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

a pan containing water is placed in a positio n where it is exposed to a 10 mile per hour wind. the pan contains a uniform depth of 1.27 cm of water, is quite wide, and has a length of 2.44 m in the wind direction. the water in the pan is at a constant temperature of 15.5 °c.