Students measured the concentration of HCl in a solution by titrating with different indicators to find the end point. (Use the table to find critical F values.)Mean HCl concentration (M)(+ standard deviation)IndicatorNumber of measurements1. Bromothymol blue0.09565 + 0.00170282. Methyl red0.08681 ± 0.00098183. Bromocresol green0.08641 + 0.0010629Is the difference between Indicators 1 and 2 significant at the 95% confidence level?O YesO NoFenlculatedclegrees of freedomEcalculatedIs the difference between indicators 2 and 3 significant at the 95% confidence level?O YesO NoFealculatedSpooledtcalculated

95 % confidence interval for a population mean can be represented as 1. Bromothymol blue, the…

Students measured the concentration of HCl in a solution by titrating with different indicators to find the end point. (Use the table to find critical F values.) Mean HCl concentration (M) (i standard deviation) Indicator Number of measurements 1. Bromothymol blue 0.09565 + 0.00170 28 2. Methyl red 0.08681 1 0.00098 18 3. Bromocresol green 0.08641 + 0.00106 29 Is the difference between Indicators 1 and 2 significant at the 95% confidence level? Yes O No Fealculated degrees of freedom tralculated Is the difference between indicators 2 and 3 significant at the 95% confidence level? Yes

Students measured the concentration of HCl in a solution by titrating with different indicators to find the end point. (Use the table to find critical F values.) Mean HCl concentration (M) (i standard deviation) Indicator Number of measurements 1. Bromothymol blue 0.09565 + 0.00170 28 2. Methyl red 0.08681 1 0.00098 18 3. Bromocresol green 0.08641 + 0.00106 29 Is the difference between Indicators 1 and 2 significant at the 95% confidence level? Yes O No Fealculated degrees of freedom tralculated Is the difference between indicators 2 and 3 significant at the 95% confidence level? Yes

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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Using the table of pH indicators and their respective pKin. Match the best-suited indicator for the following titration scenarios. Note: You do not need to calculate the pH at the equivalence point, an estimation will be sufficient for this question. Indicator Pkin Thymol Blue 1.65 Methyl Red 5.00 Bromothymol 7.30 Blue Phenolphthalein 8.70 0.10 M acetic acid (pKa = 4.74) is titrated with 0.08 M NaOH [ Choose ] 0.10 M HCI is titrated with 0.0993 M NaOH [ Choose ] 0.10 M ammonia (pKb = 4.74) is titrated with 0.12 M HCI [ Choose ]
If you perform this experiment with a titrant of 0.5M NaOH , would you expect your results in Data Table 2 to change or stay the same? Explain the answer.
Why is standard qualitative analysis of water is qualitative rather than quantitative?
Questions 30-35 refer to the same weak acid/strong base (WA/SB) titration. Prior to the beginning of the titration, there were 0.0090 moles of hypobromous acid present in the flask. The Ką of hypobromous acid is 2.8 x 10-9. (Q30) A 30.00 mL solution of 0.300 M hypobromous acid (HBRO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LIOH). What is the initial solution pH (i.e., when 0.00 mL of titrant have been added)?
Bromoscresol purple is an indicator that changes colour over a range of pH = 5.2 to pH = 6.8. What is Ka of bromoscresol purple? Express your answer to one significant figure.
Calculate the number of moles of acetic acid in 100mL of both samples of vinegar accurately titrated. given: NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL 20.0 mL To find the average volume Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3 = 20.3 mL Concentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL = 0.2627 M Concentration of NaOH = Volume of H2SO4 * Concentration of H2SO4Volume of NaOHVolume of H2SO4 * Concentration of H2SO4Volume of NaOH…
Consider the spectrophotometric pH measurement of seawater with the indicator thymol blue illustrated at the opening of this chapter. The blue form of the indicator In22 on page 202 has maximum absorbance at a wavelength of 596 nm (nanometers). The yellow form HIn2 has maximum absorbance at 435 nm. Measurements of absorbance at the two wavelengths allows us to find the ratio [In22]/[HIn2]. How would you use this measurement to find the pH?
We used Phenolphthalein as our indicator. Look up other type of indicator and provide pH range where it changes color.
The following titration data was collected by a students in CH1031. Based on the results, determine the concentration of the aqueous hydrochloric acid. Concentration of NaOH used: 0.25 M Volume of NaOH used: 25.0 mL phenolphthalein Colorless to pale pink Indicator: Endpoint color change: Table 1 Volume of hydrochloric acid Required Burette reading (mL) Trial 1 29.28 1.78 Trial 2 Trial3 36.62 43.98 16.62 Final reading Initial reading Volume HCl used (mL) 9.28
Using the data below please do the calculations in the image attached Both images go together Please please answer super super fast it’s super important
30. Indicate the FALSE statement about pH indicators and their use in titrations: A) A pH indicator suitable for titrations of strong bases with strong acids cannot be used for titrations of strong acids with strong bases. B) pH indicators should be used sparingly (in small amounts) as they are weak acids/ bases, and thus could affect the volume of titrant used. C) An indicator should be selected such that its pKits value matches the equivalence point pH. D) pH indicators all contain at least one acidic group that can be deprotonated to form a differently colored conjugate base. E) The colours of the acid and base forms of a given pH indicator depend on their chemical structures.