What would the pH of the solution be after addition of a) 1.0 mL of NaOH and b) 9.0 mL of NaOH
A 46.3 mL sample of a 0.380 M solution of NaCN is titrated by 0.350 M...
A 46.3 mL sample of a 0.380 M solution of NaCN is titrated by 0.350 M HCl. Kb for CN- is 2.0×10-5. Calculate the pH of the solution: (a) prior to the start of the titration pH = (b) after the addition of 25.1 mL of 0.350 M HCl pH = (c) at the equivalence point pH = (d) after the addition of 71.9 mL of 0.350 M HCl. pH =
A 44.9 mL sample of a 0.350 M solution of NaCN is titrated by 0.260 M...
A 44.9 mL sample of a 0.350 M solution of NaCN is titrated by 0.260 M HCl. Kb for CN- is 2.0×10-5. Calculate the pH of the solution: (a) prior to the start of the titration pH = (b) after the addition of 48.4 mL of 0.260 M HCl pH = (c) at the equivalence point pH = (d) after the addition of 76.2 mL of 0.260 M HCl. pH =
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 student determines the acetic acid concentration of a sample of distilled vinegar by titration of...
A student determines the acetic acid concentration of a sample of distilled vinegar by titration of 25.00 mL of the vinegar with standardized sodium hydroxide solution using phenolphthalein as an indicator. Which error will give an acetic acid content for the vinegar that is too low? (A) Some of the vinegar is spilled when being transferred from the volumetric flask to the titration flask. (B) The NaOH solution is allowed to stand for a prolonged period after standardization and absorbs...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT