in my text book it says that if the calculated value is less than or equal to 0.1 then the color of the conjugate base (In- in this case) predominates. does this mean that the solution will be yellow then?
yes, yellow
In my text, it says FOR AN ACID INDICATOR, HIn, that if (HIn)/(In^-) = or> 10, the acid color predominates or if (HIn)/(In) <or= 0.1, the base color predominates. Make sure you are reading about acid indicator (versus base indicators) and that the ratio is as I have it above. The problem states that it is an acid indicator, I think, and that it dissociates into H3O^+ and In^- in the ionized form.
you are right....I wrote it wrong. Does this mean that the solution will be more toward the redish side?
Yes, I think red.
To determine the color of a solution, it's important to consider the specific chemical species present and not rely solely on a threshold value like 0.1. Generally, the color of a solution is determined by the wavelength of light absorbed or transmitted by the solution.
In the case you mentioned, the presence of the conjugate base In- suggests that there is an acid-base equilibrium. The acid form (HA) will be in equilibrium with its conjugate base (In-) according to the equation: HA ⇌ H+ + In-.
The color of HA or In- ions might depend on their electronic structure and absorption spectrum. For example, if the In- ions absorb light in the visible spectrum and transmit yellow light, then the solution could indeed appear yellow. However, without specific information about the compound or its absorption spectrum, it is not possible to definitively determine the color of the solution. It's worth noting that factors such as concentration, pH, and presence of other compounds can also influence the observed color.
To gain more accurate information about the color of a specific compound or solution, it is recommended to consult reliable sources like scientific literature, databases, or specific experiments conducted on the compound in question.