Answer:
An ionic bond is that in which an electron is trasferred to another atom. Atoms that are considered metals have a low electronegativity meaning they are less likely to gain any electrons. Atoms that are non-metals have a higher electronegativity and are more likey to gain electrons than lose electrons. When an electron is either lost or gained by another electron the atome becomes more stable. Atoms with a complete and balanced valence shell stay close together because of the Nucleus with its strong electromagnetic pull. The stronger the pull the more likely the atom will gain an electron. The weaker the pull the more likely it will lose an electron.
I would say 2. suspension. hope it helps.
Answer: An existing theory is modified so that it can explain both the old and new observations.
Explanation:
<u>Answer:</u> The boiling point of solution is 100.62°C
<u>Explanation:</u>
Elevation in boiling point is defined as the difference in the boiling point of solution and freezing point of pure solution.
The equation used to calculate elevation in boiling point follows:
![\Delta T_b=\text{Boiling point of solution}-\text{Boiling point of pure solution}](https://tex.z-dn.net/?f=%5CDelta%20T_b%3D%5Ctext%7BBoiling%20point%20of%20solution%7D-%5Ctext%7BBoiling%20point%20of%20pure%20solution%7D)
To calculate the elevation in boiling point, we use the equation:
![\Delta T_b=iK_bm](https://tex.z-dn.net/?f=%5CDelta%20T_b%3DiK_bm)
Or,
![\text{Boiling point of solution}-\text{Boiling point of pure solution}=i\times K_b\times \frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ in grams}}](https://tex.z-dn.net/?f=%5Ctext%7BBoiling%20point%20of%20solution%7D-%5Ctext%7BBoiling%20point%20of%20pure%20solution%7D%3Di%5Ctimes%20K_b%5Ctimes%20%5Cfrac%7Bm_%7Bsolute%7D%5Ctimes%201000%7D%7BM_%7Bsolute%7D%5Ctimes%20W_%7Bsolvent%7D%5Ctext%7B%20in%20grams%7D%7D)
where,
Boiling point of pure water = 100°C
i = Vant hoff factor = 1 (For non-electrolytes)
= molal boiling point elevation constant = 0.512°C/m.g
= Given mass of solute = 23.6 g
= Molar mass of solute = 103.5 g/mol
= Mass of solvent (water) = 188 g
Putting values in above equation, we get:
![\text{Boiling point of solution}-100=1\times 0.512^oC/m\times \frac{23.6\times 1000}{103.5g/mol\times 188}\\\\\text{Boiling point of solution}=100.62^oC](https://tex.z-dn.net/?f=%5Ctext%7BBoiling%20point%20of%20solution%7D-100%3D1%5Ctimes%200.512%5EoC%2Fm%5Ctimes%20%5Cfrac%7B23.6%5Ctimes%201000%7D%7B103.5g%2Fmol%5Ctimes%20188%7D%5C%5C%5C%5C%5Ctext%7BBoiling%20point%20of%20solution%7D%3D100.62%5EoC)
Hence, the boiling point of solution is 100.62°C
Answer:
0.868M Cu⁺
Explanation:
The reaction is:
KMnO₄ + 5Cu⁺ + 8H⁺ → 5Cu²⁺ + Mn²⁺ + K⁺ + 4H₂O
<em>Where 1 mol of KMnO₄ reacts with 5 moles of Cu⁺</em>
<em />
3.30x10⁻²L of 0.132M KMnO₄ are:
3.30x10⁻²L × (0.132mol KMnO₄ / L) = <em>4.356x10⁻³mol KMnO₄</em>
As 1 mol reacts with 5 moles of Cu⁺, moles of Cu⁺ are:
4.356x10⁻³mol KMnO₄ × (5mol Cu⁺ / 1mol KMnO₄) = <em>0.02178moles Cu⁺</em>
As these moles are in 2.51x10⁻²L, the starting concentration of the Cu⁺ solution is:
<em>0.02178moles Cu⁺ / </em>2.51x10⁻²L = <em>0.868M Cu⁺</em>