What volume of 0.08892 m hno3 is required to react completetly with 0.2352 g of potassium hydrogen phosphate?
2hno3 + k2hpo4 ? h2po4 + kno3

The volume of nitric acid is 0.025 L.

Explanation:

To calculate the number of moles, we use the equation:

Given mass of KHP = 0.2352 g

Molar mass of KHP = 204.22 g/mol

Putting values in above equation, we get:

The chemical reaction for the formation of chromium oxide follows the equation:

By Stoichiometry of the reaction:

1 mole of potassium hydrogen phosphate reacts with 2 mole of nitric acid

So, 0.0011 moles of potassium hydrogen phosphate will react with = of nitric acid

To calculate the volume of nitric acid, we use the equation:

We are given:

Moles of Nitric acid = 0.0022 moles

Molarity of solution = 0.08892 M

Putting values in above equation, we get:

Hence, the volume of nitric acid is 0.025 L.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.