negatively
Positively
Neutrally
Explanation:
An object that is negatively charged has more electrons than protons.
An object that is positively charged has fewer electrons than protons.
An object that is neutrally charged has the same number of electrons and protons.
The subatomic particles in an atom are protons, neutrons and electrons.
Protons are the positively charged particles in an atom
Electrons are the negatively charged particles in an atom
Neutrons do not carry any charges.
When an atom is neutral, it has equal number of protons and electrons.
When an atom forms a cation, the number of protons is greater than electrons and it suggest that it has lost electron. This is therefore positively charged.
When an atom forms an anion, the number of electrons is greater than the number of protons. It suggests that it has gained electrons. This is therefore negatively charged.
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Explanation:
It is known that relation between 
, 
, and pH is as follows.
![E_{cell} = E^{o}_{cell} - (\frac{0.0591}{n}) \times log[H^{+}] ](https://tex.z-dn.net/?f=E_%7Bcell%7D%20%3D%20E%5E%7Bo%7D_%7Bcell%7D%20-%20%28%5Cfrac%7B0.0591%7D%7Bn%7D%29%20%5Ctimes%20log%5BH%5E%7B%2B%7D%5D%0A)
Also, it is known that for hydrogen is equal to zero.
Hence, substituting the given values into the above equation as follows.
0.238 V = 0 - (\frac{0.0591}{1}) \times log[H^{+}]
[/tex]
![-log[H^{+}]](https://tex.z-dn.net/?f=-log%5BH%5E%7B%2B%7D%5D)
= 4.03
![[H^{+}]](https://tex.z-dn.net/?f=%5BH%5E%7B%2B%7D%5D)
= antilog 4.03
= 3.5
As, pH = .
Thus, we can conclude that pH of the given unknown solution at 298 K is 3.5.
<span>covalent. When two atoms share valence electrons, such a type of a bond is called a covalent bond. An example of such a bond could be the H2 molecule, where two H (hydrogen) atoms share electrons in a covalent bond.</span>
What exactly is this asking
Answer:
33.8 m
Explanation:
(a) We want to know the molality of nitric acid in a concentrated solution of nitric acid (68.0% HNO₃ by mass).
Step 1: Determine the mass of HNO₃ and water in 100 grams of solution.
Step 2: Convert the mass of HNO₃ to moles.
Step 3: Convert the mass of water to kilograms.
Step 4: Calculate the molality.
(b)
Step 1
In 100 g of solution, there are 68.0 g of HNO₃ and 100 g - 68.0 g = 32.0 g of water.
Step 2
The molar mass of HNO₃ is 63.01 g/mol. The moles corresponding to 68.0 g are:
68.0 g × (1 mol/63.01 g) = 1.08 mol
Step 3
The mass of water is 32.0 g = 0.0320 kg
Step 4
The molality of HNO₃ is:
m = moles of solute / kilograms of solvent
m = 1.08 mol / 0.0320 kg
m = 33.8 m
