Question

. Нашатырный спирт – это водный раствор аммиака. Для получения нашатырного спирта в 300 мл воды растворили 56 л аммиака (н.у.). Вычислите массовую долю и молярную концентрацию аммиака в полученном растворе, если его плотность 0,96 г\мл.

Answer 1

Ответ:

Перевод компонентов смеси в граммы

m(NH3)=(56/22.4)*17=42,5 грамм

m(H2O)=300*1=300 грамм

Масса раствора

m(Sol)=42.5+300=342.5 грамм

Массовая доля

W(NH3)=42.5/342.5=0,124 - 12.4%

Молярная концентрация Сm=(m/M)/V

Cm(NH3)=(42.5/17)/((342.5*0.96)/1000)=7,6 моль/литр

Answer 2

Calculation of Mass Fraction and Molar Concentration of Ammonia in the Solution

To calculate the mass fraction and molar concentration of ammonia in the given solution, we need to use the provided information:

- Volume of water: 300 mL - Amount of ammonia (NH3) dissolved: 56 L (at standard temperature and pressure) - Density of the solution: 0.96 g/mL

Let's calculate the mass fraction and molar concentration step by step.

# Step 1: Convert Volume to Mass

First, we need to convert the volume of water and ammonia to mass using the density of the solution.

The mass of water can be calculated using the formula:

Mass of water = Volume of water × Density of water

Given that the density of the solution is 0.96 g/mL and the volume of water is 300 mL, we can calculate the mass of water as follows:

Mass of water = 300 mL × 0.96 g/mL

Calculating this, we find that the mass of water is 288 g.

Next, we need to convert the volume of ammonia to mass. Since the density of the solution is given, we can directly calculate the mass of ammonia using the formula:

Mass of ammonia = Volume of ammonia × Density of solution

Given that the volume of ammonia is 56 L and the density of the solution is 0.96 g/mL, we can calculate the mass of ammonia as follows:

Mass of ammonia = 56 L × 0.96 g/mL

Calculating this, we find that the mass of ammonia is 53.76 kg.

# Step 2: Calculate Mass Fraction

The mass fraction of ammonia in the solution can be calculated using the formula:

Mass fraction = Mass of ammonia / Total mass of solution

Given that the mass of ammonia is 53.76 kg and the total mass of the solution is the sum of the mass of water and the mass of ammonia, we can calculate the mass fraction as follows:

Mass fraction = 53.76 kg / (53.76 kg + 0.288 kg)

Calculating this, we find that the mass fraction of ammonia in the solution is approximately 0.994.

# Step 3: Calculate Molar Concentration

The molar concentration of ammonia in the solution can be calculated using the formula:

Molar concentration = Amount of substance / Volume of solution

Given that the amount of ammonia is the number of moles of ammonia and the volume of the solution is the sum of the volume of water and the volume of ammonia, we need to convert the mass of ammonia to moles using the molar mass of ammonia.

The molar mass of ammonia (NH3) is approximately 17.03 g/mol.

First, we calculate the number of moles of ammonia:

Number of moles of ammonia = Mass of ammonia / Molar mass of ammonia

Given that the mass of ammonia is 53.76 kg (or 53760 g), we can calculate the number of moles of ammonia as follows:

Number of moles of ammonia = 53760 g / 17.03 g/mol

Calculating this, we find that the number of moles of ammonia is approximately 3157.9 mol.

Next, we calculate the volume of the solution:

Volume of solution = Volume of water + Volume of ammonia

Given that the volume of water is 300 mL and the volume of ammonia is 56 L, we need to convert the volume of water to liters:

Volume of solution = 0.3 L + 56 L

Calculating this, we find that the volume of the solution is 56.3 L.

Finally, we can calculate the molar concentration of ammonia:

Molar concentration = 3157.9 mol / 56.3 L

Calculating this, we find that the molar concentration of ammonia in the solution is approximately 56.1 mol/L.

Therefore, the mass fraction of ammonia in the solution is approximately 0.994, and the molar concentration of ammonia is approximately 56.1 mol/L.

Please note that the provided search results did not contain specific information for this exact calculation. The calculation was performed based on the given information and general knowledge of chemistry principles.