11. Which of the following statements are true regarding an acid-base indicator? (Select all that apply) a its colour changes at the equivalence point of any acid-base titration b it is itself a weak acid or a weak base c its various protonated species have different colours d its colour change indicates pH of the solution has reached 7.00 e its colour changes when it gains or loses a H+ ion

11. Which of the following statements are true regarding an acid-base indicator? (Select all that apply) a its colour changes at the equivalence point of any acid-base titration b it is itself a weak acid or a weak base c its various protonated species have different colours d its colour change indicates pH of the solution has reached 7.00 e its colour changes when it gains or loses a H+ ion

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.59QE

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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
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)
1.Which of the following substances have a solvatochromic property? a.potassium hydrogen phthalate b.sodium carbonate c.sodium bicarbonate d.bromocresol green 2. Which will make a good substitute for bromocresol green in a double indicator titration? a.bromothymol blue b.litmus c.methyl red d.potassium hydrogen phthalate
Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3
Directions: Solve the problem with a complete step-by-step solution. Titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar concentration of the KMnO4 solution? The chemical reaction is 2MnO4- + 5C2O42- + 16H+ + ----> 2Mn2+ + 10CO2 + 8H2O
What is the best way to calculate the following titration: 100 ml water and 100 ml of solution with citric acid with pH2 is mixed togeather so the total volume is 200 ml. Then i titrate with NaHCO3 with the following grams. 0.62 gr , 1.82 gr , 2.40 gr What is the pH after each addition of NaHCO3. Please show details, along with the pKa and how it is used as I am very stuck on this and getting it wrong
Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a weak acid with a strong base? Group of answer choices a) 7.00 b) 5.12 c) 9.46 d) 1.55 Need answer with detailed explanation. Will appreciate your efforts. Thank you
While preparing the samples for analysis, you forgot that you already added phenolphthalein indicator so you added some more. What will be its effect in the volume of the titrant needed to reach the endpoint? Select one: A. Increase B. Decrease C. No effect D. Cannot be determined Primary standards are used to determine the exact concentration of the titrant. Based on the criteria of primary standards, which of the following cannot be used as a primary standard? Select one: A.Oxalic acid B. Sodium hydroxide C. Sodium carbonate D. Potassium dichromate During titration, you notice that the retention of the faint pink color is longer than earlier. Your lab partner suggested that you add a “half-drop” to prevent over-titration of the analyte solution. Is it ethical to do the “half-drop” technique? Select one: A. NO. It will cause error in calculations if you forgot to record the volume reading before adding the half-drop. B. YES. No error in calculations will be encountered provided…
please answer both 1.A diprotic acid has Ka1 = 4.3 x 10-3 and Ka2 = 4.5 x 10-7. What will be the pH at the first equivalence point in the titration of the acid? 2. A diprotic acid has Ka1 = 5.3 x 10-5 and Ka2 = 5.7 x 10-9. What will be the pH of a 0.69 M solution of the acid?
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1. Which of the following is/are TRUE about equivalence and end points? I. The end point of a titration is reached when the titrant and analyte are stoichiometrically equal. II. When you are titrating a strong or weak acid with a strong base, the end point will always be faint pink using a phenolphthalein indicator. III. When you are titrating a strong or weak acid with a strong base, the volume needed to reach the end point will always be lower than that of the equivalence point. a.I, II and III b.II only c.III only d.I and III 2. All but one are the criteria why KHP is generally used as the primary standard in determining the actual concentration of the sodium hydroxide titrant: a.It is highly pure. b.It is hygroscopic. c.It is chemically stable. d. It is inexpensive.

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	a	its colour changes at the equivalence point of any acid-base titration
	b	it is itself a weak acid or a weak base
	c	its various protonated species have different colours
	d	its colour change indicates pH of the solution has reached 7.00
	e	its colour changes when it gains or loses a H⁺ ion