What is the pH of a 5.41g of HNO3 in 7L of solution (mass of HNO3=63.02g)

A) 3.56
B) 2.88
C) 2
D) 1

The pH of the solution is 1.91

Explanation:

Step 1:

Data obtained from the question. This includes the following:

Mass of HNO3 = 5.41g

Volume of solution = 7L

Molar Mass of HNO3 = 63.02g/mol

pH =?

Step 2:

Determination of the number of mole of HNO3. This is illustrated below:

Mass of HNO3 = 5.41g

Molar Mass of HNO3 = 63.02g/mol

Number of mole HNO3 =?

Number of mole = Mass/Molar Mass

Number of mole of HNO3 = 5.41/63.02

Number of mole of HNO3 = 0.086 mole

Step 3:

Determination of the molarity of HNO3. This is illustrated below:

Mole of HNO3 = 0.086 mole

Volume of solution = 7L

Molarity of HNO3 =.?

Molarity = mole/Volume

Molarity of HNO3 = 0.086/7

Molarity of HNO3 = 0.0123 M

Step 4:

Determination of the hydrogen ion concentration in HNO3. This can be achieved by doing the following:

Dissociation equation of HNO3

HNO3(aq) —> H+ + NO3-

From the above equation,

1 mole of HNO3 produced 1 mole of H+.

Therefore, 0.0123 M of HNO3 will also produce 0.0123 M of H+.

The concentration of H+ is 0.0123 M

Step 5:

Determination of the pH of the solution.

pH = –Log [H+]

[H+] = 0.0123 M

pH = –Log 0.0123

pH = 1.91

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

some sources quote the lethal dose, for an average 170lbs opiate-naive individual is between 75 and 375 mg