Answer:
strength = 10⁻²/10⁻³ = 10 times more acidic
Explanation:
1. A solution with a pH of 9 has a pOH of
pH + pOH = 14 => pOH = 14 - pH = 14 - 9 = 5
2. Which is more acidic, a solution with a pH of 6 or a pH of 4?
pH of 4 => Higher [H⁺] = 10⁻⁴M vs pH of 6 => [H⁺] = 10⁻⁶M
3. How many times more acidic is a solution with a pH of 2 than a solution with a pH of 3?
soln with pH = 2 => [H⁺] = 10⁻²M
soln with pH = 3 => [H⁺] = 10⁻³M
strength = 10⁻²/10⁻³ = 10 times more acidic
4. What is the hydrogen ion concentration [H + ] in a solution that has a pH of 8?
[H⁺] = 10^-pH = 10⁻⁸M
5. A solution has a pOH of 9.6. What is the pH? (Use the formula.)
pH + pOH = 14 => pH = 14 - 9.6 = 4.4
Answer:
a. The specific heat capacity of the gaseous ethanol is less than the specific heat capacity of liquid ethanol.
Explanation:
The heating curve is a curve that represents temperature (T) in the y-axis vs. added heat (Q) in the x-axis. The slope is T/Q = 1/C, where C is the heat capacity. Then, the higher the slope, the lower the heat capacity. For a constant mass, it can also represent the specific heat capacity (c).
Heats of vaporization and fusion cannot be calculated from these sections of the heating curve.
<em>Which statement below explains that?</em>
<em>a. The specific heat capacity of the gaseous ethanol is less than the specific heat capacity of liquid ethanol.</em> YES.
<em>b. The specific heat capacity of the gaseous ethanol is greater than the specific heat capacity of liquid ethanol.</em> NO.
<em>c. The heat of vaporization of ethanol is less than the heat of fusion of ethanol.</em> NO.
<em>d. The heat of vaporization of ethanol is greater than the heat of fusion of ethanol.</em> NO.
Did u mean mass of potassium nitrate or the mass of nitrogen in potassium nitrate
I believe the answer is D.
Answer:
<span>Chlorine (Cl) is the oxidizing agent because it gains an electron.
Explanation:
Reaction is as follow,
</span><span> Cl</span>₂<span> (aq) + 2 Br</span>⁻<span> (aq) </span>→ <span> 2Cl(aq) + Br</span>₂ <span>(aq)
Oxidation Reaction:
2 Br</span>⁻ → Br₂ + 2 e⁻
Two atoms of Br⁻ (Bromide) looses two electrons to form Br₂ molecule. Hence it is oxidized and is acting as reducing agent.
Reduction Reaction:
Cl₂ + 2 e⁻ → 2 Cl⁻
One molecule of Cl₂ gains two electrons to form two chloride ions (Cl⁻). Therefore, it is reduced and has oxidized Br⁻, Hence, acting as a oxidizing agent.
