The K of a certain indicator is 7× 107. The color of HIn is green and that of Inis red. A few drops of the indicator are added to an HC1 solution, which is then titrated against an NaOH solution. Over which pH range will the indicator change color? Select the single best answer. 7.2 to 9.2 ○ 4.2 to 6.2 O 6.2 to 8.2 O 5.2 to 7.2 O 3.2 to 5.2

The K of a certain indicator is 7× 107. The color of HIn is green and that of Inis red. A few drops of the indicator are added to an HC1 solution, which is then titrated against an NaOH solution. Over which pH range will the indicator change color? Select the single best answer. 7.2 to 9.2 ○ 4.2 to 6.2 O 6.2 to 8.2 O 5.2 to 7.2 O 3.2 to 5.2

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

The indicator thymol blue changes from red to yellow between pH 1.2 and pH 2.8. If thymol blue is added to a solution, and the solution turns yellow, then the pH of the solution must be above 2.8, and the solution is basic. the pH of the solution must be above 2.8, and the solution is acidic. the solution is basic, and the pH must be at or below 1.2. the pH of the solution is above 2.8, and the solution could be acidic, neutral or basic. the solution is acidic, and the pH must be at or below 1.2.
The pK, of hypochlorous acid is 7.530. A 52.0 mL solution of 0.148 M sodium hypochlorite (NaOCI) is titrated with 0.293 M HCI. Calculate the pH of the solution after the addition of 10.3 mL of 0.293 M HCI. pH = Calculate the pH of the solution after the addition of 27.9 mL of 0.293 M HCI. pH = Calculate the pH of the solution at the equivalence point with 0.293 M HCI. pH =
Bromothymol blue is yellow in acid solutions. HBB is acidic form of the indicator . The indicator is blue in basic solutions. BB- is basic form of the indicator. HBB + H2O H3O+ + BB- (a) Predict what will happen if NaOH is added to the reaction system. And why ? (b). Predict what will happen if HCl solution is added to the reaction system. And why ?
A 1.0-L buffer solution contains 0.100 mol acid, HA, and 0.100 mol base, NaA. The value of K, for the acid HA is 1.8x104. Ignoring the small volume change, what is the most likely pH of the solution if a 10.0 mL- sample of 1.00 M HCI is added to the original buffer? O 5.50 < pH < 5.74 O 3.51 < pH < 3.69 O 4.10 < pH < 4.22 O 1.20 < pH < 1.45
Hydrofluoric acid has a Ka of 6.6 x 10-4. 40.00 mL of 0.150 M sodium fluoride, NaF, is titrated against 0.125 M HBr. Give the pH at these four points: initial, 32.00 mL of acid have been added, at the equivalence point, and when 60.00 mL have been added.
Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a samplefor a pharmaceutical company with a quantitative titration and dissolve 10 tablets, eachcontaining 200 mg of aspirin, in 150 mL of water.a) Determine the pH of this solution.b) Determine the pH of the solution after you have added 20.0 mL of 0.500 M NaOH.
A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2 (ethylamine), the burette is filled with 0.20 M HCl as titrant. Kb of C2H3NH2 = 6.5 ´ 10-4 What is the initial pH of above sample solution before titration starts?
A 1.0-L buffer solution contains 0.100 mol acid, HA, and 0.100 mol base, NaA. The value of K, for the acid HA is 1.8x104. Ignoring the small volume change, what is the most likely pH of the solution if a 10.0 mL- sample of 1.00M HCI is added to the original buffer? O 1.20 < pH < 1.45 O 5.50 < pH < 5.74 O 4.10 < pH < 4.22 O 3.51 < pH < 3.69
For a buffer initially containing .08 mol of benzoic acid (HC7H5O2) and .12 mol of C7H5O2 in 1.0 L, what is the pH after .07 mol of OH is added to the buffer? .07 mol OH- .08 mol HC,H,O2 .12 mol C,H¿0; O 4.57 O 5.47 O 2.91 O 4.37 O 3.71
A solution is prepared that is initially 0.26M in hydrofluoric acid (HF) and 0.25M in potassium fluoride (KF). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H₂O*]. You can leave out the M symbol for molarity. initial change final [HF] 0 П [F] 0 0 0 [H₂O*] 0 0 0 X
A certain indicator, HA, has a Ka value of 3.2×10−5. The protonated form of the indicator is red and the ionized form is yellow. What is the pKa of the indicator? a) pKa= b) what is the color of this indicator in a solution with pH = 7? -orange -red -yellow
Consider a buffer made from 255 mL 0.10M HC2H:O2 and 125 mL 0.10 NaC2H:O2. Ka for HC2H3O2 is 1.8 x 105. Choose the true statement. A) Adding 25 mg NaOH (s) will reduce the pH. B) Adding 25 mL water will increase the pH. C) Adding 25 mL 0.0050 M HCI will increase the pH. D) Adding 25 mL 0.0050 M HF will reduce the pH. E) Adding 25 mg NaCl (s) will increase the pH.