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Flura [38]
3 years ago
6

at 20°c, a 0.376 m aqueous solution of ammonium chloride has a density of 1.0045 g/ml. what is the mass % of ammonium chloride i

n the solution? the formula weight of nh4cl is 53.50 g/ml.
Chemistry
1 answer:
madam [21]3 years ago
7 0

At 20°c, a 0.376 m aqueous solution of ammonium chloride has a density of 1.0045 g/ml. The mass percent of the ammonium chloride in the solution is 2.003%.

The number of moles of a substance can be estimated as:

\mathbf{number\ of\ moles = \dfrac{mass}{molar \ mass}}

Given that:

  • number of moles = 0.376 M
  • molar mass of ammonium chloride = 53.50 g/ml

Mass = number of moles × molar mass

Mass = 0.376 × 53.50

Mass = 20.116 grams

In one mL of ammonium chloride; the grams of ammonium chloride is:

\mathbf{= \dfrac{20.116 \ grams}{1000 \ mL}}

= 0.020116 g/mL

The mass of ammonium chloride in the solution can be computed as:

\mathbf{=(\dfrac{mass \ of \ NH_4Cl}{density \ of  \  the \  solution})\times 100}

\mathbf{=(\dfrac{0.020116 }{1.0045})\times 100}

= 2.003%

Therefore, we can conclude that the mass percent of the ammonium chloride in the solution is 2.003%.

Learn more about ammonium chloride here:

brainly.com/question/23387600?referrer=searchResults

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A student mixed 50 ml of 1.0 M HCl and 50 ml of 1.0 M NaOH in a coffee cup calorimeter and calculated the molar enthalpy change
MrRa [10]

Answer:

-54 kJ/mol

Explanation:

Given that:

A student mixed 50 ml of 1.0 M HCl and 50 ml of 1.0 M NaOH in a coffee cup calorimeter and calculated the molar enthalpy change of the acid-base neutralization reaction to be –54 kJ/mol

i.e

50 ml of 1.0 M HCl +  50 ml of 1.0 M NaOH -----> -54 kJ/mol

If he repeat the same experiment with :

100 ml of 1.0 M HCl + 100 ml of 1.0 M NaOH. ------> ????

From The experiment; the molar enthalpy of change of the acid-base neutralization reaction will be -54 kJ/mol

This is because : The second reaction requires 50 ml in order to neutralize the reaction, then the remaining 50 ml will be excess, Hence, there is no change in the enthalpy of the reaction.

Similarly; we can assume that :

In the first reaction;  P moles of  is used to liberate Q kJ heat ; then  the change in molar enthalpy will be Q/P (kJ/mol).

SO; when he used 100 ml ;

then the amount of moles used is double, likewise the heat liberated will be doubled ;

So;

2P moles is used to liberate 2Q kJ heat ;

2P/2Q = Q/P ( kJ/mol) = -54 kJ/mol

8 0
3 years ago
A student investigated the factors that affect math grades. Which statement from the lab report best represents a conclusion for
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The correct answer choice from the statement above about investigated factors from lab results is :

Students who spend less time studying after school get lower math grade

Option D is the correct answer

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Mathematics is one of the most important aspect of knowledge in the education.

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Students who spend less time studying after school get lower math grade

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5 0
2 years ago
4
Archy [21]

Answer:

Pressure

Explanation:

The variable that describes how often the particles in a sample of gas collides with each other and the walls of the container is the pressure.

The pressure of a gas is the combined force with which the gas molecules bombard a unit area of the wall of the container i.e the sum of all the tiny pushes on the unit area of the wall of the container.

The various units of gas pressure atmosphere, millimeters of Hg, torr, pascal, newton per meter squared.

  • Temperature is the degree of hotness or coldness of a body
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3 0
3 years ago
A compound contains 75% carbon and 25% hydrogen by mass. what is the empirical formula for this compound?
Lady bird [3.3K]
These percentages are most likely mass percentages. Therefore, determine the mass of each element in 100g of the compound. 

<span>75g C, 25g H. </span>

<span>Divide these masses by their molar mass to find the ratios of the moles of element in the compound. Divide these values by the smallest of the two/three to get the ratios. </span>

<span>6.25:25 C:H --> 1:4 </span>


<span>So the formulae are CH4 (methane).</span>
4 0
3 years ago
Read 2 more answers
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