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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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State the nature of the pH (acidic, basic, or neutral) at the equivalence point for the following titrations and the suitable indicator (methyl orange pKin= 4 ; bromothymol blue pKin=7; phenolphthalein pKin=9).
a. Sodium hydroxide added to nitric acid
b. Ammonia added to nitric acid
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- d. The following acid-base indicators are available to follow the titration. Which of them would be most appropriate for signaling the endpoint of the titration? Explain. Color Change Indicator Acid Form Base Form pH Transition Interval Bromphenol blue Bromthymol blue Thymol blue yellow yellow yellow blue 3.0–5.0 blue 6.0–7.6 blue 8.0–9.6arrow_forward3 a) The Ka value for phenolphthalein is 8 x 10-10. What is the concentration of hydrogen ton when this indicator changes colour? b) What is the pH at end paint? c) From your pH curve, why is the assumption that end point equals equivalence point valid for phenolphthalein?arrow_forwardTitration 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 pH 7 6 alizarin yellow R 5 O quinaldine red 4 3 O clayton yellow 2 1 metacresol purple 4 6 8 10 12 14 16 18 20 Volume of Titrant (mL) O methyl green 2.arrow_forward
- se or conjugate base. 12 2. A 50.0mL sample of an acid HA, of unknown molarity is titrated with 0.1000 M KOH. The pH of the resulting solution is measure with a pH meter and graphed below. Select the letter that corresponds to the following. Some letters may be used more than once. Some may not be used at all. 10+ a. the equivalence point: R 9 b. the half equivalence point: Q 8+ c. where [KOH] is greatest: 7+ P I of d. where [H+] is greatest: T e. where [HA]=[A-]: 5+ 4 f. where [A-] is the predominate species: 3+ 2 SO a. What is pH after 10.0mL of 0.15M NaOH solution has been added to 25.0 mL of 0.12M HF solution? Ka = 6.8 x 10-4. b. After adding NaOH, is the resulting solution a buffer solution? Explain. 3. Complete the following calculations. (P) (Q) 84 3 ST PRarrow_forwardIn the titration of HF with NaOH, which species are present at the equivalence point? O HF, NAOH, and H20 only O NaF, NAOH, and H20 only O NaF, HF, and H20 only O NaF and H20 only O HF and H20 onlyarrow_forwardCH3COOH + NaOH → CH3COONa + H₂O If at the beginning you have 1 mol of acetic acid and you have added phenolphthalein as an indicator, when will the end point of the titration be reached? a) When 1 mol of NaOH has reacted b) When the solution changes from clear to a pink color c) When a buffer is formed d) When the solution changes pHarrow_forward
- 1) a)Interpret and explain each region that appears in the titration graph. b)Indicate the color changes and the range in which each indicator is changing the colorarrow_forwardFrom the standard properties of plotted titration curves, which one best represents the titration of a weak acid with a strong base? The curve is with a semi S orientation with the midpoint of the steep part at pH 7 The curve is with a semi Z orientation with the midpoint of the steep part at pH 7 The curve is with an "S' orientation with the midpoint of the steep part at pH > 7 The curve is with a "Z" orientation with the midpoint of the steep part at pH <7 Representative curve cannot be predictedarrow_forward25.0 ml of 0.100M NaOH is titrated with HC2H3O2 and 50.0mL of the acid is used to reach the endpoint. e)Would the compound formed at the equivalence point be acidic, basic or neutral? Write a hydrolysis equation for the salt formed in a) to support your answer. f) Which indicator should be used for this titration? g)Sketch a titration curve for this reaction. Label the x and y axes.arrow_forward
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