Chemistry: How many milliliters of a 0.15--m solution of koh will be reuired to titrate 40.00ml of a 0.656-m solution of h3po4? h3po4 + 2koh ? k2hpo4 + 2h2o

How many milliliters of a 0.15--m solution of - id0152215017, daevinepetersopa86on

sam9043

02.01.2022

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:

n_1M_1V_1=n_2M_2V_2

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is H_3PO_4

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is KOH

We are given:

$n_1=3\\M_1=0.656M\\V_1=40mL\\n_2=1\\M_2=0.15M\\V_2=?mL$

Putting values in above equation, we get:

$3\times 0.656\times 40=1\times 0.15\times V_2\\\\V_2=542.8mL$

Hence, the volume of KOH solution required is 542.8 mL

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xEmqq2034

25.11.2021

Explanation:

Proper scientific notation looks like a decimal after the first whole number times 10 with an eponent of either a negative or posiitiveumber n

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