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3 years ago

How do the isotopes hydrogen-1 and hydrogen-2 differ?

Chemistry

2 answers:

g100num [7]3 years ago

4 0

Hydrogen-2 has one neutron; hydrogen-1 has none

galina1969 [7]3 years ago

3 0

Answer: They differ by the number of neutrons

Explanation:

Isotopes are defined as the chemical species which have same number of protons but differ in the number of neutrons.

The general isotopic representation is $_{Z}^A\textrm{X}$

where,

Z = Atomic number of the atom

A = Mass number of the atom

X = Symbol of the atom

Atomic number is defined as the number of protons or electrons that are present in a neutral atom.

Atomic number = number of protons = number of electrons

Mass number is defined as the sum of number of protons and number of neutrons present in an atom.

Mass number = Number of neutrons + Number of protons.

We are given two isotopes:

$_1^1\textrm{H}\text{ and }_1^2\textrm{H}$

For $_1^1\textrm{H}$ isotope:

Number of protons = 1

Mass number = 1

Number of neutrons = 1 - 1 = 0

For $_1^2\textrm{H}$ isotope:

Number of protons = 1

Mass number = 2

Number of neutrons = 2 - 1 = 1

Hence, they differ by the number of neutrons

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3 years ago

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2 years ago

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14. What is the pH of a 0.24 M solution of sodium propionate, NaC3H502, at 25°C? (For

Murrr4er [49]

Answer:

9.1

Explanation:

Step 1: Calculate the basic dissociation constant of propionate ion (Kb)

Sodium propionate is a strong electrolyte that dissociates according to the following equation.

NaC₃H₅O₂ ⇒ Na⁺ + C₃H₅O₂⁻

Propionate is the conjugate base of propionic acid according to the following equation.

C₃H₅O₂⁻ + H₂O ⇄ HC₃H₅O₂ + OH⁻

We can calculate Kb for propionate using the following expression.

Ka × Kb = Kw

Kb = Kw/Ka = 1.0 × 10⁻¹⁴/1.3 × 10⁻⁵ = 7.7 × 10⁻¹⁰

Step 2: Calculate the concentration of OH⁻

The concentration of the base (Cb) is 0.24 M. We can calculate [OH⁻] using the following expression.

[OH⁻] = √(Kb × Cb) = √(7.7 × 10⁻¹⁰ × 0.24) = 1.4 × 10⁻⁵ M

Step 3: Calculate the concentration of H⁺

We will use the following expression.

Kw = [H⁺] × [OH⁻]

[H⁺] = Kw/[OH⁻] = 1.0 × 10⁻¹⁴/1.4 × 10⁻⁵ = 7.1 × 10⁻¹⁰ M

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We will use the definition of pH.

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3 years ago

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Orlov [11]

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3 years ago

What is the volume of 0.20 moles of helium at STP?

stealth61 [152]

The volume of 0.20 moles of helium at STP is 4.5 liters.

Explanation:

Given:

Number of moles = 0.20 moles

To Find:

The volume of Helium at STP =?

Solution:

According to ideal gas law

PV = nRT

where

P is pressure,

V is volume,

n is the number of moles

R is the gas constant, and

T is temperature in Kelvin.

The question already gives us the values for p and T ,because helium is at STP. This means that temperature is 273.15 K and pressure is 1 atm .

We also already know the gas constant. In our case, we'll use the value of

0.08206 L atm/K mol since these units fit the units of our given values the best

On substituting these values we get

$1 atm \times V = 0.20 moles \times 0.08206 L atm/K mol$

$V = \frac{0.20 moles \times 0.08206 L atm/K mol }{ 1 atm}$

$V = \frac{4.482}{1}$

V = 4.5 Liters

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3 years ago