For the titration of a weak base with a strong acid, determine the initial color of solution if the indicator methyl yellow is used. State the color at the completion of the titration

For the titration of a strong acid with a strong base, which of the following indicators would be most suitable?bromomethyl blue, pH range 6.0–7.6bromocresol green, pH range 3.8–5.4methyl orange, pH range 3.1–4.4methyl red, pH range 4.2–6.3Submit answer

WHICH OF THE FOLLOWING IS USED AS AN INDICATOR IN THE TITRATION OF A STRONG ACID AND A WEAK BASE?a.Phenolphthaleinb.Methyl orangec.Fluoresceind.Thymol blue

The best indicator for the detection of end point in titration of a weak acid and a strong base is :-Methyl orange (3.1 to 4.4)Methyl red (4.2 to 6.3)Bromothymol blue (6 to 7.6)Phenolphthalein (8.2 to 10)

For the titration of a strong acid with a strong base, the equivalence point at which base completely neutralizes the acid has a pH of 7.0. Select and justify your choice of an indicator that will allow you to visually determine the equivalence point.

A water sample is alkaline to both phenolphthalein as well as methyl orange. 200 mL of a this water sample on titration with N/50 HCl required 9.4 mL of the acid to phenolphthalein end point. When a few drops of methyl orange are added to the same solution and titration is further continued, the yellow color of the solution just turned red after addition of 30.4 mL of the acid solution. Calculate the  alkalinity present in the water sample.a.P = 152 ppm., M =  47ppm and HCO3– alkalinity = 58 ppm, CO32– alkalinity = 94 ppmb.P = 1520 ppm., M =  470ppm and HCO3– alkalinity = 940 ppm, CO32– alkalinity = 580 ppmc.P = 47 ppm., M = 152 ppm and HCO3– alkalinity = 58 ppm, CO32– alkalinity = 94 ppmd.P = 470 ppm., M = 1520 ppm and HCO3– alkalinity = 580 ppm, CO32– alkalinity = 940 ppm