Respuesta :
Answer:
0.0303 Liters
Explanation:
Given:
Mass of the potassium hydrogen phosphate = 0.2352
Molarity of the HNO₃ Solution = 0.08892 M
Now,
From the reaction it can be observed that 1 mol of potassium hydrogen phosphate reacts with 2 mol of HNO₃
The number of moles of 0.2352 g of potassium hydrogen phosphate
= Mass / Molar mass
also,
Molar mass of potassium hydrogen phosphate
= 2 × (39.09) + 1 + 30.97 + 4 × 16 = 174.15 g / mol
Number of moles = 0.2352 / 174.15 = 0.00135 moles
thus,
The number of moles of HNO₃ required for 0.00135 moles
= 2 × 0.00135 mol of HNO₃
= 0.0027 mol of HNO₃
Now,
Molarity = Number of Moles / Volume
thus,
for 0.0027 mol of HNO₃, we have
0.08892 = 0.0027 / Volume
or
Volume = 0.0303 Liters
Answer: The volume of nitric acid is 0.025 L.
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Given mass of KHP = 0.2352 g
Molar mass of KHP = 204.22 g/mol
Putting values in above equation, we get:
[tex]\text{Moles of KHP}=\frac{0.2352g}{204.22g/mol}=0.0011mol[/tex]
The chemical reaction for the formation of chromium oxide follows the equation:
[tex]K_2HPO_4+2HNO_3\rightarrow H_2PO_4+KNO_3[/tex]
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 = [tex]\frac{2}{1}\times 0.0011=0.0022mol[/tex] of nitric acid
To calculate the volume of nitric acid, we use the equation:
[tex]\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}[/tex]
We are given:
Moles of Nitric acid = 0.0022 moles
Molarity of solution = 0.08892 M
Putting values in above equation, we get:
[tex]0.08892mol/L=\frac{0.0022mol}{\text{Volume of solution}}\\\\\text{Volume of solution}=0.025L[/tex]
Hence, the volume of nitric acid is 0.025 L.
