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Calcualte the pH at which an indicator w...

Calcualte the `pH` at which an indicator with `pK_(b) = 4` changes colour.

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To calculate the pH at which an indicator with \( pK_b = 4 \) changes color, we can follow these steps: ### Step 1: Calculate \( K_b \) from \( pK_b \) The relationship between \( pK_b \) and \( K_b \) is given by the formula: \[ pK_b = -\log(K_b) \] Given \( pK_b = 4 \), we can find \( K_b \) as follows: ...
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STATEMENT-1: In the acid-base titration involving strong base and weak acid, methyl red can be used as an indicator. STATEMENT-2: Methyl red changes its colour in the pH range 4.2 to 6.3.

An acid base indicator has K_(a)=1.0xx10^(-5) the acid form of the indicator is red and the basic form is blue. Calculate the pH change required to change the colour of the indicator from 80% red to 80% blue.

Select the correct set of the statements for an acid type indicator used in a titration : (i) In general, pH range of an indicator is (pK_(a)-1) to (pK_(a)+1) and indicator shows its characteristic colours in this range. (ii) In general pH range of an indicator is (pK_(a)-1) to (pK_(a)-1) and indicator does not show its characteristic colours in this range (iii) In this relation : pH=pK_(In) +log_(10)((["In"^(-)])/(["HIn"])),pH value representes pH of indicator solution. (iv) In this relation : pH=pK_(In) +log_(10)((["In"^(-)])/(["HIn"])),pH value represents pH of resulting solution containing indiactor .

Acid-base indicators are either weak organic acids or weak organic bases. Indicator change colour in dilute solution when the hydonium ion concentration reaches a particular calur For example. Phenolphthalein is a coloureless stbstance in any aqueous solution with a pH less than 8.3 In between the pH range 8.3 to 10, transition of colour (colourless to pink ) takes place and if pH of solution is greater than 10 solution is dark pink. Considering an acid indicator Hln, the equilibrium involving it and its conjgate base In^(-) can be represented as : " " underset("acidic from")(HIn)hArrH^(+)underset("basic from")(In^(-)) pH of solution can be computed as : " " pH=pK_(In)+log.([IN^(-)])/([HIn]) In general, transition of colour takes place in between the pH range pK_(In+-1. Calculate the pH at equivalence point when 5 milli mol of HB is titrated with 0.1 M NaOH.

CENGAGE CHEMISTRY ENGLISH-IONIC EQUILIBRIUM-Archives Subjective
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