Question

someone help me please im stuck on a equation


3. Rearrange the titration calculation to find the Mb in a solution. (* Mb = molarity of the basic solution )

(~0.3 mL) of indicator to the KHP

solution.

(~ 0.5 mL or less) of NaOH


The moles of acid= 0.5 x 100/1000=0.05 Mb = (0.5/55)x1000=0.9

Answer 1

Answer: The molarity of basic solution is 1M

Explanation:

The chemical reaction for the reaction of KHP and NaOH follows

$KHP+NaOH\rightarrow KNaP+H_2O$

By Stoichiometry of the reaction:  

1 mole of KHP reacts with 1 mole of NaOH.  

Thus moles of acid = moles of base

Given :

moles of acid =  [/tex]0.5\times \frac{100}{1000}[/tex]

moles of base = $0.05\times M_b$

Equating the two :

$0.5\times \frac{100}{1000}=0.05\times M_b$

$M_b=1M$

Thus molarity of basic solution is 1M