Explanation:
Ionic bonds
Covalent bond
Vanderwaal force of attraction
Answer:
pH change is -0.07
Explanation:
Using H-H equation for acetic acid:
pH = pKa + log [Acetate salt] / [Acetic acid]
Replacing:
pH = 4.74 + log[1.188M] / [1.188M]
pH = 4.74
The HCl reacts with sodium acetate producing acetic acid, thus:
HCl + CH₃COONa → CH₃COOH + NaCl
That means the final moles of sodium acetate are initial moles - moles of HCl and moles of acetic acid are initial moles + moles of HCl.
As the volume of the buffer is 1.0L, initial moles of both substances are 1.188moles. After reaction, the moles are:
sodium acetate: 1.188mol - 0.1mol = 1.088mol
Acetic acid: 1.188mol + 0.1mol = 1.288mol
Using again H-H equation:
pH = 4.74 + log[1.088M] / [1.288M]
pH = 4.67
pH change is: 4.67 - 4.74 = -0.07
Answer:
6.28 L
Explanation:
Given data:
Volume of NO₂ = ?
Mass of NO₂ = 12.9 g
Temperature and pressure = ?
Solution:
First of all we will calculate the number of moles of gas.
Number of moles = mass/molar mass
Number of moles = 12.9 g/ 46 g/mol
Number of moles = 0.28 mol
At standard temperature and pressure 1 mole of gas occupy 22.4 L volume.
Thus,
0.28 mol × 22.4 L/1 mol
6.27 L ≅ 6.28 L
Answer: 8.7 grams
Explanation:
According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number 
of particles.
To calculate the moles, we use the equation:
As oxygen is in excess, Aluminium is the limiting reagent and limits the formation of products.
According to stoichiometry:
4 moles of aluminium give = 2 moles of 
Thus 0.17 moles of aluminium give=
Mass of 
Thus the mass of is 8.7 grams
