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3 years ago

Which of the following describes the stage that occurs after condensation in the water cycle?

Chemistry

1 answer:

NISA [10]3 years ago

5 0

Answer:

Precipitation

Explanation:

There are four main stages in the water cycle. They are evaporation, condensation, precipitation and collection. Let's look at each of these stages. Evaporation: This is when warmth from the sun causes water from oceans, lakes, streams, ice and soils to rise into the air and turn into water vapour (gas).

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What happens to an acid when it dissolves in water?

shusha [124]

The concentration of the acid decreases

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3 years ago

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Which of these solutes raises the boiling point of water the most?

Alekssandra [29.7K]

The answer is <span>ionic aluminum fluoride (</span>AlF3). Note that boiling points of pure solvents are raised in the presence of solutes. The type of solute also affects the boiling point elevation of the solution. Ionic substances tend to raise it more than covalent ones, so sucrose is out of the picture. Next, consider the number of ions the ionic substance produces. The more ions, the greater the BPE. AlF3 dissociates into 4 ions.

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3 years ago

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What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K?

salantis [7]

Answer:

Option A = 14.19 atm

Explanation:

Given data:

Volume of gas = 2.50 L

Number of moles of gas = 1.35 mol

Temperature of gas = 320 K

Pressure of gas = ?

Solution:

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K

T = temperature in kelvin

Now we will put the values in formula.

P × 2.50 L = 1.35 mol × 0.0821 atm.L/ mol.K× 320

P = 35.467 atm.L/ 2.50 L

P = 14.19 atm

Thus, option A is correct.

6 0

3 years ago

Suppose you wanted to make a buffer of exactly ph 7.00 using kh2po4 and na2hpo4. if the final solution was 0.10 m in kh2po4, wha

OleMash [197]

Answer:- 0.138 M

Solution:- The buffer pH is calculated using Handerson equation:

$pH=pKa+log(\frac{base}{acid})$

$KH_2PO_4$ acts as a weak acid and $Na_2HPO_4$ as a base which is pretty conjugate base of the weak acid we have.

The acid hase two protons(hydrogen) where as the base has only one proton. So, we could write the equation as:

$H_2PO_4^-\rightleftharpoons H^++HPO_4^-^2$

Phosphoric acid gives protons in three steps. So, the above equation is the second step as the acid has only two protons and the base has one proton.

So, we will use the second pKa value. The acid concentration is given as 0.10 M and we are asked to calculate the concentration of the base to make a buffer of exactly pH 7.00.

Let's plug in the values in the equation:

$7.00=6.86+log(\frac{base}{0.10})$

$7.00-6.86=log(\frac{base}{0.10})$

$0.14=log(\frac{base}{0.10})$

Taking antilog:

$10^0^.^1^4=\frac{base}{0.10}$

$1.38=\frac{base}{0.10}$

On cross multiply:

[base] = 1.38(0.10)

[base] = 0.138

So, the concentration of the base that is $Na_2HPO_4$ required to make the buffer is 0.138M.

5 0

3 years ago

If 23.5 g of ammonia (NH3) is dissolved in 1.0 L of solution, what is the molarity?

Alex

The molarity of the ammonia solution is 1.38 M

<h3>Definition of molarity</h3>

Molarity is defined as the mole of solute per unit litre of the solution. Mathematically, it can be expressed as:

Molarity = mole / Volume

<h3>Determination of the mole of NH₃</h3>

•Mass of NH₃ = 23.5 g

•Molar mass of NH₃ = 14 + (3×1) = 17 g/mol

•Mole of NH₃ =?

Mole = mass / molar mass

Mole of NH₃ = 23.5 / 17

Mole of NH₃ = 1.38 mole

<h3>Determination of the molarity </h3>

•Mole of NH₃ = 1.38 mole

•Volume = 1 L

•Molarity of NH₃ =?

Molarity = mole / Volume

Molarity of NH₃ = 1.38 / 1

Molarity of NH₃ = 1.38 M

Learn more about molarity:

brainly.com/question/9468209

3 0

3 years ago