In a lab project, a student obtained a colored basic solution whose concentration has to bedetermined. The student wants to perform a titration but he does not know which indicator hecan use. Can he perform a titration without an indicator? Which method can he use todetermine the concentration and why?

If the basic solution changes its color due to neutralization by addition of acid in titration at…

Answered: In a lab project, a student obtained a…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Similar questions

if a substance changes color at a higher ph but acids neutralize at a lower ph, would that affect the results of an experiment?
Use the References to acces Which of the following aqueous solutions are good buffer systems? 0.27 M ammonium bromide + 0.37 M ammonia O 0.12 M acetic acid + 0.20 M sodium acetate 0.25 M hydrochloric acid + 0.24 M sodium chloride O 0.15 M sodium fluoride + 0.21 M hydrofluoric acid O 0.39 M hydrocyanic acid + 0.29 M sodium cyanide
Some soluble compounds are listed in the table below. Complete the table by filling in the name or chemical formula of each compound, whichever is missing. (If there is more than one way to name the compound, choose the name used when the compound is dissolved in water.) Also classify the compound using the checkboxes. compound 0 HCH₂ CO₂ NH3 HCIO4 name barium hydroxide 0 0 type of compound (check all that apply) strong weak strong weak acid base base acid ionic molecular 0 0 0 0 X S
What's a definition of "Titration"
A 0.398 g sample of KHP will be titrated with a NaOH solution with an assumed concentration of 0.100 M. Calculate the volume of NaOH that should neutralize the KHP sample. volume: mL
At the beginning of a titration, the acetic acid burette reads 0.30 mL. At the end of the titration. thé burette reads 27.70 mL. What volume had been added to the flask? Answer to two places past the decimal.
Scenario Titration Analysis Use scenario to answer the following question:
I have a 50.0 mL sample of a solution of hydrocyanic acid, HCN, of unknown concentration. I titrate the HCN solution with a stock solution of 10.0 M NaOH. I reach endpoint when 6.50 mL of LIOH solution have been added. What is the original concentration of my HCN solution?
What are the stock solutions? Give some examples?
25.0 mL of a weak base is titrated with 0.708 M solution of HCl. The equivalence point is reached when 13.0 mL of HCl is added. What is the concentration of the original 25.0 mL weak base solution?
Recognizing common acids and bases Some soluble compounds are listed in the table below. Complete the table by filling in the name or chemical formula of each compound, whichever is missing. (If there is more than one way to name the compound, choose the name used when the compound is dissolved in water.) Also classify the compound using the checkboxes. compound 0 KOH 0 name acetic acid ammonia 0 sodium perchlorate type of compound (check all that apply) strong weak strong weak acid acid base base ionic molecular 000 O On
A 1.0 g sample of an unknown substance was titrated with a 0.1 M HCl solution (Figure 1). Another 1.0 g sample of it was titrated with a 0.1 M NaOH solution (Figure 2). Given the following possibilities, what is the sample? A. Na2CO3 B. NaHCO3 C. H2CO3 D. KOH E. HNO2

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