Use the following information as a guide to help answer the next three questions. Your answer MUST be in the same format. Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between 6.0 and 7.6 Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Using the method outlined above in the example of bromothymol blue, indicate what the colours of the indicators tell us about the pH approximation of the solution. Values and wording are very important, so be precise. Be sure to word your pH approximation as outlined in the example. Indicator Colour pH approximation methyl red orange Indicator Colour pH approximation phenolphthalein colourless Indicator Colour pH approximation phenol red red

Use the following information as a guide to help answer the next three questions. Your answer MUST be in the same format. Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between 6.0 and 7.6 Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Using the method outlined above in the example of bromothymol blue, indicate what the colours of the indicators tell us about the pH approximation of the solution. Values and wording are very important, so be precise. Be sure to word your pH approximation as outlined in the example. Indicator Colour pH approximation methyl red orange Indicator Colour pH approximation phenolphthalein colourless Indicator Colour pH approximation phenol red red

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...

See similar textbooks

Similar questions

The indicator phenol red changes from yellow to red between pH 6.8 and pH 8.4. If phenol is red added to a solution, and the solution turns red then A.) The solution is basic and the pH must be at or below 7.0. B.) The pH of the solution must be below 6.8, and the solution is basic. C.) The pH of the solution must be below 6.8, and the solution is acidic. D.) The pH of the solution must be above 8.4, and the solution is basic E.) The pH of the solution is above 8.4, and the solution is acidic.
What is buffer capacity, and when it is largest
Calculate the pH of the resulting solution if 34.0mL of 0.340 M HCl (aq) is added to 44.0 mL of 0.390 M NaOH (aq) . Please show steps to solve, formulas utilized and any other applicable changes. I'm not sure what I am doing wrong and want to see how to get to the solution correctly. Will thumbs up! Thanks.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
A 0.1-L unbuffered solution needs the pH adjusted from 4 to 1. How many microliters of a 12 molar HCl solution need to be added to adjust the pH? Report your answer to four decimal places. For this question: Assume the volume of HCl being added is negligible and the total volume of the solution does not change. The volume of the solution is *not* 1 L like it was in the practice pools. The question requests your answer be reported in μL (microliters)!!
I need the answer as soon as possible
Suppose a 0.14 M aqueous solution of oxalic acid (H₂C₂O₂) is prepared. Calculate the equilibrium molarity of CO,. You'll find information on the properties. of oxalic acid in the ALEKS Data resource. Round your answer to 2 significant digits. M D.P X S
An unknown solution is blue with indigo carmine and blue with thymolphthalein. From that information, predict the approximate pH range of the unknown solution, then determine the colour of the following indicators in that solution. Indicator Colour alizarin yellow R yellow/red/orange phenolphthalein colourless/pink thymol blue yellow/red/orange/green/blue
A student is asked to design an experiment that uses indicators to identify which of three unknown solutions labelled X, Y, and Z have pH values of 1.3, 5.7, and 6.9. The student must select a maximum of four indicators from the following list to perform the experiment. 1. orange IV 2. phenolphthalein 3. bromocresol green 4. alizarin yellow R 5. bromothymol blue 6. chlorophenol red 7. cresol red 8. indigo carmine The indicators that will allow the student to identify successfully the pH of the unknown solutions are and List the numbers from lowest to highest.
Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between 6.0 and 7.6 Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Indicator Colour pH approximation orange IV orange Indicator Colour pH approximation thymol blue red Indicator Colour pH approximation alizarin yellow R red
If the total concentration of a buffer is known (and not the individual concentrations of the weak acid and its conjugate base), can the pH be calculated?
At the equivalence point, all of the acid has been neutralized by the base. Why does the pH change so sharply around the equivalence point?