**Titration Analysis**The given titration plot has an equivalence point at pH = 4.3.**Identify which of the indicators would be appropriate for this titration:**- [ ] bromothymol blue- [ ] ethyl orange- [ ] phenolphthalein- [ ] bromophenol blue- [ ] methyl orange- [ ] bromocresol purple**Graph Explanation:**The graph, titled "Titration Data," shows the relationship between pH and the volume of titrant added. The curve begins at a higher pH and descends, indicating an acidic titration environment. The equivalence point is marked at pH 4.3. The endpoint pH range is illustrated between 3.3 and 5.3, which will help in selecting a suitable indicator for the titration.

Answer: Indicator is a substance that is used in a titration to identify the end point. Usually…

Macm The titration shown in the plot has an equivalence point at pH = 4.3. Identify which of the indicators would be appropriate for this titration. bromothymol blue ethyl orange phenolphthalein bromophenol blue methyl orange bromocresol purple pH Titration Data Titrant volume end-point pH range 5.3 3.3

Macm The titration shown in the plot has an equivalence point at pH = 4.3. Identify which of the indicators would be appropriate for this titration. bromothymol blue ethyl orange phenolphthalein bromophenol blue methyl orange bromocresol purple pH Titration Data Titrant volume end-point pH range 5.3 3.3

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

A chemist titrates 230.0 mL of a 0.1072M ethylamine (C,H,NH,) solution with 0.5758M HCI solution at 25 °C. Calculate the pH at equivalence. The p K, of ethylamine is 3.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = Explanation Check 2021 McGraw-Hill Education All Rights sved T Le/Py 18 MacBook Air esc F7 FI F2 F3 F4 *
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
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 .0 and 7.6 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
Consider how best to prepare one liter of a buffer solution with pH = 6.52 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32 How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams sodium salt of weak acid = grams sodium salt of conjugate base =
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
Titration Curve Using the table of indicators identify which of the given 13 12 indicators would be appropriate for the titration 11 10 represented in the titration curve. 9 thymol blue 8 metacresol purple pH 7 phenol red alizarin O metanil yellow 0 2 6 8 10 12 14 16 18 20 thymolphthalein Volume of Titrant (mL) 4. O54 321
Determine the concentration of CH NH¸* in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of CH NH+. The Kb for CH NH₂ is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. 2 1 2 3 NEXT > 2 A buffer solution contains dissolved CH NH and CH NH Cl. The initial concentration of CH NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of CH NH+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CH NH2(aq) + H₂O(I) = OH(aq) + C HẠNH, (aq) RESET 0 0.50 x 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 × 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x-4.20 x + 6.3 x 10-5 x - 6.3 × 10-5 x + 1.6 × 10-10 x-1.6 × 10-10 x + 3.8 × 10-10 x - 3.8 × 10-10
Explain the difference between an indicator endpoint for a titration analysis and the true equivalence point for the titration. Please simplify the answer so I can understand. Thanks
A scientist is attempting to recreate this titration using the same concentration of hydrochloric acid, but decides to use a lower concentration of sodium hydroxide(titrant). The original concentration of sodium hydroxide is 0.1M. How will this affect the amount of titrant needed? Explain.Correctly predicts the relative amount of titrant needed and explains.
Calculate change in pH of a buffer solution
An aqueous solution of an unknown solid salt was placed into five different test tubes. Into each test tube a couple of drops of different indicators were then added to each test tube and the color of the indicator in the solution was recorded as shown below. What is the approximate pH of the solution? Test pH Acid Base Color in Unknown Indicator tube Range Color Color Solution 3.0 - 1 Methyl orange 4.4 Red Yellow Yellow 3.0 - Congo Red Purple Red Red 5.0 Bromcresol 3.8 - Yellow Blue Blue Green 5.4 Bromthymol 6.0 - 7.6 4 Yellow Blue Yellow Blue 8.2 - Phenolphthalein Colorless Blue Colorless 10.0 4.3 O 8.4 O 5.2 6.7
Interpret pH titration plots. Answer the following about the titration plot shown below, involving a monoprotic acid and base. 20 mL of 0.1M titrand titrated with 0.1M titrant. Data points at 1 mL increments. 14.0 12.0 10.0 5 8.0 6.0 4.0 2.0 0.0 seededood 0 0.0 10.0 مهمه 20.0 30.0 Volume of titrant (mL) (a) Is the species being titrated an acid or a base? (b) Is the species being titrated strong or weak? (c) What is the value of Ka (if a weak acid) or K, (if a weak base) for the species being titrated? If the species is strong (100% dissociated), enter 999. rààààààààà 40.0 50.0