Methyl orange is an indicator with a Ka of 1 x 10-4. Its acid form, HIn, is red, while its base form, In-, is yellow. At pH 7.0, the indicator will be___________. a. red. b. orange. c. yellow. d. blue. e. not enough information
Methyl orange is an indicator with a Ka of 1 x 10-4. Its acid form, HIn,...
An indicator, HIn, has a Ka of 1.5 x 10-6. The color of the neutral form is red and that of the ionized form is yellow. Predict the colour of this indicator in a solution with a pH of 10.50.
15. The acid-base indicator bromocresol green has a Ka of 6.3 x 10-5. Its protonated form is yellow while its deprtonated form is blue. If bromocresol green is added to a colorless solution with a pH of 8, then what will the color be?
Consider the following indicator reaction for methyl orange: HIn(aq)+H2O(l)↽−−⇀H3O+(aq)+In−(aq) Given that the anion of methyl orange, In−, is yellow, and the nonionized form HIn is red. If most of the indicator is present as In−, then we observe which color?
How do you get the answer just a little confused
Version 1 12. Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 x 10-. Its un-ionized form 7.82 is red and its anionic form is yellow. What color would a methyl red solution have at pH A) violet B) yellow C) green D) blue E) red 13 Assuming egual concentrations of conllgate hase and acid uhich one of tho f uolu, n a
A weak acid indicator HIn is blue while its conjugate base In is green. Kaln for the indicator is 7.7 x 10*5 Over what pH range does the indicator change color? lower pH upper pH
A weak acid indicator Hin is blue while its conjugate base in is green. Kain for the indicator is 4.7 x 10-5 Over what pH range does the indicator change color? lower pH upper pH
a) An unknown indicator (called “HIn”) has a Ka of 4.0 x 10-6. The color of the neutral form is green, and that of ionized form is red. The indicator is added to a HCl solution, which is then titrated against a NaOH solution. At what pH will the indicator change color? b) 350. mL of a NaOH solution was added to 500. mL of 2.50 M HNO2. The pH of the mixed solution was 1.75 units greater than that...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is to indicate the of the titration. Use Table 10.2 for the following question. If an acidic solution is titrated with a basic solution and methyl violet is used as an indicator, the solution color will change from to QUESTION 2 3 points Save Answer The molarity of a solution prepared by dissolving 17.0 g of hydrochloric acid (HCI (aq) in 133 mL of water...
Methyl orange may be used as an indicator in acid-base titrations, it is described by the equilibrium HMOrng (red) = H+ + MOrng (yellow) pka = 3.98 At what pHs might we observe the following colors in this order?: red, orange, yellow a. O 1.00, 14.00, 7.00 b. O 7.00, 1.00, 4.00 c. O 2.00, 6.00, 4.00 d. O 2.00, 4.00. 6.00
Consider the titration of 25.00 mL of 0.115M NH3 (ka= 5.70e-10 ;
kb= 1.75e-5) with 0.0920 M HCl.
a) calculate the pH of the solution for the following volume of
HCl: 6.25 mL
b) calculate the pH of the solution for the following volume of
HCl: 31.25 mL
c) calculate the pH of the solution for the following volume of
HCl: 50.0 mL
d) Which indicator from the table minimizes the titration error
and why?
blue Indicator thymol blue bromophenol...