Answer: The volume of HBr solution required is 542.8 mL
Explanation:
To calculate the concentration of base, we use the equation given by neutralization reaction:
[tex]n_1M_1V_1=n_2M_2V_2[/tex]
where,
[tex]n_1,M_1\text{ and }V_1[/tex] are the n-factor, molarity and volume of acid which is [tex]H_3PO_4[/tex]
[tex]n_2,M_2\text{ and }V_2[/tex] are the n-factor, molarity and volume of base which is [tex]KOH[/tex]
We are given:
[tex]n_1=3\\M_1=0.656M\\V_1=40mL\\n_2=1\\M_2=0.15M\\V_2=?mL[/tex]
Putting values in above equation, we get:
[tex]3\times 0.656\times 40=1\times 0.15\times V_2\\\\V_2=542.8mL[/tex]
Hence, the volume of KOH solution required is 542.8 mL
