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2 years ago

H+ ion concentration of 2.5 x 10-5

Chemistry

1 answer:

gladu [14]2 years ago

5 0

Answer:

What is the hydrogen ion concentration of a solution labeled "Solution A", whose pH is 5.60?

Tutorial

In this problem we are given pH and asked to solve for the hydrogen ion concentration. Using the equation, pH = − log [H+] , we can solve for [H+] as,

− pH = log [H+] ,

[H+] = 10−pH,

by exponentiating both sides with base 10 to "undo" the common logarithm. The hydrogen ion concentration of "Solution A" is,

[H+] = 10−5.6 ≈ 0.0000025 = 2.51 × 10−6 M.

We can always check our solution by computing −log (2.5 × 10−6) ≈ 5.6.

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The Intermolecular force is a type of force which exists between particles in an Ideal gas.

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Intermolecular forces are considered weaker attractions that hold molecules in gas close together. This force of attraction is present between molecules or particles.

So we can conclude that the Intermolecular force is a type of force which exists between particles in an Ideal gas.

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1 year ago

Does water evaporate ant any temprature

natka813 [3]

Answer:

Explanation:

I'm not educated enough on the matter but from what I've been taught water boils at 100 Celsius and it simultaneously evaporates.

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1 year ago

When 231. mg of a certain molecular compound X are dissolved in 65. g of benzene (CH), the freezing point of the solution is mea

Elan Coil [88]

Answer:

Molar mass X = 18.2 g/mol

Explanation:

Step 1: Data given

Mass of compound X = 231 mg = 0.231 grams

Mass of benzene = 65.0 grams

The freezing point of the solution is measured to be 4.5 °C.

Freezing point of pure benzene = 5.5 °C

The freezing point constant for benzene is 5.12 °C/m

Step 2: Calculate molality

ΔT = i*Kf*m

⇒ΔT = the freezing point depression = 5.5 °C - 4.5 °C = 1.0 °C

⇒i = the Van't hoff factor = 1

⇒Kf = the freezing point depression constant for benzene = 5.12 °C/m

⇒m = the molality = moles X / mass benzene

m = 1.0 / 5.12 °C/m

m = 0.1953 molal

Step 3: Calculate moles X

Moles X = molality * mass benzene

Moles X = 0.1953 molal * 0.065 kg

Moles X = 0.0127 moles

Step 4: Calculate molar mass X

Molar mass X = mass / moles

Molar mass X = 0.231 grams / 0.0127 moles

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2 years ago

Balance the equation below for the reaction between hydrogen and chlorine, using the smallest whole-number

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1, 1, 2 (coefficients)

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2 years ago

Select all steps below that you followed to practice laboratory safety during the experiment. used tongs or a test tube holder t

uysha [10]

Explanation:

Steps followed to practice laboratory safety during the experiment are as follows.

Used tongs or a test tube holder to hold materials over the Bunsen burner flame.
Wore gloves and goggles.
Made careful observations of the products and reactants.
Did not smell the gases produced.

When we heat a test tube over bunsen flame then the tube gets hot and when we hold it with bare hands then out hands will burn. Therefore, it is advised to hold test tube with the help of tongs or a holder so that our hands did not burn.

We should also wear gloves and goggles so that any acid would not spill directly on our hands, skin and eyes as it can affect or damage the skin severely.

Careful observations were made so that correct calculations about the experiment can be carried out.

It is also advised that we should not smell the gases produced but gases move freely from one place to another in a laboratory or any where else.

So, we can try to avoid it by covering our mouth with a cloth but we cannot stop it. If we keep on inhaling the gases produced in a laboratory then it can also lead to severe disease or defect in the human body.

8 0

2 years ago

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