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3 years ago

Which compound is more soluble in an acidic solution than in a neutral solution?

Chemistry

1 answer:

Nady [450]3 years ago

8 0

Answer : Salt is more soluble in an acidic solution than in an neutral solution.

Explaination : In an acidic solution molecules of salt are assaociated with hydrogen bonding whereas in neutral solutions it molecules are not assaociated with hydrogen bonding. Acidic solution is a type of solution which has higher concentration of hydrogen ions than water is called acidic solution for ex: water.

Neutral solution is a solution which has a pH of 7,it is neither acidic nor basic but it is middle so that is called neutral solution.

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Zinc reacts with iodine in a synthesis reaction: Zn + I2 → Znl2. What is the theoretical yield of Znl2, if 1.912 mol of zinc is

lawyer [7]

Answer:

610.3g

Explanation:

Zn:

m = 1.912

Zn : ZnI₂

1 : 1

1.912 : 1.912

ZnI₂:

m = 1.912 Mr = 65.4 + 2(126.9) = 319.2

mass = m×Mr:

mass = 1.912×319.2

mass = 610.3104 → 610.3g

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4 years ago

Use the development of the atomic model to explain how scientist recline and build off each other’s findings in order to develop

LenKa [72]

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3 years ago

Question 1-8

JulijaS [17]

If 28.0 grams of a gas occupies 22.4 liters at STP, the gas could be carbon monoxide, CO

<h3>Ideal gas </h3>

We understood from the ideal gas equation that 1 mole of any gas occupies 22.4 liters at standard temperature and pressure (STP)

<h3>How to determine the identity of the gas</h3>

To determine the identity of the gas, we shall determine the mass of 1 mole of each gas. This can be obtained as

For C₂H₂

1 mole of C₂H₂ = (12×2) + (2×1) = 26 g

For C₂H₆

1 mole of C₂H₆ = (12×2) + (6×1) = 30 g

For CO₂

1 mole of CO₂ = 12 + (16×2) = 44 g

For CO

I mole of CO = 12 + 16 = 28 g

From the above illustrations, we can see that 1 mole of CO is equivalent to 28 g.

Thus, the correct answer to the question is CO

Learn more about ideal gas equation:

brainly.com/question/4147359

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3 0

2 years ago

A 27.5 −g aluminum block is warmed to 65.9 ∘C and plunged into an insulated beaker containing 55.5 g water initially at 22.1 ∘C.

Wittaler [7]

Answer:

The final temperature of aluminium ≈ 26.32 °C

Explanation:

<u>Step 1:</u> explain the problem

A 27.5 −g aluminum block is warmed to 65.9 ∘C and plunged into an insulated beaker containing 55.5 g water initially at 22.1 ∘C.

<u>Step 2:</u> Data given

We will use the formule : Q = mcΔT

with Q = heat transfer ( J)

with m = mass of the substance (g)

with c = specific heat ( J/g °C)

with ΔT = change in temperature ( in °C or K)

mass of aluminium = 27.5g

mass of water = 55.5g

specific heat of aluminium = 0.900J/g °C

specific heat of water = 4.186 J/g °C

initial temperature of aluminium T1= 65.9 °C

initial temperature of water T1 = 22.1 °C

final temperature of water and aluminium = TO BE DETERMINED

<u>Step 3:</u> Calculate the initial temperature

To find the final temperature, we have to use the following formule:

-(Mass of aluminium) * (caluminium)*(ΔT)) = (Mass of water) *(cwater)*(ΔT)

-27.5g (0.900)(T2 - 65.9) = 55.5g (4.184j/g °C) (T2- 22.1)

-24.75*(T2-65.9) = 232.212 *(T2-22.1)

-24.75T2 + 1631.025 = 232.212T2 -5131,8852

-256.962 T2 = -6762.9102

T2 = 26.32 °C

The final temperature of aluminium ≈ 26.32 °C

6 0

3 years ago

what conclusion can be drawn from the statement that the element has a high ionization energy and a small atomic size?

nignag [31]

Answer: What conclusion can be drawn from the statement that an element has high ionization energy and small atomic size? The element is most likely from Group 1A or 2A and in period 1 or 2. Describe how the atomic radius of an element is related to metallic character.

Explanation:

3 0

3 years ago