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

The molarity of basic solution is 1M

Explanation:

The chemical reaction for the reaction of KHP and NaOH follows

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 =

Equating the two :

Thus molarity of basic solution is 1M

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole