ZuoTi.Pro
Question

concentration if the following errors occurred: Explain the effect on your calculated acid concentration nel in the buret dur
science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

The base is generally taken in the burette during an acid base titration. If the buret funnel used is left in the burette then any droplets on the funnel will drop into the burette during the titration. as a result, the volume of base used will be low and thus concentration of acid calculate will be low than the actual value.

Formula is N1V1=N2V2

If the burette used contains air bubbles, then the volume used to get end point will be high than the actual volume. As the volume of base is high, the concentration of acid calculated will be high than the actual concentration value.

If the acid is diluted, it's concentration will decrease.

If the flask is wet, means it contain water droplets. If water is present, dilution occurs that is concentration of acid decreases.

0 0
Add a comment
Know the answer?
Add Answer to:
concentration if the following errors occurred: Explain the effect on your calculated acid concentration nel in...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • POST-LAB QUESTIONS Explain the effect on your calculated acid concentration if the following errors occurred 1....

    POST-LAB QUESTIONS Explain the effect on your calculated acid concentration if the following errors occurred 1. A student left his or her buret funnel in the buret during the titration. 2. A student started their titration with air bubbles in the buret tip. 3. The dilute HCl was over-diluted in the volumetric flask. 4. The flask that the student added the dilute acid to before the titration was wet. Titration of an unknown Acid

  • explain the effect of each of thes following sources of error on the molarity of acetic...

    explain the effect of each of thes following sources of error on the molarity of acetic acid as determined in this experiment stating whether the concentration of acetic acid obtained would be too high or too low. a. The buret is contaminated with an acid solution b. The buret contains a larger air bubble in the tip, which disappears in the course of a titration. c. A small volume of the acid solution is spilled when you transfer it into...

  • Concentration of NaOH = 1600 x10- Molar Sodium hydroxide Nach Trial 1 Trial 2 Trial Trial 4 2.60/1.20 1...

    Concentration of NaOH = 1600 x10- Molar Sodium hydroxide Nach Trial 1 Trial 2 Trial Trial 4 2.60/1.20 11.40/1.30 28.20 29.10.26.1026.50 Initial buret reading Final buret reading Volume of NaOH added Moles of NaOH added Moles of HCl reacted Molarity of diluted HCI Molarity of undiluted HCI Average molarity of undiluted HCI Precision PROCEDURE 1. Obtain approximately 40 mL of an unknown acid in an Erlenmeyer flask from your teaching assistant. 2. Clean your 250-ml volumetric flask (contains exactly 250.00...

  • Concentration of NaOH = 1600 x10- Molar Sodium hydroxide Nach Trial 1 Trial 2 Trial Trial...

    Concentration of NaOH = 1600 x10- Molar Sodium hydroxide Nach Trial 1 Trial 2 Trial Trial 4 2.60/1.20 1.40/1.30 28.20 29.10.26.1026.50 Volume of NaOH added Initial buret reading Final buret reading Moles of NaOH added Moles of HCl reacted Molarity of diluted HCI Molarity of undiluted HCI Average molarity of undiluted HCI Precision PROCEDURE 1. Obtain approximately 40 mL of an unknown acid in an Erlenmeyer flask from your teaching assistant. 2. Clean your 250-ml volumetric flask (contains exactly 250.00...

  • Is the calculated concentration for IO3- in the data table correct, and if not, how do I calculat...

    Is the calculated concentration for IO3- in the data table correct, and if not, how do I calculate it. Also, the questions below the data table in the second picture. How are they calculated? 2. The molar solubility of Cal(IO3)2 in pure water Temperature of the saturated solution of calcium iodate: Volume (or mass) of saturated calcium iodate solution titrated:O -24 °C ted:1 Q mL (or g) Data Trial 1 Trial 2 Trial 3 Volume of Na2S203 titrant Final buret...

  • 1. A student carries out a back titration to determine the concentration of ammonium chloride in a solution. The student...

    1. A student carries out a back titration to determine the concentration of ammonium chloride in a solution. The student collects 10.80 mL of the original NH4Cl solution and dilutes it to 250.0 mL (we will refer to this as the dilute NH4Cl solution). Then 25.00 mL of the dilute NH4Cl solution are transferred to an Erlenmeyer flask and 25.00 mL of 0.1963 M NaOH are added. Calculate the moles of NaOH added to this Erlenmeyer flask. 2. In the...

  • For vinegar titration in this experiment, would the following errors cause the % acetic acid in vinegar determined to be...

    For vinegar titration in this experiment, would the following errors cause the % acetic acid in vinegar determined to be (A) too large, (B) too small, (C) no effect, or (D) not enough information to answer. Assume that the mistake given is the only mistake made in the experiment. EXPLAIN. 1.) The burst is rinsed with distilled water, but not NaOH solution before the vinegar sample is titrated. 2.) After standardization, the NaOH solution is not stoppered and obsorbs CO2...

  • I need it right now, please help me?? PROCEDURE PART I: DILUTING THE VINEGAR SOLUTION The...

    I need it right now, please help me?? PROCEDURE PART I: DILUTING THE VINEGAR SOLUTION The vinegar solution must be diluted by a factor of 5 to be suitable for titration. 1. Obtain - 20 ml of the stock vinegar solution from the fume hood. 2. Using the 10-ml. pipet, pipet" 10 mL of the stock solution to a 50-ml volumetric flask. 3. Fill the volumetric flask to the calibration line with distilled water. Be sure not to go over...

  • What effect on your calculated yield would the following experimental errors have had? A) Incomplete evaporation...

    What effect on your calculated yield would the following experimental errors have had? A) Incomplete evaporation of the excess hydrochloric acid B) Excessive heating of the product to cause decomposition (say to manganese(II) oxide) C) Cooling the product in the open air (especially on a humid day) D) Which of the above errors are the most probable? Experiment: Manganese sample is dissolved in concentrated HCl, exess HCl and water will be evaporated to obtain solid manganese(II) chloride.

  • ALL THE INFO YOU NEED IS BELOW average volume of NaOH: 15.7 mL or 0.0157 L...

    ALL THE INFO YOU NEED IS BELOW average volume of NaOH: 15.7 mL or 0.0157 L average number of moles of NaOH added: 6.28*10-4 moles molar concentration of [HT] in saturated solution(HT– acts as a monoprotic acid, reacting with NaOH in a 1:1 ratio (Volume of KHT measured using 25.00 mL volumetric pipet.)): 0.2512 M Analysis of KHT in water 1. Weigh out 0.8 grams of potassium hydrogen tartrate (KHT) on weighing paper. Add the KHT to a clean dry...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT