1.08 atm is the pressure for a certain tire in atmosphere.
<u>Explanation:</u>
One kilo pascal (1 kPa) corresponds to 1000 pascal. Another common unit used for pressure is atmosphere (symbolised as ‘atm’). 1 atm refers the standard atmospheric pressures and corresponds to 760 mm Hg and 101.3 kPa. Atmospheric pressures are commonly referred as square inches (psi)/ pounds.
Given:
The air pressure for a certain tire = 109 kPa
We need to find pressure in atmospheres
So, we know,
1 atm = 101.3 kPa
Hence,
1.08 atm is the pressure for a certain tire in atmosphere.
Answer:
4.4 g
Explanation:
The equation of the reaction is;
NaHCO3 (aq) + CH3COOH (aq) ----> CO2 (g) + H2O (l) + CH3COONa (aq)
Mass of baking soda - 4.5 g
Molar mass of NaHCO3 = 84.007 g/mol
Number of moles of baking soda= 4.5 g/84.007 g/mol = 0.0536 moles
If 1 mole of NaHCO3 yields 1 mole of CH3COONa
0.0536 moles of NaHCO3 also yields 0.0536 moles moles of CH3COONa
Hence;
Theoretical yield of CH3COONa = 0.0536 moles * 82.0343 g/mol = 4.4 g
Answer:
Determine the pH of the solution half-way to the end-point on the pH titration curve for acetic acid.
Explanation:
The equation for the ionization of acetic acid is
HA + H₂O ⇌ H₃O⁺ + A⁻
For points between the starting and equivalence points, the pH is given by the Henderson-Hasselbalch equation:
![\text{pH} = \text{pK}_{\text{a}} + \log\dfrac{[\text{A}^{-}]}{\text{[HA]}}](https://tex.z-dn.net/?f=%5Ctext%7BpH%7D%20%3D%20%5Ctext%7BpK%7D_%7B%5Ctext%7Ba%7D%7D%20%2B%20%5Clog%5Cdfrac%7B%5B%5Ctext%7BA%7D%5E%7B-%7D%5D%7D%7B%5Ctext%7B%5BHA%5D%7D%7D)
At the half-way point, half of the HA has been converted to A⁻, so [HA] = [A⁻]. Then,
The pKₐ is the pH at the half-way point in the titration.
The correct answer is B. The concentration of a solution does not decreases when you add more solute to the solvent. Instead, the concentration increases. Concentration is expressed as the amount of solute per unit of solvent. Therefore, increasing the solute, increases this value and increasing the solvent, decreases this value.
