From the list of acid-base indicators below, select the one BEST indicator for a titration with an equivalence point at pH 5.8 (BE CAREFUL--enter indicator name EXACTLY as it appears in table): Indicator Acid color Base color pKa 0.80 Yellow Blue Methyl violet 1.0 Red Yellow Cresol red Malachite green Thymol blue Phloxine Blue-green Yellow 1.3 Yellow 1.7 Red 1.8 Colorless Pink Red Yellow Orange IV Benzopurpurin Methyl yellow Methyl orange Bromophenol blue Congo red Dinitrophenol Alpha-Naphthyl red Bromocresol green Methyl red Ethyl red Azolitmin (litmus) Bromocresol purple Bromothymol blue Nitrophenol Phenol red Thymol blue Phenolphthalein Alizarin yellow R 2.1 2.8 Violet Red 3.3 Red Yellow 3.7 Red Yellow 4.0 Yellow Blue-violet 4.1 Blue Red 4.1 Colorless Yellow 4.3 Red Yellow 4.7 Yellow Blue 5.1 ed Yellow 5.4 Colorless red 5.8 Red Blue 6.3 Yellow Violet 7.0 Yellow Blue 7.2 Colorless Yellow 7.9 Yellow Red 8.9 Yellow blue 9.4 Colorless Red 11.0 Yellow red

From the list of acid-base indicators below, select the one BEST indicator for a titration with an equivalence point at pH 5.8 (BE CAREFUL--enter indicator name EXACTLY as it appears in table): Indicator Acid color Base color pKa 0.80 Yellow Blue Methyl violet 1.0 Red Yellow Cresol red Malachite green Thymol blue Phloxine Blue-green Yellow 1.3 Yellow 1.7 Red 1.8 Colorless Pink Red Yellow Orange IV Benzopurpurin Methyl yellow Methyl orange Bromophenol blue Congo red Dinitrophenol Alpha-Naphthyl red Bromocresol green Methyl red Ethyl red Azolitmin (litmus) Bromocresol purple Bromothymol blue Nitrophenol Phenol red Thymol blue Phenolphthalein Alizarin yellow R 2.1 2.8 Violet Red 3.3 Red Yellow 3.7 Red Yellow 4.0 Yellow Blue-violet 4.1 Blue Red 4.1 Colorless Yellow 4.3 Red Yellow 4.7 Yellow Blue 5.1 ed Yellow 5.4 Colorless red 5.8 Red Blue 6.3 Yellow Violet 7.0 Yellow Blue 7.2 Colorless Yellow 7.9 Yellow Red 8.9 Yellow blue 9.4 Colorless Red 11.0 Yellow red

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 37QAP: Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at...

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Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
I have contacted Bartleby customer support and they said this question is valid to be asked! They have said if someone denys again, i can contact them back and they will know who has declined and have a talk with them! Dont cause any issues! Use acid-base titration to determine theconcentration of:– A weak acid: CH3COOH 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10
An acid-base indicator is usually a weak acid with a characteristic color in the protonated and deprotonated forms. In this assignment, you will monitor the color of an acetic acid solution containing Bromocresol Green as an indicator, as the pH is changed and then you will estimate the ionization constant, Ka, for the indicator. 1. Start Virtual ChemLab, select Acid-Base Chemistry, and then select Ionization Constants of Weak Acids from the list of assignments. The lab will open in the Titration laboratory. Bottles of 0.1104 M NaOH and 0.1031 M HAc (acetic acid) will be on the lab bench. The buret will be filled with the NaOH solution and a beaker containing 10.00 mL of the HAc solution will be on the stir plate. The stir plate will be on, Bromocresol Green indicator will have been added to the beaker, and a calibrated pH probe will also be in the beaker so the pH of the solution can be monitored. 2. What is the color and pH of the solution? Yellow, 2.87 3. On the…
pH Titration Curve for titrating 64.4 mL of Nitric Acid with 0.798 mol/L Aqueous Potassium Hydroxide The volume of titrant used to reach the equivalence point for the titration is _____ mL. (Record your 3-digit answer)b. The pH at the equivalence point for the tittation is ______ c. An appropriate indicator to use is ______At the start of the titration, the indicator colour would be _____and at the endpoint of the reaction the indicator colour would be _____. d. The concentration of the nitric acid solution analyzed in this titration is calculated to be _____ mol/L. (Record your answer with the correct number of significant digits)
Which of these apply to the Image (attached)? There should be 4 total answers: A. High End pH B. High Initial pH C. Vertical Line with Equivalence Point Tall D. Equivalence Point Not at pH 7 E. Equivalence point at pH 7 F. low end pH G. low initial pH H. Vertical Line with Equivalence Point Short Using the info identified above, what type of analyte and tirant combo are in the image. Options for Analyte and Titrant: - Weak base - Strong Acid - Strong Base - Weak Acid
50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. In the presence of phenolphthalein indicator, the acid consumption is 15 mL. Then, the titration is continued by adding bromocresol green indicator, and in the presence of this indicator, the acid consumption is 10 mL. Accordingly, which of the following is the amount of Na2CO3 (in grams) in the sample? (NaOH: 40 g / mol; NazCO3: 106 g / mol)
Which of these apply to Image C (attached)? There should be 4 total answers: A. High End pH B. High Initial pH C. Vertical Line with Equivalence Point Tall D. Equivalence Point Not at pH 7 E. Equivalence point at pH 7 F. low end pH G. low initial pH H. Vertical Line with Equivalence Point Short Using the info identified above, what type of analyte and tirant combo are in the image. Options for Analyte and Titrant: - Weak base - Strong Acid - Strong Base - Weak Acid
which indicator is best used for the titration of aqueous ammonia and benzoic acid?
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