Question

Oпределите pH, раствора объемом 100 мл, в котором содержится 0,063 г азотной кислоты

Answer 1

1. Найдем молярную концентрацию раствора :
С(HNO3)=m(HNO3)/(M(HNO3)*V)=0,063/(63*0,1)=0,01моль/л
2. Рн=-LOG C(HNO3)=2
рН=2

Answer 2

Determining the pH of a solution containing 0.063 g of nitric acid in 100 mL

To determine the pH of a solution, we need to know the concentration of the acid. In this case, we are given the mass of nitric acid (HNO3) in the solution, which is 0.063 g, and the volume of the solution, which is 100 mL.

To calculate the concentration of the nitric acid, we can use the formula:

Concentration (C) = mass (m) / volume (V)

Substituting the given values, we have:

C = 0.063 g / 100 mL

Now, we need to convert the volume from milliliters to liters to match the units of the concentration. There are 1000 mL in 1 L, so:

V = 100 mL / 1000 mL/L = 0.1 L

Substituting the values into the concentration formula, we have:

C = 0.063 g / 0.1 L = 0.63 g/L

Now that we have the concentration of the nitric acid, we can calculate the pH of the solution. The pH is a measure of the acidity or alkalinity of a solution and is defined as the negative logarithm (base 10) of the hydrogen ion concentration ([H+]).

The concentration of hydrogen ions in a solution of nitric acid is equal to the concentration of the acid because nitric acid is a strong acid and dissociates completely in water to produce hydrogen ions. Therefore, the concentration of hydrogen ions is 0.63 g/L.

To calculate the pH, we can use the formula:

pH = -log[H+]

Substituting the concentration of hydrogen ions, we have:

pH = -log(0.63 g/L)

Now, let's calculate the pH using a calculator or software:

pH ≈ 0.20

Therefore, the pH of the solution containing 0.063 g of nitric acid in 100 mL is approximately 0.20.

Please note that the pH calculation assumes ideal conditions and does not take into account any other substances or factors that may affect the acidity or alkalinity of the solution.